Final Revision - JEE (Main) : Subjective
Final Revision - JEE (Main) : Subjective
Final Revision - JEE (Main) : Subjective
Subjective:
3. Why potassium can not be obtained by the electrolysis of fused potassium chloride?
4. Explain why halides of beryllium fume in moist air but other alkaline earth metals halides
do not.
5. A piece of burning magnesium ribbon continuous to burn in sulphur dioxide. Explain.
6. Explain
(a) Be does not react with water or steam.
(b) Mg does not react readily with water.
7. Blue colour of the solution of alkali metals in liquid ammonia fades on standing why?
8. Explain
(a) The hydroxides of alkaline earth metals are weaker bases than their corresponding
alkali metals.
(b) Ca, Br, Sr are stored in paraffin but Be & Mg are not?
9. Account for the following
(a) Be OH 2 is insoluble but Ba OH 2 is fairly soluble in water.
(b) Be OH 2 is amphoteric while Mg OH2 is basic.
16. 20 ml of a solution containing 0.2 g of impure sample of H2O2 reacts with 0.316 g of
KMnO4 (acidic). Calculate
(a) Purity of H2O2 .
(b) Volume of dry O2 evolved at 0 C and 750 mm P.
In the reaction H2+I2 2HI the rate of disappearance of I2 is found to be 10 mole per
-6
18.
litre per second. What would be the corresponding rate of appearance of HI?
When silver nitrate is added to the solution, AgCN gets precipitated. What will happen to
the equilibrium?
21. Which of the following reactions will get affected by increase in pressure? Also mention
whether the change will cause the reaction to go to the right or left direction.
(i) CH4 g 2S2 g CS2 g 2H2S g (ii) CO2 g C s 2CO g
(iii) 4NH3 g 5O2 g 4NO g 6H2O g (iv) C2H4 g H2 g C2H6 g
23. At 540 K, 0.10 mole of PCl5are heated in a 8.0 L flask. The pressure of the equilibrium
mixture is found to be 1.0 atm. Calculate Kp and KC for the reaction.
24. In the reaction C(s) + CO2(g) CO2(g) the equilibrium pressure is 12 atm. If 50% of CO 2
reacts calculate Kp.
25. Ammonium carbamate dissociates as: NH2COONH4 (s) 2NH3 (g) + CO2 (g)
In a closed vessel containing ammonium carbamate in equilibrium with its vapour
ammonia is added such that the partial pressure of ammonia now equals to the original
total pressure. Calculate the ratio of the total pressure now to the total pressure of the
original mixture.
1
26. Calculate the equilibrium constant for reaction NO2 N2 O2 , if equilibrium
2
constant is 100 atm for equilibrium N2 2O2 2NO2 , at constant temperature
-1
28. N2O4 is 20% dissociated at 27C and 1 atm pressure. Calculate (i) Kp and (ii) the
percentage dissociation at 0.2 atm and 27C
29. When 0.10 mole of NH3 is dissolved in water to make 1.0 L solution, the solution is found
to have OH 1.34 103 M . Calculate Kb for NH3.
-6
30. An acid - base indicator, HIn(KIn= 10 ) displays the colour of its acid form only when it is
ionised to a maximum of 9.09%, while it displays its basic colour when it is ionised to the
extent of at least 95.24%. What is the pH - range of the indicator?
2+ 2+
31. When a solution containing Ca and Mg ions is at first saturated with NH 4Cl(s) and then
2+
treated with (NH4)2CO3, only Ca is precipitated as carbonate. Explain.
32. A weak acid type indicator was found to be 40% dissociated at pH = 9.1249. What be %
dissociation at pH = 9?
34. A buffer of pH 9.26 is made by dissolving x mole of ammonium sulphate and 0.1 mole of
ammonia into 100 mL solution. If pKb of ammonia is 4.74, calculate value of x.
+
35. Calculate [H ] in
(a) 0.01 M C6H5COOH solution and
(b) 0.01 M C6H5COOH in 0.01 M C6H5COONa; K a C6H5COOH 6.5 105
38. It is found that 0.1 M solution of three sodium salts NaX, NaY and NaZ have pH 7.0, 9.0
and 11.0 respectively. Arrange the acids HX, HY and HZ in order of increasing strength.
