Protocols in Biochemistry and Clinical Biochemistry 1st Edition Buddhi Prakash Jain Shyamal K Goswami Shweta Pandey
Protocols in Biochemistry and Clinical Biochemistry 1st Edition Buddhi Prakash Jain Shyamal K Goswami Shweta Pandey
Protocols in Biochemistry and Clinical Biochemistry 1st Edition Buddhi Prakash Jain Shyamal K Goswami Shweta Pandey
https://ebookmeta.com/product/concepts-and-cases-in-biochemistry-
as-per-the-revised-competency-1st-edition-binita-goswami/
https://ebookmeta.com/product/clinical-case-discussion-in-
biochemistry-1st-edition-poonam-agrawal/
https://ebookmeta.com/product/marks-basic-medical-biochemistry-a-
clinical-approach-5th-edition-michael-lieberman/
https://ebookmeta.com/product/practical-biochemistry-with-
clinical-correlation-for-mbbs-students-1st-edition-poonam-
agrawal/
Terpenoids Chemistry Biochemistry Medical Effects Ethno
pharmacology Bimal K. Banik
https://ebookmeta.com/product/terpenoids-chemistry-biochemistry-
medical-effects-ethno-pharmacology-bimal-k-banik/
https://ebookmeta.com/product/marks-basic-medical-biochemistry-a-
clinical-approach-6th-edition-michael-a-lieberman/
https://ebookmeta.com/product/physeo-biochemistry-1st-edition-
physeo-com/
https://ebookmeta.com/product/biochemistry-and-cell-biology-of-
ageing-part-iv-clinical-science-1st-edition-j-robin-harris/
https://ebookmeta.com/product/plant-biochemistry-caroline-
bowsher/
Protocols in
Biochemistry and
Clinical
Biochemistry
Protocols in
Biochemistry and
Clinical
Biochemistry
BUDDHI PRAKASH JAIN
Assistant Professor, Department of Zoology, School of Life Sciences, Mahatma Gandhi
Central University Bihar, Motihari, India
SHYAMAL K. GOSWAMI
Professor, School of Life Sciences, Jawaharlal Nehru University, New Delhi, India
SHWETA PANDEY
Govt VYT PG Autonomous College, Durg, Chhattisgarh, India
Academic Press is an imprint of Elsevier
125 London Wall, London EC2Y 5AS, United Kingdom
525 B Street, Suite 1650, San Diego, CA 92101, United States
50 Hampshire Street, 5th Floor, Cambridge, MA 02139, United States
The Boulevard, Langford Lane, Kidlington, Oxford OX5 1GB, United Kingdom
© 2021 Elsevier Inc. All rights reserved.
No part of this publication may be reproduced or transmitted in any form or by any means, electronic or
mechanical, including photocopying, recording, or any information storage and retrieval system, without
permission in writing from the publisher. Details on how to seek permission, further information about the
Publisher’s permissions policies and our arrangements with organizations such as the Copyright Clearance
Center and the Copyright Licensing Agency, can be found at our website: www.elsevier.com/permissions.
This book and the individual contributions contained in it are protected under copyright by the Publisher
(other than as may be noted herein).
Notices
Knowledge and best practice in this field are constantly changing. As new research and experience broaden our
understanding, changes in research methods, professional practices, or medical treatment may become
necessary.
Practitioners and researchers must always rely on their own experience and knowledge in evaluating and using
any information, methods, compounds, or experiments described herein. In using such information or
methods they should be mindful of their own safety and the safety of others, including parties for whom they
have a professional responsibility.
To the fullest extent of the law, neither the Publisher nor the authors, contributors, or editors, assume any
liability for any injury and/or damage to persons or property as a matter of products liability, negligence or
otherwise, or from any use or operation of any methods, products, instructions, or ideas contained in the
material herein.
Library of Congress Cataloging-in-Publication Data
A catalog record for this book is available from the Library of Congress
British Library Cataloguing-in-Publication Data
A catalogue record for this book is available from the British Library
ISBN 978-0-12-822007-8
1. Centrifugation
G ¼ ω2 r
2. Electrophoresis
3. Spectrophotometer or
4. Chromatography
4π 2 s2 r
5. Titration G¼
3600
The unit of G is cm/s.
CENTRIFUGATION Relative centrifugal force is
In biology, centrifugation is a technique that utilizes the G
centrifugal force for the separation of the biological con- RCF ¼
g
tents from the liquid medium. The separation of the
or
contents depends on their shape, size, density, and the
viscosity of the medium. Analytical centrifugation is 4π 2 s2 r
RCF ¼
used for the analysis of the purified macromolecules ð3600Þð981Þ
and was first developed by Svedberg in the late 1920s.
or
Preparative centrifugation deals with the actual separa-
tion of biological contents. RCF ¼ 1:12 105 s2 r
Application of preparative centrifugation: Subcellular
According to the Stokes’ law, when a particle moves
fractionation, affinity purification of membrane
through a viscous medium, it experiences a frictional
vesicles, etc.
force:
Application of analytical centrifugation: Determination
of the purity of macromolecules and their relative F ¼ 6πrp ηv
molecular mass, detection of changes in conforma-
where
tion, and ligand-binding studies.
η ¼ viscosity of the medium
The process utilizes the principle that a particle, in a
ν ¼ velocity of the particle
liquid medium, will sediment much faster when placed
rp ¼ radius of the particle
under the influence of centrifugal force. While moving
Also, when particle sediment, it feels an upward
through a viscous medium, they experience a frictional
force. This force will be equal to the weight of water
force. This force acts in the opposite direction to its
displaced.
sedimentation.
4
Relative centrifugal force: F ¼ πrp3 ρp ρm ω2 r
3
F ¼ Mω2 r
where
where ρp ¼density of the particle
M ¼mass of particle ρm ¼density of the medium
r ¼ radius of the rotor r ¼ distance of the particle from the medium
ω ¼ angular velocity rp ¼ radius of the particle
Angular velocity in rad/s: ω ¼ angular velocity
2π s A nonhydrated spherical particle will accelerate
ω¼ under centrifugal force till the net force of sedimenta-
60
tion becomes equal to the frictional force.
where
Or
s ¼ speed of the rotor (revolution/min)
ω ¼ angular velocity (rad/s) 4 3
πrp ρp ρm ω2 r ¼ 6πrp ηυ
Applied centrifugal force (G) is 3
vii
viii TECHNIQUES
Centrifugal force
Negative Positive
electrode − +
electrode
Buffer
Gel
where a is the absorptivity or absorption coefficient or 5. Fluorescence: Some solutes, especially drugs or their
extinction coefficient. intermediates fluoresce, and their fluorescent inten-
Specific absorption coefficient—when path length is sity are also detected by the spectrophotometer.
expressed in cm and concentration in g/L, then the Absorption spectrum—it is the pattern of energy
absorption coefficient is termed as a specific absorp- absorption by a substance, when, the light of varying
tion coefficient. wavelength passes through it. It is a unique characteristic
Molar absorption coefficient—when path length is of the substance as every substance is made up of mol-
expressed in cm and concentration in mol/L, then ecules and each element/ion of the molecule has unique
the absorption coefficient is termed as the molar arrangements of an electron in their orbits/orbitals.
absorption coefficient and is denoted as am. When light is passed through them, they absorb energy,
according to their electronic configuration and their
am ¼ as Mw ðmolecular weightÞ electrons get excited. These electrons get promoted to
a higher energy level. According to the quantum theory,
For a given compound, if the solvent and wavelength
the electron gets excited only after accepting the radia-
are defined, then molar absorptivity is a physical con-
tion, which has exact quantized energy that can push
stant. Molar absorptivity of some compounds are listed
the electron to a permitted energy level. The wavelength
as below:
at which it absorbs the maximum amount of light is
Compound Solvent λmax am × 1023 λmax. When the concentration of any substance is
Adenine Water 260 13.3 increased, the absorbance at all wavelength increases,
NADH Water 340 6.22 although the change in absorbance per unit change in
ATP Water 260 15.4 concentration is maximum at λmax. Therefore, during a
FAD Water 445 11.3 quantitative experiment, absorbance of a compound
is measured at λmax.
When a sample is placed in a cuvette and light is passed Factors that can affect the absorption spectra are
through it, we can calculate the concentration of the polarity (affect the transition states of the electrons)
sample. When path length is constant, then the optical and pH of the solvent (it can change the ionization state
density is directly proportional to the concentration of of the molecules) as well as the relative orientation of
the sample, it can be written as follows: the neighboring absorbing groups.
Some isolated covalently bonded groups characteris-
OD1 OD2
¼ tically absorb the light in esters, carbonyl, and nitrile
C1 C2
group of ethylenic or acetylenic groups. Similarly, there
where are auxochromes that themselves don’t act as chromo-
OD1 and OD2 ¼ optical density of sample 1 and 2, phores, but their absence or presence shifts the absorp-
respectively tion spectrum toward longer wavelengths. They are also
C1 and C2 ¼ concentration of samples 1 and 2, known as color enhancers, e.g., OH, OR, SH, NH2
respectively groups. They can share the nonbonding electrons by
Deviations from Beer-Lambert law: extending the conjugation.
