Nothing Special   »   [go: up one dir, main page]
Scribd Logo
Upload

Welcome to Scribd!

  • 19 views

    MLL Questions

    Uploaded by

    Sanjayraj
    This document contains 22 questions regarding concepts in physical chemistry including: 1) Definitions of molarity and molal elevation constant. 2) Calculations involving mole fraction, molality, and molarity for a 10% glucose solution. 3) Statements of Henry's law and Raoult's law as well as explanations for how temperature affects gas solubility and deviations from ideal behavior. 4) Calculations of boiling point elevations, freezing point depressions, and osmotic pressures for various solutions. 5) Explanations for experimental techniques like osmotic pressure measurements and behaviors of solutions and blood cells in different conditions.

    Copyright:

    © All Rights Reserved
    Download as DOCX, PDF, TXT or read online from Scribd

    MLL Questions

    Uploaded by

    Sanjayraj
    19 views3 pages
    This document contains 22 questions regarding concepts in physical chemistry including: 1) Definitions of molarity and molal elevation constant. 2) Calculations involving mole fraction, molality, and molarity for a 10% glucose solution. 3) Statements of Henry's law and Raoult's law as well as explanations for how temperature affects gas solubility and deviations from ideal behavior. 4) Calculations of boiling point elevations, freezing point depressions, and osmotic pressures for various solutions. 5) Explanations for experimental techniques like osmotic pressure measurements and behaviors of solutions and blood cells in different conditions.

    Original Description:

    Original Title

    MLL QUESTIONS

    Copyright

    © © All Rights Reserved

    Available Formats

    DOCX, PDF, TXT or read online from Scribd

    Did you find this document useful?

    Is this content inappropriate?

    This document contains 22 questions regarding concepts in physical chemistry including: 1) Definitions of molarity and molal elevation constant. 2) Calculations involving mole fraction, molality, and molarity for a 10% glucose solution. 3) Statements of Henry's law and Raoult's law as well as explanations for how temperature affects gas solubility and deviations from ideal behavior. 4) Calculations of boiling point elevations, freezing point depressions, and osmotic pressures for various solutions. 5) Explanations for experimental techniques like osmotic pressure measurements and behaviors of solutions and blood cells in different conditions.

    Copyright:

    © All Rights Reserved
    Download as DOCX, PDF, TXT or read online from Scribd
    Download as docx, pdf, or txt
    19 views3 pages

    MLL Questions

    Uploaded by

    Sanjayraj
    This document contains 22 questions regarding concepts in physical chemistry including: 1) Definitions of molarity and molal elevation constant. 2) Calculations involving mole fraction, molality, and molarity for a 10% glucose solution. 3) Statements of Henry's law and Raoult's law as well as explanations for how temperature affects gas solubility and deviations from ideal behavior. 4) Calculations of boiling point elevations, freezing point depressions, and osmotic pressures for various solutions. 5) Explanations for experimental techniques like osmotic pressure measurements and behaviors of solutions and blood cells in different conditions.

    Copyright:

    © All Rights Reserved
    Download as DOCX, PDF, TXT or read online from Scribd
    Download as docx, pdf, or txt
    of 3

    Q.

    1 Define the following terms:


    (i) Molarity (ii) Molal elevation constant (Kb)

    Q.2 A solution of glucose (molar mass= 180 g mol–1) in water is labeled 10 % (by mass). What
    would be the mole fraction, molality and molarity of the solution?
    (Density of solution = 1.2 g mL–1)

    Q.3 State Henry’s law. Why do gases always tend to be less soluble in liquids as the
    temperature is raised?

    Q.4 How Henry’s constant depends on temperature?

    Q.5 State Raoult's law for a solution containing volatile components. Write two characteristics
    of the solution which obeys Raoult's law at all concentrations.

    Q.6 What type of deviation is shown by a mixture of ethanol and acetone? Give reason.

    Q.7 In non-ideal solution what type of deviation shows the formation of minimum boiling
    Azeotropes.

    Q.8 why a mixture of carbon disulphide and acetone shows a positive deviation from roults
    law? What type of azeotrope is formed by this mixture?

    Q.9 Acetone and chloroform are mixed together then predict that_
    (a) What type of deviation is formed by this solution?
    (b) What type of azeotrope is formed by this solution?

    Q.10 Give reasons for the following:


    (a) Measurement of osmotic pressure method is preferred for the determination of molar
    masses of macromolecules such as proteins and polymers.
    (b) Aquatic animals are more comfortable in cold water than in warm water.
    (c) Elevation of boiling point of 1M KCl solution is nearly double than that of 1 M sugar solution.

    Q.11 On mixing liquid X and liquid Y, the volume of resulting solution increases.
    What type of deviation from Raoult’s law is shown by the resulting solution?
    What change in temperature would you observe after mixing liquids X and Y?

    Q.12 Calculate the boiling points of solution when 2 gm of Na 2SO4 (molecular mass 142
    gm/mol) was dissolved in 50 gm of water assuming Na 2SO4 undergoes complete ionization.
    (Kb for water = 0.52 K Kg mol-1)

    Q.13 Calculate the freezing point of a solution when 20 g of CaCl 2 (M=111 g mol -1) was
    dissolved in 500 g of water, assuming CaCl 2 undergoes complete ionization.
    (Kf for water = 1.86 K kg mol-1)
    Q.14 Calculate the freezing point of a solution containing 60 g glucose (Molar mass = 180
    g mol−1mol-1) in 250 g of water. (Kf of water = 1.86 K kg mol−1)

    Q.15 A 5% solution (by mass) of cane sugar in water has freezing point of 271 K. Calculate the
    freezing point of 5% solution (by mass) of glucose in water
    (Molecular mass: Glucose C6H12O6 : 180 amu; Cane –sugar C12H22O11: 342 amu)

    Q.16 3.9 g of benzoic acid dissolved in 49 g of benzene shows a depression in freezing point of
    1.62K. Calculate the van’t Hoff factor and predict the nature of solute (associated or
    dissociated)
    (Given molar mass of benzoic acid = 122 g mol -1, Kf for benzene = 4.9 K kg mol -1)

    Q.17 Calculate the mass of ascorbic acid (Vitamin C, C 6H8O6) to be dissolved in 75 g of acetic
    acid to lower its melting point by 1.5°C. Kf = 3.9 K kg mol-1.

    Q.18 Visha took two aqueous solutions one containing 7.5g of urea and the other containing
    42.57 g of substance Z in 100g of water, respectively. It was observed that both the solutions
    froze at the same temperature. Calculate the molar mass if Z.

    Q.19 (a) What happens when blood cells are placed in pure water (hypotonic)?
    (b) When a pressure higher than the osmotic pressure is applied on the surface of the solution
    separated from a solvent by semi permeable membrane, what will happen?

    Q.20 For a 5% solution of urea (Molar mass = 60 g/mol), calculate the osmotic pressure at 300
    K. (R = 0·0821 L atm K-1 mol-1)

    Q.21 A solution containing 15 g urea (molarmass= 60 g mol –1) per liter solution in water has the
    Same osmotic pressure (isotonic) as a solution of glucose (molarmass= 180 g mol –l) in water.
    Calculate the mass of glucose present in one liter of its solution.

    Q.22

    You might also like