Where possible, calculate ionization constant of acids. 32. Concentration of HCN
and NaCN in a solution is 0.01 M each. Calculate H3O and [OH]
K a HCN 7.2 1010
39. Concentration of HCN and NaCN in a solution is 0.01 M each. Calculate H3O and
[OH] K a HCN 7.2 1010
42. To a 25 ml H2O2 solution excess of acidify solution of potassium iodide was added. The
iodine liberated required 20 ml of 0.3 sodium thiosulphate solution. Calculate the volume
strength of H2O2 solution.
o
43. In a mixture of N2 and H2 initially in a mole ratio of 1:3 at 30 atm and 300 C, the
percentage of ammonia by volume under equilibrium is 17.8. Calculate the equilibrium
constant (KP) of the mixture, for the reaction, N2(g) + 3H2(g) 2NH3(g)
44. An equilibrium mixture at 300 K contains N2O4 and NO2 at 0.28 and 1.1 atm respectively.
If the volume of container is doubled, calculate the new equilibrium pressures of the two
gases.
45. The value of Kc for the reaction N2 g 3H2 g 2NH3 g is 0.50 at 400C. Find the
value of Kp at 400C when concentrations are expressed in mol 1 and pressure in
atmosphere.
49. A solution of volume V contains ‘a’ mole of MCl and ‘b’ mole of NCl where MOH and
NOH are two weak bases having dissociation constants K1, K2 respectively. Show that
1 K K V
the pH of the solution can be expressed as pH = log10 1 2
2 K W aK 2 bK1
50. 0.025 moles of a hydrochloride salt of – amino acid (NH2 – CH2 – COOH) was dissolved
in 250 ml of water and the pH of the solution was 2.7. Same moles of sodium salt of this
acid is added to 250 ml water and the pH of solution now is 11, Calculate the pH of
amino acid at which isoelectric point will occur.
1. When a substance (A) reacts with water, it produces a combustible gas (B) and a solution
of substance (C) in water. When another substance (D) reacts with the solution of (C), it
produces the same gas (B) on warming, but (D) can produce (B) on reaction with dilute
H2SO4 at room temperature. (A) imparts a golden yellow colour to brown flame. (A), (B),
(C) and (D) could be?
(A) K, H2, KOH, Al (B) Na, H2, NaOH, Zn
(C) CaC2, C2H2, Ca(OH)2, Fe (D) Ca, H2, Ca(OH)2, Sn
2+
2. If NaOH is added to an aqueous solution on Zn ions, a white ppt. appears and on
adding excess NaOH, the ppt. dissolves. In this solution zinc exist in the
(A) cationic part (B) anionic part
(C) both in cationic and anionic parts (D) there is no zinc left in the solution
5. A metal (X) on heating in nitrogen gas gives (Y). (Y) on treatment with H 2O gives a
colourless gas which when passed through CuSO4 solution gives a blue colour .(Y) is
(A) Mg(NO3)2 (B) Mg3N2
(C) NH3 (D) MgO
7. Match list – I with list – II and select the correct answer using the codes given below
List – I List – II
(a) Liquid Na metal 1. Breathing apparatus in submarine
(b) Potassium stearate 2. Explosive
(c) KNO3 3. Coolant in nuclear reactors
(d) KO2 4. Soft soap
Codes
a b c d
(A) 3 4 1 2
(B) 3 1 4 2
(C) 3 4 2 1
(D) 4 3 2 1
17. Disodium hydrogen phosphate in presence of NH4Cl and NH4OH gives a white ppt. with a
2+
solution of Mg ions. The precipitate is
(A) Mg(H2PO4)2 (B) Mg3(PO4)2
(C) MgNH4PO4 (D) MgHPO4
18. Commercial 10 volume H2O2 is a solution with a strength of approximately
(A) 30% (B) 3%
(C) 1% (D) 10%
19. Hydrogen peroxide when added to a solution of KMnO 4 acidified with H2SO4
(A) forms water only (B) acts as an oxidizing agent
(C) acts as a reducing agent (D) reduces H2SO4
20. In basic medium, H2O2 acts as an oxidizing agent in its reaction with
(A) Cr2(SO4)3 (B) Ag2O
(C) K3[Fe(CN)6] (D) K2Cr2O7
37. A buffer solution contains 100 mL of 0.01 M CH3COOH and 200 mL of 0.02 M
CH3COONa. 700 ml water is added. pH before and after dilution are: (pKa = 4.74)
(A) 5.04, 5.04 (B) 5.04, 0.504
(C) 5.04, 1.54 (D) 5.34, 5.34
38. H2O H3PO4 H3O H2PO4 pK1 2.15
2
H2O H2PO H3O HPO
4 pK 2 7.20
4
Hence pH of 0.01 M NaH2PO4 is
(A) 9.35 (B) 4.675
(C) 2.675 (D) 7.350
O COCH 3
COOH
39.