1. When the concentration of the reagent is high: It may There are different conditions like change in the
lead to dimerization or polymerization of the reagent. polarity of the solvent or the presence of chromophore,
OD of monomer differs from polymers. High concen- etc., which can shift the absorption spectrum in four dif-
tration may also lead to aggregation leading to the for- ferent directions and result in the following shifts:
mation of aggregates, which scatter light. 1. Bathochromic shift: Due to the presence of auxo-
2. Temperature: On heating, the solvents may expand. chrome, the shift is toward the higher wavelength.
The change in the degree of solubility, dissociation/ This is also known as the redshift.
association of solutes, and hydration of solutes may 2. Hypochromic shift: The shift is toward shorter wave-
vary according to the temperature. These changes can length, due to the removal of conjugation or the
lead to variation in absorbance. change in the polarity of the solvent. This is also
3. Turbidity: A turbid solution absorbs more light. known as a blueshift.
4. Sample instability: Some colored complexes are 3. Hyperchromic shift: This results in an increase in the
unstable and their intensity can increase or decrease intensity of the absorption maximum. It results in a
with time. For example, the ANSA method of phos- higher extinction coefficient. This occurs mostly due
phate determination. to the presence of auxochrome.
xii TECHNIQUES
Body of
spectrophotometer
1 2 3 4
Lid
Slot for
Display unit cuvette
1 2 3
Absorbance of a solution depends on its concentration and path length: (a) As the absorbance depends on the
concentration, the absorbance of the tube 4 will be highest and that of the tube 1 will be lowest. (b) (a) As the
absorbance depends on the pathlength, the absorbance of the tube 3 will be highest and that of the tube 1 will be
lowest.
FIG. 3 Spectrophotometer.
4. Hypochromic shift: The shift of absorption maxi- The term partition coefficient or distribution coeffi-
mum to a lower value. It occurs due to the introduc- cient (Kd) is used to describe the mode of distribution
tion of the groups that is appropriate result in the of a compound between two immiscible phases. At a
distortion of the geometry of the absorbing molecule given temperature, when a sample is allowed to equili-
(Fig. 3). brate itself between two different liquids that are immis-
cible and are present in equal volumes, the ration in
which it does the distribution is known as partition coef-
ficient. It is the concentration of a component present in
CHROMATOGRAPHY one phase divided by that in another phase. It can be
The first account of chromatography was given by expressed as
Michael Tswett in 1906. In the experiment, chlorophyll
was separated from a mixture of plant pigments, the col- Concentration in phase A
Kd ¼
ored pigments and chlorophyll get separated forming Concentration in phase B
distinct colored bands. Hence, the term chromatogra- The effective distribution coefficient is the total amount
phy was given to the separation technique. It is a of the analyte in a phase divided its total amount in
method of separation of an analyte between two immis- another phase. It also considers the volume of the
cible phases. One of the phases remains stationary, phases, for example, if the distribution coefficient of
while the other is mobile. The mobile phase usually an analyte between A and B phases is 1, but the total vol-
moves over the surface of the stationary phase. It can ume of phase A is 5 times more than that of B, then the
also percolate through the interstices of the stationary effective distribution coefficient is of the analyte is 5. Its
phase. A sample is introduced in the system with the amount in phase A is 5 times more in A than B. In the
mobile phase and the components of the sample inter- technique, the stationary phase (immobilized) can be
act with two phases in a differential manner, depending solid, gel, liquid, or solid/liquid mixture, while the
on their properties. Each component migrates at a differ- mobile phase is liquid or gas (Fig. 4).
ent rate based on the rate of interactions between the
components of the sample and each of the phases. Types of Chromatographic Techniques
The component showing the least interaction with the Based on the nature of the support that is used to hold
mobile phase but strong interaction with the mobile the stationary phase, the techniques can be classified as
phase will migrate slowly. The separation is done by follows:
the virtue of the differential movement of the compo- 1. Plane chromatography: The following are the types
nents of the sample. of plane chromatography:
TECHNIQUES xiii
Support Support
Pin Pin
a. Paper chromatography: In this technique, the sup- In the case of an anion exchanger, the negatively
port for the stationary phase is paper, i.e., cellu- charged sample will interact with the stationary
lose. The separation is done by adsorption or phase, while the positively charged and neutral mol-
partition principle. ecules will elute first.
b. Thin-layer chromatography: In this technique, the 4. Molecular sieve chromatography: In this chromatog-
glass plate coated with a layer of silica (partition raphy, a gel consisting of porous beads is the support
principle), Kieselguhr, and alumina (adsorption medium. The molecules smaller than the pore size
principle). will get entrapped in the pore of the gel, while the
2. Column chromatography: In this, the stationary larger molecules will not and thus get eluted first.
phase is packed in a column of glass or metal. 5. Affinity chromatography: In this chromatography,
The mixture of analytes is applied to the column the specificity of an enzyme toward its substrate or
and the mobile phase passes through it. The substrate analogs. The technique utilizes the specific-
mobile phase is termed as eluent. The stationary ity of an enzyme for its substrate (also receptor for its
phase is coated on the matrix and packed in the agonist, the antibody for an antigen) or substrate
column or is applied on the walls of the column. analog for the enzyme’s (other proteins with biolog-
The eluent flows through the column and separates ical specificity) separation. A substrate analog is
the sample according to the partition coefficient of coupled to the gel matrix and the cellular suspension
the components in the sample. The components can percolate through. The enzyme which is specific
that leave the column individually are termed as for the substrate analog binds to the gel becoming
an eluate. immobile, while all other components move down
Based on the interaction phenomenon between sta- and out. The technique has a very high-
tionary and mobile phase, the technique can be classi- resolution power.
fied in the following types:
1. Partition chromatography: In this, the separation
involves a large number of partition steps on the TITRATION
granules of an insoluble hydrated inert substance, It is a method to determine the concentration of an
e.g., silica gel or starch. The granules are hydrated identified analyte. It is a volumetric analysis, i.e., a
and hold water in a very tightly bound manner. method in which the amount of a solution is deter-
Hence, water is the stationary phase. mined by measuring its volume. In this process, a vol-
2. Adsorption chromatography: In this chromatogra- ume of a solution of known strength is added to
phy, the components are absorbed with the help of another solution to complete the reaction. There are a
weak electrostatic forces or hydrogen bonding on few important terms used in the procedure, which can
the surface of the stationary phase. be listed as below:
3. Ion exchange chromatography: In this chromatogra- 1. Titer: It is the weight of solution in 1 mL of solution
phy, an ion exchanger consisting of inert support or weight of a substance that will react with 1 mL of
covalently coupled with negative (cation exchanger) solution or is equivalent to 1 mL of solution.
or the positive (anion exchanger) functional group. 2. Standard solution: A solution of an accurately known
The support can exchange the charged functional concentration is known as the standard solution.
group with that of the components of the sample. They can be of two types—primary standard
xiv TECHNIQUES
The solution is a homogenous mixture of two or more But it is true if the conc. HCl is 100%, but in the bot-
components. Solutions that are made up of two compo- tle, the conc. HCl is 37.23%, so the volume needed is
nents are binary. The component in which something is 82.38 mL in 1 L of solution.
dissolved or, in other words, the component which is in
larger quantity is known as a solvent; the component
which is dissolved or, in other words, which is present MOLALITY (M)
in smaller quantity is the solute. A solution containing 1 mol of solute in 1 kg of a solvent
is known as 1 molal solution.
Solute + Solvent ¼ Solution
No:of moles of solute
Each component may be in any state, i.e., solid, liquid, Molality ¼
Weight of solvent in kg
or gaseous state. The strength of any solution is very
important in doing any experiment and it has to be For example,
made cautiously. The strength of a solution can be To prepare 1 m solution of NaOH in water, we need
defined as the amount of solute dissolved per unit solu- 1 mol of NaOH in 1000 g of water.
tion or solvent. It can be expressed in various terms. As specific gravity of water is 1,
1 g water ¼ 1 mL of water.
1 mol of NaOH ¼ 40 g of NaOH.
MOLARITY (M) Now, if we add 40 g of NaOH in 1000 mL of water, it
It is the most common way to represent the strength of will result in a 1 M solution of NaOH in water.
any solution. It is defined as the no. of moles of a solute Note that molarity refers the total volume of solution
per liter of the solution. (solvent + solute) whereas molality refers the weight of
the solvent.