(Aspirin) is a pain reliever with pKa = 2.
41. A monoprotic acid in 1.00 M solution is 0.001% ionized. The dissociation constant of
formic acid is
(A) 1.0 103 (B) 1.0 106
8
(C) 1.0 10 (D) 1.0 1010
42. Formic acid is 4.5% dissociated in 0.1 N solution at 20C. The ionization constant of
formic acid is
(A) 21 104 (B) 21
(C) 0.21 104 (D) 2.1 104
44. The precipitate of CaF2 (Ksp = 1.7 1010) is obtained when equal volumes of which of
the following are mixed?
(A) 104 M Ca + 104 M F (B) 102 M Ca + 103 M F
2+ 2+
2 5
(D) 10 M Ca + 105 M F
3
2+ 2+
(C) 10 M Ca + 10 M F
45. Buffering action of a mixture of CH3COOH and CH3COONa is maximum when the ratio of
salt to acid is equal to
(A) 1.0 (B) 100.0
(C) 10.0 (D) 0.1
47. For two ionic solids CaO and KI, identify the correct statement/s among the following:
(A) Lattice energy of CaO is much higher than that of KI.
(B) KI is soluble in benzene.
(C) CaO has high m. pt.
(D) KI has high m. pt.
A reaction is catalysed by H ion. In presence of HA, rate constant is 2 103 min1 and
+
50.
in presence of HB rate constant is 1 103 min1, HA and HB both being strong acids, we
may conclude
(A) equilibrium constant is 2
(B) HA is stronger than HB
(C) relative strength of HA and HB is 2
(D) HA is weaker than HB and relative strength is 0.5
51. Which of the following statement(s) is(are) wrong?
(A) at equilibrium concentration of reactant and product become constant because the
reaction stops
(B) addition of catalyst speeds up the forward reaction more than the backward reaction
(C) equilibrium constant of an exothermic reaction decreases with increase of
temperature
(D) Kp is always greater than Kc
52. Which of the following will not affect the value of equilibrium constant of a reaction?
(A) change in concentration of the reactants (B) change in temperature
(C) change in pressure (D) addition of catalyst
1
53. The equilibrium constant of the reaction SO2 O2 SO3 and 2SO2 O2 2SO3 are
2
K1 and K2 respectively. The relationship between K1 and K2 is
(A) K1 = K2 (B) K 2 K12
(C) K1 K 2 (D) K 2 K1
54. For which of the following reactions is the equilibrium constant called an acidity constant?
(A) 2H2O H3 O OH
(A) K p PCO2 (B) K p K c RT
(C) K c CO2 (D) none of these
1 1
56. N2O2 2NO, K1; N2 O2 2NO, K 2 ;
2 2
1 1
2NO N2 O2 , K 3 ; NO N2 O2 , K 4 ;
2 2
Correct relation (s) between K1, K2, K3 and K4 is/are
57. For the reaction, PCl5 g PCl3 g Cl2 g the forward reaction at constant
temperature is favoured by
(A) introducing an inert gas at constant volume
(B) introducing chlorine gas at constant volume
(C) introducing an inert gas at constant pressure
(D) introducing the volume of the container
(E) introducing PCl5 at constant volume
58. Which of the following will favour the formation of NH3 by Haber’s process?
(A) increase temperature (B) increase of pressure
(C) addition of catalyst (D) addition of promoter
59. Which of the following will not affect the volume of equilibrium constant of a reaction?
(A) change in the concentration of the reactants
(B) change in temperature
(C) change in pressure
(D) addition of catalyst
60. For the gas phase reaction,
C2H4 H2 C2H6 , H 136.8kJmol1
Carried out in a reaction vessel, the equilibrium concentration of C 2H4 can be increased
by
(A) increasing the temperature (B) decreasing the pressure
(C) removing some H2 (D) adding some C2H6
61. When NaNO3 is heated in a closed vessel oxygen is liberated and NaNO 2 is left behind.
At equilibrium which are not correct?
(A) Addition of NaNO2 favours reverse reaction
(B) Addition of NaNO3 favours forward reaction
(C) Increasing temperature favours forward reaction
(D) Increasing pressure favours reverse reaction
62. Zn 2H Zn2 H2
Half life period is independent of concentration of Zn at constant pH. For the constant
concentration of Zn, rate becomes 100 times when pH is decreased from 3 to 2. Hence
dx
k Zn H
2
(A)
dt
dx
k Zn H
2
(B)
dt
+
(C) rate is not affected if concentration of Zn is made four times and that of [H ] ion is
halved
+
(D) rate becomes four times if concentration of [H ] ion is doubled at constant Zn
concentration
63. All of the following are acid-base conjugate pairs.
(A) HONO, NO2 (B) H3O , OH
+
66. An acid-base indicator has a Ka of 3.0 105. The acid form of the indicator is red and the
basic form is blue. Then
(A) pH is 4.05 when indicator is 75% red
(B) pH is 5.00 when indicator is 75% blue
(C) pH is 5.00 when indicator is 75% red
(D) pH is 4.05 when indicator is 75% blue
70. Addition of which of the either reactant or products to the equilibrium mixture will NOT
affect the partial pressure of H2(g)?
72. If there is an increase in mole percent of HBr(g) after increasing the temperature of the
above reaction is ……………… in nature.
Comprehension-II
83. The oxide that gives hydrogen peroxide on treatment with dilute acid is
(A) PbO2 (B) Na2O2
(C) MnO2 (D) TiO2
.
84. 0.2 g sample of H2O2 required 10 ml of N KMnO4 in a titration in the presence of H2SO4
The purity of H2O2 is
(A) 25% (B) 65%
(C) 85% (D) 95%
87. Match the chemical reaction in equilibrium (in list I) with the pressure dependence of
degree of dissociation of the reaction (in list II):
List-I List-II
A. A 2 g 3H2 g 2NH3 g
1. x p
B. 2SO2 g O2 g 2SO3 g 2. 1
x
p
C. PCl5 g PCl3 g Cl2 g 3. xp
D. N2 O2 2NO 4. x p0
88. Match the effect of addition of 1 M NaOH to 100 mL 1 M CH 3COOH (in list-I) with
pH (in list-II):
List-I List-II
(A) 25 mL of NaOH 1. pKa
(B) 50 mL of NaOH 2. pKa + log3
(C) 75 mL of NaOH 3. pKa log3
89. Match the salt (in list-I) with its equation of pH (in list-II):
List-I List-II
(A) Weak acid and strong base 1. 1
pK w
2
(B) Strong acid and weak base 2. 1
pK w pK a pKb
2
(C) Weak acid and weak base 3. 1
pK w pKb logC
2
(D) Strong acid and strong base 4. 1
pK w pK a logC
2
1. Anhydrous MgCl2 can not be prepared by simply heating MgCl2.6H2O because it get
hydrolysed by its own water of crystallization.
MgCl2 6H2 O MgO 2HCl 5H2O
However if hydrated magnesium chloride is heated in an atmosphere of HCl gas at 650
K, it cheeks the above hydrolysis reaction and the hydrated magnesium chloride now
loses water of crystallization to form anhydrous MgCl2.
MgCl2 6H2O
HCl gas
650 K
MgCl2 6H2O
2. Halides of Be are covalent because of high I.E. of Be while those of Ba are ionic due to
low I.E. of Ba.
4. BeCl2 reacts with the moisture to form HCl while other halides do not.
BaCl2 + 2H2O Ba(OH)2 + 2HCl
5. A piece of Mg ribbon continues to burn in SO2 since it reacts to form MgO and S
2Mg SO2 heat
2MgO S
This reaction is so much exothermic that heat evolved keeps the Mg ribbon burning.
7. On standing the ammoniated ions and electrons combine to form metal amide, hence the
colour fades.
8. (a) Due to high ionization energies and less solubilities of alkaline earth metals as
compared to alkali metals.
(b) Ca, Ba, Sr are much reactive towards oxygen and forms respective oxide but Be &
Mg are not so reactive and they form a protective layer of oxide on their surface so
they are not stored in paraffin.
10. (i) HNO3 is partially decomposed in sun light to produce NO 2. The NO2 formed get
dissolved in HNO3 to produced yellow colour.
4HNO3 Sunlight
4NO2 + 2H2O + O2
(ii) Liquor ammonia possess high vapour pressure at room temperature and thus before
opening a bottle of liquor ammonia, it should be cooled to lower the pressure of NH 3
inside the bottle, otherwise NH3 will bump out of the bottle.