No:of moles of solute
Molarity ¼
Volume of the solution in liters
For example, NORMALITY
To prepare a solution of 2 M NaOH in 100 mL of It is the number of gram equivalents of the solute that
solution, we need 2 M of NaOH dissolved in 100 mL has been dissolved in 1 L of solution. Gram equivalent
of the solution. or equivalent weight of a given substance is the mass
1 mol NaOH ¼40 g of NaOH of a substance that combines with or displaces a fixed
2 mol NaOH ¼80 g of NaOH quantity of other substances. This can be defined as
Now, if in 1000 mL of solution, 80 g of NaOH is dis- the following:
solved then 2 M solution could be obtained. 1. For an element the mass of the element that com-
For 100 mL of solution, 8 g of NaOH is needed. bines with/displaces 1.008 g of hydrogen, 8.0 g of
But in case of liquid it differs as here density comes oxygen, or 35.5 g of chlorine. It can be obtained by
into play: dividing the atomic weight of an element by its
Preparation of 1 M HCl: valency.
MW of HCl is 36.5 g. 2. For acids and bases, it is the mass of acid or base that
So, if 36.5 g of HCl is dissolved in 1 L of solution then provides or reacts with 1 mol of H+.
1 M HCl could be obtained. The unit of equivalent weight is g.
The specific gravity of HCl is 1.19, which means, For example, in the case of NaCl: anion is Na+ and
1 mL of HCl weigh 1.19 g. cation is Cl. The total charge on anion or cation is 1.
So, the volume needed is mass/specific gravity or So, the equivalent weight is (23 +35.5)/1 ¼ 58.5.
36.5/1.19. In the case of Al2(SO4)3: anion is two molecules of
The volume of HCl needed is 30.67 mL. Al3+ and cation is three molecules of (SO4)2.
Ka + Kb ¼ Kw ½unionized form
pH ¼ pKa + log
½ionized form
where Ka and Kb are equilibrium constant of acid and
base, respectively. Buffering capacity is the ability of a buffer to resist a
For example, in the case of acetic acid (CH3COOH) change in pH when an acid or base is added to it. It is
denoted as β and can be defined as the moles of acid
CH3 COOH Ð CH3 COO + H + or base which is required to change the pH of the buffer
and by one unit.
½CH3 COO ½H + ½conjugated base½H db da
Ka ¼ ¼ β¼ ¼
½CH3 COOH ½weak acid dpH dpH
5
¼ 1:75 10 and its pKa is 4:75 where db and da are the amount (moles) of base and
Further, acid, respectively, and dpH is the change in pH.
Ka Kb ¼ ½H + ½OH ¼ Kw ¼ 1 1014 HA Ð H + + A
and ½H + ½Cl
Ka ¼ ¼ 1:75 105
pKa + pKb ¼ pKw ½HA
Stronger acid will have a smaller numerical value of pKa HA will dissociate to form equal amounts of ions H+
(and larger Ka) than a weaker acid. The smaller the pKa and Cl.
value, the more it will be in ionized form. Let x be the amount of H+ forms. Then Cl will be x
and HA will be 0.01 x M.
Buffer ½x½x
1:75 105 ¼
A solution that resists change in its pH, upon the addi- ½0:01 x
tion of acid or base, is known as a buffer solution.
Mostly they are weak electrolytes, due to this their ionic 1:75 107 1:75 105 x ¼ x2
status varies with pH. In an aqueous solution, they are In this equation we can neglect x as its value is very
either a mixture of a weak acid with its conjugate base small, so the above equation can be written as
or a weak base with its conjugate acid. For the prepara-
tion of buffer solution or to estimate its pH Henderson- 1:75 107 ¼ x2
4 Protocols in Biochemistry and Clinical Biochemistry
Carbohydrate
A. Qualitative test for carbohydrates 19. Extraction and analysis of soluble carbohydrates
1. Determination of the presence of carbohydrates from plants.
in the given sample by Molisch’s test.
2. Determination of the presence of reducing carbo- QUALITATIVE TEST FOR CARBOHYDRATES
hydrates in the given sample by picric acid test. Definition
3. Determination of the presence of reducing car- Determination of the presence of carbohydrates in the
bohydrates in the given sample by Fehling’s test. given sample by Molisch’s test.
4. Determination of the presence of reducing carbo-
hydrates in the given sample by Benedict’s test.
Rationale
5. Determination of the presence of reducing carbo-
All types of carbohydrates—monosaccharides (except
hydrates in the given sample by Tommer’s test.
triose and tetrose), disaccharides, and
6. Determination of the presence of reducing car-
polysaccharides—get dehydrated upon treatment with
bohydrates in the given sample by
conc. sulfuric acid or hydrochloric acid and produce
Nylander’s test.
an aldehyde. This aldehyde condenses with two mole-
7. Distinguish between monosaccharides and
cules of α-naphthol to form a purple-colored ring.
reducing disaccharides by Barfoed’s test.
8. Distinguish between aldose and ketose by conc:H2 SO4 or HCl
Pentose sugar ! Furfural
Seliwanoff’s test.
conc:H2 SO4 or HCl
9. Determination of pentose sugar by Bial’s test. Hexose sugar ! 5 Hydroxymethylfurfural
10. Determination of the presence of galactose in a
Both aldehydes (furfural and 5-hydroxymethylfurfural)
test sample by the Mucic acid test.
condense with Molisch’s reagent (10% α-naphthol in
11. Differentiation between the presence of keto-
ethanol). Other phenols such as thymol and resorcinol
hexose and aldohexose in the test sample by
also give a colored product. This test results in the
Foulger’s test.
purple-colored product by all carbohydrates that are
12. Determination of the presence of reducing car-
larger than tetrose. Nucleic acid and glycoproteins too
bohydrates in the given sample by Fearon’s
give a positive test. In this test, oligosaccharides or poly-
methylamine test.
saccharides hydrolyzed to form monosaccharides,
13. Confirmation of the presence of reducing carbo-
which ultimately react as above.
hydrates in the given sample by osazone
formation test. Molisch’s reagent
Furfural=5 hydroxymethylfurfural ! Purple
14. Determination of the presence of polysaccha- colored dye
rides in the given sample by iodine test.
B. Quantitative test for carbohydrates
15. Quantitative estimation of carbohydrates in the Materials, equipment, and reagents
given sample by anthrone test. A. Reagents: Molisch’s reagent (10% α-naphthol in eth-
16. Quantitative estimation of reducing carbohy- anol), test sample (sugar solution), concentrated
drates in the given sample by 3,5-dinitro salicylic H2SO4.
acid (DNSA) test. B. Glassware: Test tube, test tube holder, dropper.
C. Other tests for carbohydrates
17. Extraction and estimation of glycogen from the Protocol
liver and muscle of the well-fed and starved rat. 1. Take 2 mL of the sample solution in a test tube.
18. Separation and identification of sugars present 2. To this add 2–3 drops of Molisch’s solution.
in fruit juices using thin-layer chromatography 3. Add 1 mL of conc. H2SO4 or HCl along the sides of
(TLC). the test tube, so that two layers are formed.
MOLISCH TEST
Purple ring
Acid
along the
Molisch side of Positive
solution test tube Molisch test
Sample
+
NaOH
Sample +
Sample + Acid
Molisch
Negative
Molisch test
CHAPTER 2 Carbohydrate 7
The sugars which have a free aldehyde or ketone group, Safety considerations and standards
in other words if the aldose C1 and ketose C2 are not 1. Picric acid is a highly acidic solution with pH 2 and
involved in any bond formation, are known as reducing hence should be handled very carefully.
sugars. The free aldehyde or ketone group enables them
to work as reducing agents. All monosaccharides are
reducing sugars while disaccharides can be classified Pros and cons
as reducing or nonreducing.
Picric acid is reduced under the alkaline condition in Pros Cons
the presence of reducing sugar. This results in the change Easy and sensitive Indicates the presence of reducing
of color of the solution from yellow to red. experiment sugars only
r
olo
dc
Sodium Mix and Re Positive Picric
Picric acid carbonate heat acid test
No
Sample co
lo
+ rc
ha
Picric ng
Sample acid e
+ +
Sample
Picric Sodium
acid carbonate
Negative Picric
acid test
Rationale Reduction
Reducing sugars get oxidized to acids and the cupric ion 4
+2 +1
gets reduced to cuprous ions, resulting in red- colored Cu ðC4 H3 O6 Þ2 + 2OH + 2e ! 2 Cu OH + 4C4 H3 O6 2
precipitate.
The copper ions of Fehling’s I solution result in its This is followed by the dehydration of copper(I) hydrox-
blue color as they exist in [Cu(H2O)4]2+ or [Cu ide and red precipitate of copper(I) oxide is formed.
(H2O)6]2+ in the aqueous solution. Upon the addition +1
2 Cu OH ! Cu2+1 O # + H2 O
of Fehling’s solution II, copper reacts with tartrate ions
and the solution becomes dark blue. The aldehyde/ketone group is oxidized to acid:
2 +
CuðH2 OÞ4 + 2C4 H4 O6 2 + 2OH RCHO + 2OH ! RCOOH + H2 O + 2e
CopperðaqÞ ðTartrate ionÞ
4 This is followed by deprotonation of carboxylic acid:
! CuðC4 H3 O6 Þ2 + 6H2 O
Copper complexed with tartrate ions RCOOH + OH ! RCOO + H2 O
CHAPTER 2 Carbohydrate 9
FEHLING TEST
Red ppt
Sample
+
Fehling
hling
Sample Solution A
+ +
Sample hling
Fehling
F
Fehling
ehling
hling
Solution A Solution B
Negative
Fehling test
Rationale
Benedict’s solution contains mild alkali Na2CO3. Upon Materials, equipment, and reagents
heating in the presence of alkali, reducing sugars are A. Reagents: Test sample (sugar solution), Benedict’s
converted into enediol. Enediols are alkenes with a reagent.
hydroxyl group on each carbon of C]C and are very B. Glassware: Test tube, test tube holder, dropper.
powerful reducing agents. The cupric ions (Cu2+) of C. Instrument: Water bath.
Benedict’s reagent get reduced to cuprous form (Cu+)
as cuprous oxide (which gets precipitated) by enediols.
Protocols
Reducing sugar + CuðcitrateÞ2 2 ! RCOO + Cu2 O # 1. Take 1 mL of test solution in a test tube.
Carboxylate ion Cuprous oxide
2. To this add 2 mL of Benedict’s solution.
In Benedict’s solution, copper sulfate furnishes cupric 3. Mix the above gently and keep in a water bath at 80°
ions, sodium carbonate makes the medium alkaline C for 5 min.
CHAPTER 2 Carbohydrate 11
Definition Summary
Distinguish between monosaccharides and reducing 1. The monosaccharides and reducing disaccharides
disaccharides by Barfoed’s test. reduce the cupric ions to red precipitate of copper.
CHAPTER 2 Carbohydrate 13
2. This test can even distinguish between monosaccha- Pros and cons
rides and reducing disaccharides as they take time to Pros Cons
produce a red color of copper. Easy and quick method
3. Disaccharides first get hydrolyzed in the acidic It can detect ketose sugars specifically
medium followed by their reaction with cupric
acetate. Summary
1. The test is for the differentiation of aldose from
Definition ketose sugars.
Distinguish between aldose and ketose by 2. Only ketose sugars get dehydrated in the presence of
Seliwanoff’s test. conc. acid.
3. The dehydrated ketose reacts with resorcinol to pro-
Rationale duce a deep cherry red color.
The test is named after the scientist, Theodor Seliwanoff,
who devised it. Polysaccharides and oligosaccharides Definition
ketose get hydrolyzed in the presence of concentrated Determination of pentose sugar by Bial’s test.
acids to yield simple sugar followed by furfural. The
dehydrated ketose reacts with resorcinol to produce a Rationale
deep cherry red-colored product. Aldose may react (at The test is named after the scientist, Manfred Bial. Pen-
a much slower rate) to form a faint pink-colored tose form furfural in acidic medium. This furfural con-
product. denses with orcinol in the presence of ferric ions to
form a blue-green-colored complex.
½H + 2 resorcinal
Ketose ! Furfural ! Deep cherry red color ½H + Orcinol, Fe3 +
Pentose sugar ! Furfural ! Blue green product
½H + Orcinol, Fe3 +
Materials, equipment, and reagents Hexose sugar ! Hydroxymethyl furfural ! Brown
A. Reagents: Test sample (sugar solution), Seliwanoff’s grey product
reagent.
In Bial’s reagent, hydrochloric acid provides the acidic
B. Glassware: Test tube, test tube holder, dropper.
medium, ferric chloride provides the Fe3+ ions, while
C. Instrument: Water bath.
orcinol condenses with furfural to form the resultant
blue-green-colored product. Hexose generally reacts to
Protocols
form brown-gray color product.
1. Take 1 mL of test solution in a test tube.
2. To this add 2 mL of Seliwanoff’s solution.
3. Mix the above gently and keep in a water bath at
Materials, equipment, and reagents
A. Reagents: Test sample (sugar solution), Bial’s
80–100°C for 1–3 min.
reagent.
B. Glassware: Test tube, test tube holder, dropper.
Analysis and statistics
C. Instrument: Water bath.
The formation of deep cherry red-colored precipitate
within 1–2 min indicates the presence of ketose. If it
takes a longer time for a faint pink-colored precipitate
Protocols
1. Take 2 mL of test solution in a test tube.
to form, then it indicates the presence of aldose.
2. To this add 2 mL of Bial’s solution.
3. Mix the above gently and keep it in a water bath at
Precursor techniques 80–100°C for 3–5 min.
1. Sugar solution: If sugar is in a powdered form add 1 g
of sugar to 100 mL of water. Analysis and statistics
2. Seliwanoff’s solution: Dissolve 0.05 mg of resorcinol The appearance of blue-green color indicates the pres-
in 100 mL of 3 N HCl. ence of pentose and that of brown-grey color indicates
the presence of hexose sugar.
Safety considerations and standards
1. Hydrochloric acid is corrosive and must be handled Precursor techniques
carefully. 1. Sugar solution: If sugar is in powdered form add 1 g
2. It is very necessary to keep track of time. of sugar to 100 mL of water.
14 Protocols in Biochemistry and Clinical Biochemistry
Analysis and statistics B. Glassware: Test tube, test tube holder, dropper.
The presence of ketohexose in the test solution is C. Instrument: Bunsen burner.
indicated by green-blue color, while the presence of
aldohexose results in yellow to olive green color. Protocols
(Although this test is used to distinguish between keto- 1. Take 1 mL of test solution in a test tube.
hexose and aldohexose; pentoses too react with the 2. To this add 2 mL of methylamine hydrochloride, fol-
reagent and yield yellow color.) lowed by the addition of 0.2 mL of sodium hydrox-
ide solution.
Precursor techniques 3. Mix the above gently and heat at 56°C for 30 min or
1. Sugar solution: If sugar is in powdered form add 1 g at 100°C for 5 min.
of sugar to 100 mL of water.
2. Foulger’s reagent: Add 40 g urea to 80 mL of 40% Analysis and statistics
H2SO4. To this add 2 g of stannous chloride and boil The appearance of red color in the solution indicates the
it vigorously till it becomes clear. Cool it and then presence of reducing sugar in the test sample.
make up the volume up to 100 mL by adding 40%
H2SO4. Precursor techniques
1. Sugar solution: If sugar is in powdered form add 1 g
Safety considerations and standards of sugar to 100 mL of water.
1. Sulfuric acid is corrosive and must be handled 2. Methylamine hydrochloride solution: Add 0.2 g of
carefully. methylamine hydrochloride (CH3NH2HCl) to
2. The process of boiling should be done carefully. 100 mL of water.
3. 10% sodium hydroxide solution: Add 10 g of NaOH
Pros and cons to 100 mL of distilled water.
Pros Cons
Easily distinguish between Other carbohydrates too Safety considerations and standards
aldohexose and ketohexose give similar color Methylamine hydrochloride can cause skin and eye irri-
tation; when inhaled can irritate the lungs, so it should
Summary be handled carefully.
1. The test is to distinguish between ketohexose and
aldohexose. Pros and cons
2. Both get dehydrated in the presence of conc. sulfuric Pros Cons
acid to hydroxymethylfurfural. But react with stan-
Easy and sensitive Indicates the presence of reducing
nous chloride to give different colored complexes.
experiment sugars only
Definition Alternative methods/procedures
Determination of the presence of reducing carbohy- Fehling’s test, Benedict’s test, Tommer’s test.
drates in the given sample by Fearon’s methylamine test.
Summary
Rationale 1. In this test, reducing sugars are treated with methyl-
Reducing carbohydrates undergo hydrolysis in alkaline amine hydrochloride in alkaline conditions.
conditions to form enediol. The enediol forms a red- 2. The sugars get hydrolyzed in the presence of alkali
colored product after reacting with methylamine hydro- and form enediol.
chloride. Enediols are alkenes with a hydroxyl group on 3. This enediol reacts with methylamine hydrochloride
each carbon of C]C and are very powerful reducing to form a colored product.
agents.
Alkaline solutions CH3 NH2 HCl Definition
Reducing sugar
! Enediol ! Red
Confirmation of the presence of reducing carbohydrates
colored product
in the given sample by osazone formation test.
detected under the microscope. Each sugar forms a char- Safety considerations and standards
acteristic crystal. Reducing sugars react with one molecule Be careful while handling the glacial acetic acid.
of phenylhydrazine hydrochloride to form phenylhydra-
zone hydrochloride, this again reacts with another mole- Pros and cons
cule of phenylhydrazine hydrochloride to give a keto Pros Cons
derivate. Finally, the keto derivative reacts with the third It is a confirmatory test for respective sugars None
molecule of phenylhydrazine hydrochloride.