(iii) Air has oxygen about 1/5 of volume, while N2O on decomposition produces oxygen
about 1/3 of the volume.
(iv) Nitrogen trifluoride is not hydrolysed because neither N nor fluorine possess vacant
d-orbitals to form extra bond with lone pair of electrons on oxygen of water molecule.
However, NCl3 has vacant d – orbitals on Cl atom and hydrolysis
NCl3 + 3H2O NH3 + 3HOCl
(v) Red phosphorus is believed to exist as chains of P4 tetrahedron linked together,
whereas in yellow phosphorus individual P4 molecules are held together by week van
der Waals forces
(vi) The existence of nitrogen as diatomic molecule is due to its ability to form it bonds
which are not possible in case of other elements due to repulsion between non –
bonded electrons of the inner core.
11. (a) O O
H O P OH H O P O H
H OH
(Phosphorus acid) (Phosphoric acid)
When phosphene is treated with acidified cupric sulphates, a black precipitate of
cupric phophide is precipitated.
3CuSO4 + 2PH3 = Cu3P2 + 3H2SO4
(b) PH3 + 6AgNO3 = Ag3P.3AgNO3 + 3HNO3
Ag3P.AgNO3 + 3H2O = 6Ag + 3HNO3 + H3PO3
When phosphene passed into silver nitrate solution phosphene forms a black ppt. of
metallic silver a yellow intermediate compound being first formed.
(c) 2HgCl2 + H3PO3 + H2O = Hg2Cl2 + 2HCl + H3PO4
Hg2Cl2 + H3PO3 + H2O = 2Hg(l) + 2HCl + H3PO4
When phosphorus acid is treated with mercuric chloride of given a white precipitate of
calomel in the cold.
14. (i) I2 is non polar nature and thus solubility in water ( a polar solvent) is less which
however becomes more if KI is present due to complex formation
I2 + KI KI3 (soluble complex)
(ii) H2F2 exists as dimeric molecule due to H-bonding and thus shows dibasic nature.
+ – – +
Hence it gives two series of salts KHF2 as [K and F ----------- H — F ] and KF [K
–
and F ] where as HCl and HBr do not show hydrogen bonding and thus formation of
KHCl2 and KHBr2 is not possible.
(iii) Unlike O2, helium is not soluble in blood even under high pressure and a mixture of
He and O2(80 : 20) is used instead of ordinary air, by divers for respiration.
15. (i) 4S + 6NaOH Na2S2O3 + 2Na2S
(ii) 2CuSO4 + SO2 + KCNS + 2H2O 2CuCNS + K2SO4 + 2H2SO4
18. H2 + I2 2HI
d[H2 ] d[I ] 1 d[HI]
2 10 6
dt dt 2 dt
Rate of disappearance of H2 per mole = rate of disappearance of I2 per mole = Rate of
appearance of HI per mole
d[HI]
2 10 6 mol lt 1 sec 1
dt
x y
19. Let rate law can be given as rate = K[A] [B] . From the data given it is clear that by
doubling the concentration of A rate also becomes double, when B is kept constant. Thus
rate is directly proportional to conc. of A
Rate [A] x= 1
When the concentration of A is kept constant and the concentration of B is doubled the
rate does not change.
y=0
dx Rate
Rate = K[A] K
dt A
0.005
K= 0.5 min1
0.01
20. Equilibrium gets displaced to the left because with removal SCN ions from the
equilibrium mixture, more of the deep red complex (Product) will decomposes into the
reactants. Thus, the colour of the solution will slowly change from deep red to pale
yellow.
21. (i) Increase in pressure will not affect the equilibrium because there is no change in the
number of moles as a result of the reaction.
(ii) Increase in pressure will favour the backward reaction because number of moles per
unit volume(or pressure) decrease in the backward direction.
(iii) Increase in pressure will favour the backward reaction because the number of moles
per unit volume (or pressure) decrease in the backward direction.
(iv) Increase in pressure will favour the forward reaction because the number of moles
per unit volume (or pressure) decrease in the forward direction.