Summary
Sugar + Phenylhydrazine hydrochloride 1. This is a confirmatory test for various reducing
! Sugar phenylhydrazone + H2 O sugars.
Sugar phenylhydrazone + 2ðphenylhydrazine hydrochlorideÞ 2. Each sugar reacts with an excess of phenylhydrazine
! Osazone + C6 H5 NH2 + NH3 + H2 O to form a characteristic crystal, which can be
observed under the microscope.
2. Iodine solution: Prepare 0.005 N iodine solution in Materials, equipment, and reagents
3% potassium iodide solution. To make this add A. Reagents: Anthrone reagent (0.2% anthrone in conc.
3 g of KI to 100 mL of the final solution in water fol- sulfuric acid), test sample (sugar solution), standard
lowed by the addition of 0.063 g of iodine to it. solutions.
B. Glassware: Test tube, test tube holder, dropper.
Safety considerations and standards C. Instruments: Water bath, colorimeter.
As glycogen and partially hydrolyzed starch give inter-
mediate color (reddish-brown), it should not be con- Protocol
fused with the yellowish-brown color of iodine- Preparation of standard curve:
potassium iodide. (A) Stock standard (1 mg/mL of glucose):
Weigh 100 mg of glucose and add 100 mL of
Pros and cons distilled water to it.
Pros Cons (B) Working standard (0.1 mg/mL of glucose):
Dilute 10 mL of stock solution to a final volume of
Used for distinguishing the It cannot be performed at a
presence of very low pH, as it results in 100 mL by adding distilled water to it.
polysaccharides hydrolysis of 1. Take six test tubes and label them.
polysaccharides 2. To these add 0–1mL of working standard solution
Increased temperature and and add water to make the final volume to 1 mL.
presence of organic 3. Simultaneously, take 1 mL of the sample solu-
solvents decrease the tion in another test tube.
intensity of the resultant 4. Add 4 mL of anthrone reagent, mix well, and
color cover each of the test tubes.
5. Put the tubes in a boiling water bath for 10 min.
Summary
6. Cool the test tubes to room temperature.
1. This test can distinguish between starch and
7. Measure the optical density at 620 nm.
glycogen.
8. Subtract the value of the absorbance of blank
2. Polysaccharides react with an iodine solution to
from the absorbance value for each of the test
form a unique color.
tubes.
9. Plot the standard calibration curve with concen-
QUANTITATIVE TEST FOR
tration plotted on the X-axis and optical density
CARBOHYDRATES
on the Y-axis.
Definition
Quantitative estimation of carbohydrates in the given
Test Tube Test
sample by anthrone test.
No. Blank 1 2 3 4 5 Sample
Working 0 0.2 0.4 0.6 0.8 1.0 1.0
Rationale solution
All types of carbohydrates, monosaccharides (except tri- (mL)
ose and tetrose), disaccharides, and polysaccharides, get Water added 1 0.8 0.6 0.4 0.2 0 0
dehydrated upon treatment with conc. sulfuric acid or (mL)
hydrochloric acid and produce aldehydes. This alde- Anthrone 4 4 4 4 4 4 4
reagent
hyde reacts with anthrone to yield a bluish-green- Heat in boiling water bath for 10 min. Cool it to room temperature
colored complex. OD at A0 A1 A2 A3 A4 A5 AT
620 nm
conc:H2 SO4 or HCl
Pentose sugar ! Furfural Final OD A0 A1–A0 A2–A0 A3–A0 A4–A0 A5–A0 AT–A0
conc:H2 SO4 or HCl
Hexose sugar ! 5 Hydroxymethylfurfural
Analysis and statistics
Calculate the concentration of the test sample corre-
Both the aldehydes (furfural and 5-hydroxymethylfurfural)
sponding to the optical density obtained, using the lin-
condense with anthrone reagent (10% α-naphthol in etha-
ear standard graph.
nol). This test results in a bluish-green-colored product by
all carbohydrates, which are larger than tetrose.
Precursor techniques
Anthrone reagent
Furfural=5 hydroxymethylfurfural
! Bluish 1. Anthrone reagent: Add 0.2 g of anthrone reagent to
green colored product 100 mL of conc. sulfuric acid (H2SO4).
18 Protocols in Biochemistry and Clinical Biochemistry
2. Test sample solution: Dissolve the test sample in yellow-colored DNSA is reduced to orange-red
10mL. The solution should be diluted accordingly so 3-amino-5-nitrosalisyclic acid (ANSA).
that the optical density of the test sample does not Alkali
exceed that of test tube no. 5, i.e., 0.1 mg/mL of sugar. Reducing sugar + 3, 5 dinitrosalicyclic acid ! RCOO
ðyellowÞ
+ 3 amino 5 nitrosalicylic acid
Calculation ðorangeredÞ
The concentration can be obtained using a standard
graph. The dilution (if made) of the test sample should
Materials, equipment, and reagents
be multiplied to obtain the final concentration of the
A. Reagents: Dinitro salicylic reagent, sodium hydrox-
test sample solution.
ide solution (2 mol/L), test sample (sugar solution),
standard solutions.
Safety considerations and standards
B. Glassware: Test tube, test tube holder, dropper.
1. Concentrated acids should be handled very carefully,
C. Instruments: Water bath, spectrophotometer.
one must wear gloves while handling it.
2. Always add acid to water.
Protocol
Preparation of standard curve:
Pros and cons
A. Stock standard (1 mg/mL of glucose):
Pros Cons
Weigh 100 mg of glucose and add 100 mL of distilled
An easy method to test the Trioses and tetrose do not give water to it.
quantity of positive result of this test B. Working standard (0.25 mg/mL of glucose):
carbohydrates Not suitable when proteins
Dilute 10 mL of stock solution to a final volume of
having a high amount of
tryptophan is present, as it
40 mL by adding distilled water to it.
too contributes to the 1. Take six test tubes and label them.
production of red color 2. To these add 0–1 mL of working standard solu-
tion and add water to make the final volume to
Alternative methods and protocols 1 mL.
Molisch’s method. 3. Simultaneously, take 1 mL of the sample solution
in another test tube.
Summary 4. Add 1 mL of DNS reagent, mix well, and cover
1. It is a quantitative test for carbohydrates, except tri- each of the test tubes.
ose and tetrose. 5. Put the tubes in a boiling water bath for 5 min.
2. In this test, the aldehyde produced by the treatment 6. Cool the test tubes to room temperature.
of carbohydrates with conc. acid reacts with anthrone 7. Measure the optical density at 540 nm.
reagent and yields colored product based on the ini- 8. Subtract the value of the absorbance of blank
tial concentration of the sugars. from the absorbance value for each of the test
3. All the tubes containing carbohydrates are treated tubes.
simultaneously so that the test sample can be com- 9. Plot the standard calibration curve with concen-
pared with the standards. tration plotted on the X-axis and optical density
4. The reaction is sensitive to temperature; therefore, all on the Y-axis.
tubes should be cooled to room temperature before
reading the absorbance.
Test Tube Test
No. Blank 1 2 3 4 5 Sample
Definition
Working 0 0.2 0.4 0.6 0.8 1.0 1.0
Quantitative estimation of reducing carbohydrates in the solution
given sample by 3,5-dinitro salicylic acid (DNSA) test. (mL)
Water added 1 0.8 0.6 0.4 0.2 0 0
Rationale (mL)
DNS reagent 1 1 1 1 1 1 1
All types of reducing sugars undergo oxidation to form Heat in boiling water bath for 5 min. Cool it to room temperature
acids and in turn reduce many reagents like DNSA. OD at A0 A1 A2 A3 A4 A5 AT
Under alkaline conditions, the free aldehyde or ketone 620 nm
group of reducing sugar is oxidized to acids and Final OD A0 A1A0 A2A0 A3A0 A4A0 A5 A0 AT A0
CHAPTER 2 Carbohydrate 19
11. Recentrifuge the tubes at 3000 rpm for 15 min. Dis- 4. 0.5 M NaOH: 2 g NaOH in a final volume of 100 mL
card supernatant. of solution in distilled water.
12. Dissolve pellets in 2 mL of water. 5. 5. 30% KOH: 30 g KOH in a final volume of 100 mL
of solution in distilled water.
Alternative method: Using KOH
Materials, equipment, and reagents Safety considerations and standards
A. Reagents: Tissue (liver, muscle), 30% KOH solution, 1. Handle all the reagents very carefully.
saturated Na2SO4, 95% ethanol, 1.2 M HCl,
0.5 M NaOH. Pros and cons
B. Glassware: Test tube, test tube holder, dropper. Pros Cons
C. Instrument: Centrifuge (table top). An easy method to isolate glycogen Time
Isolation of glycogen: from tissues taking
1. Accurately weigh 1.5 g of the liver and skeletal
muscle. Summary
2. In a centrifuge tube take 2 mL of KOH, place the tis- 1. This is a method to isolate glycogen from mice by
sue in it. homogenization of the tissue with TCA or boiling
3. Heat in a boiling water bath for 20 min, with inter- with KOH.
mittent shaking. 2. The glycogen is obtained from the liver; muscles do not
4. Let the tube cool in ice. yield it as they lack the enzyme glucose-6-phosphatase.
5. Add 0.2 mL of saturated Na2SO4 and mix it.
6. Add 5 mL of 95% ethanol and allow the tube stand Definition
on ice for 5 min. The glycogen gets precipitated. Separation and identification of sugars present in fruit
7. Centrifuge the tube at 3000 rpm for 5 min. juices using thin-layer chromatography (TLC).
8. Discard the supernatant and add 5 mL of water, mix
thoroughly (warm it in case it does not dissolve). Rationale
9. Add double distilled water to it to make a solution Fruit juices contain a wide variety of sugars. These sugars
up to 10 mL. This is glycogen solution in water. can be identified accurately by thin layered chromatogra-
10. If the rat is NOT starved and is well fed, then dilute phy. In the experiment, various sugars have varying sol-
the solution to 100 mL with water. ubility in a solvent and this property is utilized in TLC.
Hydrolysis of glycogen: Depending on the solubility, the sugars travel the dis-
11. Take 1 mL of glycogen solution in a test tube and tance (upward) with the solvent. As the experiment pro-
add 1 mL of 1.2 M HCl to it. Heat in boiling water ceeds, the most soluble sugar will travel the longest
bath for 2 h. distance with solvent and reaches the highest point,
12. To this add 1 drop of phenolphthalein and then while the least soluble sugar will travel the shortest dis-
neutralize with 0.5 M NaOH, till the pink color of tance. The sugars can be detected after the spraying the
the indicator turns yellow. solution of aniline-diphenylamine followed by heating.
13. Then dilute it to 5 mL.
14. This results in the hydrolysis of glycogen to glucose, Materials, equipment, and reagents
which can be determined by the glucose oxidase A. Reagents: Thin layered plates of silica gel G, solvent,
method (specific for glucose). fruit juices, absolute ethanol, standard sugar solu-
tion, aniline-diphenylamine location reagent.
Analysis and statistics B. Glassware: Glass plates, separation chambers.
The glycogen extracted from tissues is hydrolyzed and glu- C. Instruments: Oven, spray gun.
cose concentration, which is an indication of glycogen
content in this context, should be higher in well-fed mice. Protocols
1. Take 1 mL fruit juice; add 3 mL of ethanol to remove
Precursor techniques denatured protein.
1. 5% TCA: Weigh 5 g of TCA and add to distilled water 2. Spot the supernatant in a thin layered plate with
to a final volume of 100 mL. standard sugar solutions.
2. 95% ethanol: To 95 mL of ethanol add 5 mL of dis- 3. Irrigate the plate with the solvent system in ascending
tilled water. direction in a chamber.
3. 1.2 M HCl: Add 10.6 mL of HCl to a final volume of 4. Let it develop until the solvent front reaches the top
100 mL of solution in distilled water. of the plate.
CHAPTER 2 Carbohydrate 21
extract can be kept for 5 days at 4°C. Since the starch Alternative methods
is partially soluble in water, the water extract is not Method of Ichimura and Hisamatsu (1999).
suitable for subsequent starch determination.
11. For starch extraction, take the pellet of ethanolic Summary
extract, let the ethanol evaporate completely. 1. The plant material is ground using liquid nitrogen
12. Add 10 mL of water to sample (ethanolic extract in a and the soluble carbohydrates are extracted using
50-mL centrifuge tube) and mix. water or ethanol.
13. To gelatinize the starch, incubate the samples at 90° 2. The starch is extracted using sodium acetate and
C with intermittent mixing for 30 min. enzymatic solution.
14. Let the samples cool at RT.
15. Add 0.2 M of sodium acetate, pH 4.5, 1 mL amylo- Summary of the sugar test.
glycosidase, and α amylase to it.
16. Incubate at RT for 1–2 h for α amylase to gelatinize Sl
No. Test Substrate Result
the starch, followed by incubation at 55°C for
16–24 h. 1 Molisch’s All The purple ring is
17. Let the tubes cool at RT then centrifuge it at 30,000 g test carbohydrates formed
for 20 min. 2 Picric acid Reducing sugars The yellow color
test turns red
18. Pour the supernatant in a volumetric flask; add
3 Fehling’s test Reducing sugars The blue solution to
10 mL water to the pellet, mix it well, and incubate red ppt
it for 10 min at 60°C. 4 Benedict’s Reducing sugars The blue solution to
19. Centrifuge it at 30,000 g for 20 min. test red ppt
20. Keep the supernatant in the same volumetric flask. 5 Tommer’s Reducing sugars The blue solution to
21. Repeat the extraction with water twice. test red ppt
22. The starch extract can be stored at 4°C for up to 6 Nylander’s Reducing sugars Black ppt
5 days. test
23. The total sugar content can be determined by the 7 Fearon’s test Reducing sugars The blue solution to
anthrone method. red ppt
8 Barfoed test Mono and Monosaccharides
disaccharides turn blue to red in
Analysis and statistics a short time
The soluble sugar extracts can be obtained as both etha- Disaccharides turn
nolic extract and water extract. The starch extract is blue to red take a
obtained after removing soluble sugars from the ethano- long time
lic extract. 9 Seliwanoff’s Ketose and Ketose give deep
test aldose cherry red; aldose
turns slowly to a
Precursor techniques faint pink
1. 95% ethanol: Add 95 mL of ethanol to make a final 10 Bial’s test Pentose and Pentose give blue-
volume of 100 mL in water. hexose green color;
2. 0.2 M sodium acetate solution (pH 4.5): Mix 2.72 g hexose give
of sodium acetate with 80 mL water, maintain the brown-gray color
pH of 4.5, and adjust the volume to 100 mL with 11 Foulger’s Ketohexose and Ketohexose gives
water. test aldohexose green-blue color;
aldohexose gives
yellow or olive
Safety considerations and standards green color
1. The blank and sample should be processed carefully 12 Mucic acid Galactose Crystals of mucic acid
in the same manner. test are formed
13 Osazone test Various sugars Different types of
crystals formed
Pros and cons
14 Iodine Polysaccharides Starch gives a blue-
Pros Cons
black color;
An easy method for determination of sugars Time taking glycogen gives a
and starch process red-brown color
CHAPTER 3
Lipid
1. Solubility test for lipids. 3. Shake well and check their solubility.
2. Emulsion test for lipids. 4. Heat it to 50°C for 5 min and again check their
3. Determination of the degree of unsaturation of fatty solubility.
acids. 5. Repeat the test using other solvents and record the
4. Determination of the saponification value of the solubility.
given fat/oil sample.
5. Determination of the fatty acid value of fat. Analysis and Statistics
6. Acrolein test for the presence of glycerol. The samples that are more soluble in polar solvent have
7. Libermann-Buchard test for the detection of small fatty acids, while the samples having larger fatty
cholesterol. acids are less soluble in polar solvents even after heating.
8. Extraction of lipid from leaves (Bligh and Dyer’s
method and single-extraction method). Safety Considerations and Standards
9. Extraction of lipid from egg yolk and estimation of 1. Alcohol is highly inflammable so utmost precaution
phosphorous content in it. should be applied while heating.
10. Extraction of lipid from tissues (Folch method).
Pros and Cons
SOLUBILITY TEST FOR LIPIDS Pros Cons
Rationale A preliminary idea about the lipid can be This test is not
Fats are esters of fatty acids. They are amphoteric in obtained specific
nature and harbor a hydrophilic head of glycerol and
Alternative Methods/Procedures
hydrophobic tail of fatty acids. Other lipids too are
hydrophobic. They get dissolved in organic solvents. Tri- Emulsion test, grease spot test, Sudan test.
glycerides with a small-chain fatty acids are slightly sol-
uble in polar solvents as water, while those having long- EMULSION TEST FOR LIPIDS
chain fatty acids are insoluble in it and form emulsions. Rationale
All triglycerides are soluble in diethyl ether, benzene, The emulsion is a mixture of two immiscible liquids.
and chloroform like nonpolar solvents. Their solubility When the sample containing lipids is suspended in eth-
in polar solvents like methanol, ethanol, acetone, etc. anol, they get partially solubilize. When the above
increases on heating. Understanding their solubility solution is mixed with water, the formation of cloudy
characteristics aids in the extraction process. emulsion occurs due to the insolubility of lipids in
water. Emulsification agents like soap, bile salts, pro-
Materials, Equipment, and Reagents teins, etc. aid in the formation of a permanent
A. Reagents: Fatty acids (butyric, palmitic acid), fats, emulsion.
and oils (butter, vegetable oil), solvents. Solvent
(water, acetone, ethanol, diethyl ether, chloroform, Materials, Equipment, and Reagents
etc.). A. Reagents: Food sample, ethanol, distilled water.