22. 5.27
–2
23. Kc = 4 10 , KP = 1.77
24. 16 atm
25. 31:27
26. 0.1
27. 34%
30. pKIn = 6
In
pH = pKIn + log
HIn
For acidic colour to prevail:
In 9.09 1
HIn 90.91 10
pH 6 - 1 = 5
For basic colour to prevail:
In 95.24
20
HIn 4.76
pH 6 + 1.3 = 7.3
pH range : 5 - 7.3
- +
32. HIn In + H
C(1-) C C
C(1 )
pH = pKIn - log
C
6
9.1249 = pKIn – log = pKIn - 0.1760
4
pKIn = 9.3010 at pH = 9
1
9 = pKIn - log
1
9 = 9.3010 – log ’
1 1
0.3010 = log i.e. 2 = = 0.3
+
% dissociation = 33.3%33. If we do not consider [H ] from H2O, then
+ 8
[HCl] = [H ] = 10 M
pH = 8 which is not possible since acidic solution should have pH < 7
If we consider H 1 107 M
H2 O
pH = 9.26
pOH = 14 – 9.26 = 4.74
NH4
pOH pK b log
NH4OH
200x
4.74 4.74 log
10
log20x = 0
20x = 1
1
x 0.05
20
[OH] = 103 = C
Sin = C = 0.05
103 103
α 2 102 2%
C 0.05
(a) The solutions of alkali metal salts contain metal cations, H , OH and the anions. The
+
41.
+
discharge potential of H ions is lower than the metal cations and thus, on electrolysis
of solutions of alkali metal salts, hydrogen is discharged at cathode rather than the
metal.
However, on electrolysis of molten salt, the metal cations only present gets
discharged at cathode.
(b) Sodium hydroxide continuously absorbs carbon dioxide of atmosphere and is
converted into sodium carbonate. A stage reaches when the solution becomes
saturated and the crystals are formed. These crystals, with the passage of time lose
water of crystallization (efflorescence) and crumble to white powder.
(c) Iodine reacts with NaOH forming colourless compounds. Thus, the colour of iodine
disappears on addition of NaOH.
2NaOH I2 NaI
NaIO H2O
Colourless products
42. 1.344
46. K1 K2
N2 H2
3
N2 O2 3 H2 O2 1/ 2
The equilibrium constant for
5
2NH3 g O2 g 2NO g 3H2O g
2
NO2 H2O
2 3
K 2 K 33
will be:
NH3 O2
2 5/2
K1
pH = pKa + log
salt 4.6 = pKa + log 5
acid 10
pKa = 4.9
(i) pH of acid solution before addition of any drop of alkali
1 1
pH = [pKa - log C] = [4.9-log 0.5] = 4.6
2 2
(ii) pH of the solution at the end point which is diluted to 150 ml
No. of millimole of salt formed = 15
Volume of solutio = 150 ml
15
[salt] = 0.1 M
150
The salt formed will be hydrolysed to render the solution faintly alkaline. The pOH of
this solution may be calculated as
1 1
pOH = [pKa - pKw - log C] = [4.9-14+1] = 4.05
2 2
pH = 9.95
MCl M +
+ -
49. Cl
a/v a/v
NCl N +
+ -
Cl
b/v b/v
+ +
Now M and N ions undergoes hydrolysis simultaneously
+ +
M + H2O MOH + H
a
v x1 x1 x1 + x2 … (i)
+ + +
Similarity for N , N + H2O NOH + H
b
v x2 x2 x1 + x2
K w x1 x2 x1
From (i) KH1 ss … (iii)
K1 a/v
COOH COO
K1
H2O
H3O
NH3 NH3
0.1 c 0.1 0.1
c H 2 103
K1 C 2 4 10 5
NH 2 NH 2
Na
COONa COO
conjugate base of amino acid
NH2 NH2
Kw / K
H2O 2 OH1
COO
COOH
0.1 c 0.1 0.1
Kw
c 103 , C2 105 K 2 109
K2
Now
COO COOH
H 1
1/ K
+ +
NH3 NH3
COOH COO
K2
H
NH2 NH2
At isoelectric point [C.A.] = [C.B.]
[H ] = K1 K 2 pH = 6.7
+
1. B 2. B 3. C 4. A
5. B 6. D 7. C 8. D
9. B 10. D 11. C 12. D
13. C 14. D 15. D 16. C
17. C 18. B 19. C 20. A
21. D 22. B 23. C 24. D
25. A 26. B 27. A 28. D
29. B 30. D 31. B 32. A
33. B 34. A 35. A 36. B
37. D 38. B 39. D 40. C
41. D 42. D 43. A 44. B
45. A
87. A - 3; B - 1; C - 2; D – 4 88. A – 3; B – 1; C – 2; D – 4
89. A – 4; B – 3; C – 2; D – 1 90. A – 3; B – 1; C – 4; D – 2