B. Glassware: Test tubes, dropper. B. Glassware: Test tubes, dropper.
C. Instrument: Burner.
Protocol
Protocol 1. Crush the food sample (only in case of solid food
1. Label various test tubes and put 1 g of different lipids sample) and place it in a dry test tube. In case of liq-
in it. uid sample, add a few drops of the sample in a dry
2. To these add 5 mL water. test tube.
2. Add 2 mL of ethanol to the samples.
to the same with a longer length of fatty acids; therefore, Then, the titer value for the sample is (Y X) mL ¼
the former will require more amount of KOH. In this mL of KOH required to saponify 1 g of fat.
way, the saponification value depicts the average molec- It is also known as the saponification value of the fat.
ular weight of a triglyceride. In this process, excess of
28:05 titre value in mL
alkali is used and the remaining KOH is determined by Saponification value ¼
ðmg=gÞ Weight of sample in gram
titrating it with 0.5 N HCl.
C H2 OR C H2 OH
Since 1 mL of 0.5 N KOH contains 28.05 mg of KOH, the
| | multiplication factor of 28.05 is included in the above
C HOR + 3KOH ! C HOH + 3RCOO K + equation.
| |
CH2 OR CH2 OH The molecular weight of KOH is 56 and a triglyceride
Fat Alkali Glycerol Soap releases three molecules of fatty acids.
Therefore,
Materials, Equipment, and Reagents 3 56 1000
Saponification value ¼
A. Reagents: Fat solvent (mixture of 95% ethanol and ðmg=gÞ Average molecular weight of fat
ether in 1:1 v/v), 0.5 N alcoholic KOH, 1% phenol-
phthalein solution in 95% alcohol, 0.5 N HCl, test OR
sample. 3 56 1000
Average molecular weight of fat ¼
B. Glassware: Burette, conical flask. Saponification value ðmg=gÞ
C. Instruments: Water bath, reflux condenser.
quality of fats can be determined by the acid value of Safety Considerations and Standards
fat or the amount of free fatty acids present in it. Their 1. Glassware should be washed before and after use.
presence is determined by the titration of the sample 2. Carefully note down the mL required in the process
with KOH. The acid value is defined as milligrams of of titration.
KOH required to neutralize the free fatty acids in 1 g 3. The change in the color of the solution should be
of fat or oil. monitored carefully.
EXTRACTION OF LIPID FROM LEAVES 6. Shake the extracts at 100 rpm for 24 h in an orbital
(BLIGH AND DYER’S METHOD AND SINGLE- shaker.
EXTRACTION METHOD) 7. Transfer the intact, extracted leaf materials to a new
Rationale vial using forceps.
One phase system is used in Bligh and Dyer’s method, 8. Let it dry overnight at 105°C.
with chloroform:methanol:water (1:2:0.8), with the tis- 9. Add 280 μL of 600 mM ammonium acetate to the
sue water included in the water amount. The extraction is sample before lipid analysis.
followed by the addition of chloroform and methanol to
make two phases. Lipid is found in the chloroform phase. Precursor Techniques
BHT acts as an antioxidant. KCl form cations, which aid 1. 0.01% BHT: Weigh 1 mg of BHT and add it to 10 mL
in shifting of lipid separation to the organic phase. of water.
2. 1 M KCl: Add 7.45 g of KCl to make a 100-mL solu-
Materials, Equipment, and Reagents tion with water.
A. Reagents: Test samples, anhydrous potassium hydro-
gen sulfate, 0.01% butylated hydroxytoluene (BHT). Analysis and Statistics
B. Glassware: Test tubes, test tube holders. The pungent smell of the fumes indicates the presence of
C. Instrument: Bunsen burner. glycerol in the test sample.
Protein
800 mL distilled water. Adjust the pH 7.4 with HCl. Pros and cons
Make the final volume of 1000 mL. Pros Cons
2. RIPA buffer: Extracted proteins are compatible Not suitable for study
with various assays protein-protein
Volume for 10 mL
interaction
Reagents Stock Working Buffer
The lysis buffer does not interfere
Tris-HCl pH 7.4 1M 50 mM 500 μL with the immunoreactivity
NaCl 4M 150 mM 375 μL hence suitable for western
EDTA (pH 8) 0.5 M 1 mM 20 μL assay, immunoassays
SDS 10% 0.1% 100 μL
Triton X-100 100% 1% 100 μL
Na-deoxycholate 10 mg Alternative methods/procedures
Distilled water Remaining to make NP-40 buffer, Laemmli sample buffer (LSB).
the volume 10 mL
Protease 3–4 μL
inhibitors Troubleshooting and optimization
Phosphatase 3–4 μL Problem Solution
inhibitors or Low protein Use less RIPA buffer
sodium concentration
orthovanadate Protein Use protease inhibitors in the buffer just
degradation before use
• 1 M Tris HCl (pH 7.4): Dissolve 121.1 g Tris base in
Low protein yield Lyse the cells completely in the buffer
800 mL distilled water. Adjust the pH 7.4 using HCl. and incubate in the buffer for a
Make the final volume of 1000 mL and autoclave. longer time
• 4 M NaCl: Dissolve 58.44 g NaCl in 250 mL of dis-
tilled water.
• 0.5 M EDTA (pH 8): Dissolve 18.61g disodium ethyl- Summary
enediaminetetraacetate. 2H2O into 80mL of distilled 1. The cultured cells are first harvested, then lysed in
water. Mix and shake vigorously using a magnetic stir- RIPA buffer. The lysed cells are centrifuged at
rer. Adjust the pH 8 using NaOH pellets. Once the pH 13,000 rpm for 15 min at 4°C. The solubilized
adjusted and salt dissolves, make the final volume proteins in the supernatant is then transferred to
100 mL by distilled water and autoclave. another tube.
• 10% SDS: Dissolve 10g SDS in 100 mL distilled water. 2. The animal tissue is dissected and cut into pieces.
• Amount of RIPA buffer used for cultured cells (grown The tissues are homogenized in RIPA buffer, centri-
in). fuged, and the supernatant is transferred to another
100 mm dish 1 mL tube.
60 mm dish 0.5–0.6 mL
35 mm dish or 6 well plate 0.3 mL Definition
12 well plate 0.2 mL
To detect the presence of protein in the given sample by
24 well plate 0.1 mL
the Biuret test.
Safety considerations and standards
1. Protease and phosphatase inhibitors must be added Rationale
just before use. Biuret test is used for the detection of peptide bonds in
2. All the steps for cell lysis and protein extraction must the protein. This test is not suitable for amino acid only.
be carried out at 4°C or ice. The protein solution when reacts with CuSO4 in alkali
3. Autoclave all the reagents and solutions after condition (NaOH/KOH), purple to violet-colored cop-
preparations. per (II) cation complex is formed. The intensity of the
complex is directly proportional to the number of the
Analysis and statistics peptide bond in the protein sample.
The isolated proteins are quantitated by an appropriate
NaOH
method and stored at 20°C. Protein + CuSO4 ! Copper cation complex ðpurple to violetÞ
CHAPTER 4 Protein 33
BIURET TEST
Negative
r
Colo Biuret test
ue
Bl
NaOH CuSO4 Heat
Vi
ol
et
Sample Co
lo
+ rc
NaOH ha
Sample ng
+ e
Sample + CuSO4
NaOH
Positive Biuret
test
Definition
To detect the presence of protein in the given sample by Heating NaOH
Protein + conc:HNO3
! Yellow nitro compound ! Orange color
the Xanthoproteic test.
1. The first principle: The belief in the existence of the Creator; that
is, the belief that there exists a Being who requires no other cause
for His existence, but is Himself the cause of all beings.
2. The second principle: The belief in the Unity of God; that is, the
belief that the Being who is the cause of everything in existence is
One; not like the unity of a group or class, composed of a certain
[21]number of individuals, or the unity of one individual consisting of
various constituent elements, or the unity of one simple thing which
is divisible ad infinitum, but as a unity the like of which does not
exist.
3. The third principle: The belief in the Incorporeality of God; that is,
the belief that this One Creator has neither bodily form nor
substance, that He is not a force contained in a body, and that no
corporeal quality or action can be attributed to Him.
4. The fourth principle: The belief in the Eternity of God; that is, the
belief that God alone is without a beginning, whilst no other being is
without a beginning.
7. The seventh principle: The belief that our teacher Moses was the
greatest of all prophets, both those before him and those after him.
8. The eighth principle: The belief in the Divine origin of the Law; the
belief that the whole Pentateuch was communicated to Moses by
God, both the precepts and the historical accounts contained therein.
9. The ninth principle: The belief in the integrity of the Law; that both
the written and the oral Law are of Divine origin, and that nothing
may be added to it or taken from it. [22]
10. The tenth principle: The belief that God knows and notices the
deeds and thoughts of man.
11. The eleventh principle: The belief that God rewards those who
perform the commandments of His Law, and punishes those who
transgress them.
12. The twelfth principle: The belief that Messiah will come at some
future time, which it is impossible for us to determine; that he will be
of the house of David, and will be endowed with extraordinary
wisdom and power.
13. The thirteenth principle: The belief in the revival of the dead, or
the immortality of the soul.
These thirteen principles (שלשה עשר עקרים) may be divided into three
groups, according to their relation to the three principles:—1.
Existence of God. 2. Revelation. 3. Reward and punishment. The
first group includes the first five principles, the second the next four,
and the third the remaining four. In this order they will now be
considered.
[Contents]
“Lift up your eyes on high, and behold who hath created these? Who
is He who bringeth them forth by number? All of them He calleth by
name, by the greatness of His might, and for that He is strong in
power, not one is lacking” (Isa. xl. 26). “The heavens declare the
glory of God, and the firmament sheweth His handywork” (Ps. xix. 2).
The regularity in the rising and setting of the heavenly bodies, which
enables us to foretell the exact time and duration of an eclipse of the
sun or the moon, is certainly a strong argument for the belief that
there is a mighty and wise Creator who fixed the laws in accordance
with which these luminaries move.
“Beautiful are the luminaries which our God has created. He has
formed them with knowledge, reason, and understanding; He
endowed them with power and strength to rule in the midst of the
world. Full of splendour and beaming with light, they illumine the
whole world; they rejoice when they rise, they are glad when they
set, doing in reverence the will of their Master” (Sabbath Morning
Service).
A very general object of worship were the stars. Rabbi Jehudah ha-
Levi, in Kuzari iv. 1, in trying to explain the origin of this practice,
says as follows:—“The spheres of the sun and the moon do not
move in the same way. A separate cause or god was therefore
[26]assumed for each, and people did not think that there was a
higher force on which all these causes depended.” The ancient
monuments and the treasures stored up in our museums show how
great was the variety of forms which idolatry took, and to how great
an extent people adhered, and still adhere, to this kind of worship.
But there have been thinkers and philosophers even among the
idolatrous nations who sought a unity in the construction and working
of the universe, and early arrived at the idea of a First Cause as the
sole source of all that exists.
2. The fact that the influence of the Divine power makes itself
perceptible to the observing eye of man everywhere produced
another kind of human error: Pantheism (All-God). Modern
Pantheism dates from Spinoza; but long before Spinoza, when the
secret forces at work in the changes noticed by us in all material
objects were recognised as properties inherent in the substance of
things, these forces were considered as the sole independent
causes of the existing universe, and the combination of these forces,
called Nature, was considered to be the First Cause, or God. A
modification of this theory is contained in the philosophy of Spinoza.
According to this great philosopher’s system, the universe in its
entirety has the attributes of the Deity: there exists nothing but the
Substance (God), its attributes, and the various ways in which these
attributes become perceptible to man. Spinoza tried to defend
himself from the reproach of describing God as corporeal, but he did
not succeed. The attribute of extension or space which God
possesses, according to Spinoza, is only conceivable [27]in relation
to corporeal things. The philosophy of Spinoza is in this dilemma:
either God is corporeal, or the corporeal world does not exist. Both
assumptions are equally absurd. It is true, in one of his letters he
complains that he has been misrepresented, as if he believed God to
consist of a certain corporeal mass. But we cannot help assuming
the existence of a certain corporeal mass, and if this is not God, we
must distinguish in our mind God and something that is not God,
contrary to the fundamental doctrine of Pantheism. Besides, there
are many incongruities and improbabilities involved in this theory. It
has no foundation for a moral consciousness. The wicked and the
good are alike inseparable from God. They both result with necessity
from the attributes of God, and they cannot be otherwise than they
actually are. If we, by the consideration that injury done to us by our
fellow-man was not done by that person alone, but by a series of
predetermined necessary causes, may be induced to conquer hatred
against the apparent cause of our injury, we may equally be induced
by the same reasoning to consider the kindness and benefits of our
friends not worthy of gratitude, believing that they were compelled to
act in this manner, and could not act otherwise.
In the Bible atheism is stigmatised as the source of all evils. Thus the
patriarch Abraham suspected the [28]people of Gerar, that there was
“no fear of God” in the place, and was afraid “they might slay him”
(Gen. xx. 11); whilst Joseph persuaded his brothers to have
confidence in him by the assertion, “I fear God” (Ib. xlii. 18). The first
instance of an atheist we meet in Pharaoh, king of Egypt, when he
defiantly said, “I know not the Lord, neither will I let Israel go” (Exod.
v. 2). Another form of atheism is warned against in the words of
Moses: “Lest thou sayest in thine heart, My strength and the power
of my hand has got for me all this wealth” (Deut. viii. 17); and “Lest
they say, Our hand is high, and it is not the Lord that hath done all
this” (Ib. xxxii. 27). The prophets likewise rebuke the people for want
of belief in God. In the Psalms, the crimes and evil designs of
oppressors are traced to godlessness. “The wicked says in his heart,
There is no God” (Ps. xiv. 1). But this atheism of the Bible is not a
theoretical or dogmatic one; it is not the result of thought, or of deep
inquiry into the causes of things, but merely the voice of an evil
inclination which tempts man to act contrary to the command of God,
and assures him of immunity, under the impression that his actions
are not watched by a higher authority. In post-Biblical literature we
meet with the phrase, לית ִּד ין ולית ַּד ָּין“There is no judgment, and there
is no judge,” as the basis of atheism.
All these various systems of religion have this in common, that they
attempt to remove from religion everything that cannot be
comprehended by human reason. But all attempts to substitute
human reason for Divine authority have failed. A limit has been set to
human reason, and that cannot be overcome. In every system of
religion—the natural and the rational included—there is a mystic
element, which may be enveloped in a mist of phrases, but remains
unexplained. Whether we call the Creator and Ruler of the universe
God, Deus, or Theos, His relation to the universe, and to man in
particular, cannot be [30]determined by the laws which determine the
natural phenomena in the universe, created by His Will.
The first principle declared in our creed is this: God is not only the
Creator of the heavens and the earth, with all their hosts; He is also
the constant ruler of all created beings; He is בורא ומנהיג. We
therefore praise Him in our daily Morning prayer as “Doing wonders;
renewing in His goodness the work of the creation every day.” When
we observe the ordinary phenomena in nature, occurring in
accordance with certain fixed laws which have been discovered and
described by man, we see in them the greatness of the Creator by
whose will these laws are still in force, and by whose will any or all of
these laws may one day cease to continue.
It has been asserted that any interruption or change [32]of these fixed
laws would indicate a weakness and want of foresight on the part of
the Creator, and a fault in the plan of the Creation. This notion has
led people either to deny the truth of the Biblical accounts
concerning the miracles wrought by the Almighty, or to admit the
correctness of the facts while denying their miraculous character, or
to consider the fixed laws of nature, together with their exceptions,
as designed in the original plan of the Creation. How short-sighted is
man! He cannot even fully comprehend his own short-sightedness!
God made him ruler over the works of His hands, and he presumes
to be the ruler of God Himself! When we learn from numerous
observations and experiments the law that seems to regulate certain
recurring phenomena, have we then fathomed the infinite wisdom of
God in the Creation? Do we know the reason which led Him to
produce certain things according to certain laws, and not otherwise?
Have we in discovering a law of nature obtained the power of
prescribing the same law to God, and disallowing Him to deviate
therefrom? Far be it from us human beings, dust and ashes, to
arrogate to ourselves such a right! It may even be one of the objects
with which miracles were wrought to teach us that we do not yet
know all things, that events may happen which we are unable to
foresee, that phenomena may appear which we are unable to
explain according to the laws hitherto discovered; in short, that our
knowledge and wisdom are limited.
The fact that God has created the universe ex nihilo has been
expressed by Jewish philosophers as follows:—God is the only
Being who demands no cause for His existence; the very idea of
God implies existence, [33]and cannot be conceived without it. All
other beings owe their existence to certain causes, in the absence of
which they would not exist. God alone is therefore only active,
without ever being passive, only cause without ever being effect,
whilst every other being is both active and passive, cause and effect;
it has been produced by certain causes, and is in its turn the cause
of the existence of other beings. In the first article a phrase
expressing this idea has been added: “And He alone is the active
cause of all things, whether past, present, or future.” By the addition
of this sentence it was intended to deny the Eternity of matter (קדמות
העולם). The reference to past, present, and future is to emphasise
the constant action of the Creator, and the dependence of the natural
forces on His Will. The first principle has, therefore, the following
form:—