Unit 1: Solutions

 Unit 1: Solutions 

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Section 1: Types of Solutions & Concentration Terms

1. Which of the following concentration units is independent of temperature? A) Molarity B) Normality C) Molality D) Formality

2. An example of a solid solution (solid in solid) is: A) Salt in water B) Brass (Alloy) C) Camphor in nitrogen D) Aerated drinks

3. The number of moles of solute dissolved in 1 kg of solvent is called: A) Molarity B) Molality C) Mole fraction D) Normality

4. Which of the following is a 'Liquid in Solid' type solution? A) Fog B) Smoke C) Amalgam of mercury with sodium D) Dissolved oxygen in water

5. The sum of the mole fractions of all components in a solution is always: A) 0 B) 1 C) 100 D) Varies with temperature

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Section 2: Solubility of Gases in Liquids (Henry's Law)

6. According to Henry's Law, the solubility of a gas in a liquid is directly proportional to: A) The volume of the liquid B) The partial pressure of the gas C) The density of the gas D) The molecular mass of the gas

7. With an increase in temperature, the solubility of gases in liquids generally: A) Increases B) Decreases C) Remains constant D) First increases then decreases

8. Scuba divers use tanks diluted with Helium to avoid a painful condition called: A) Anoxia B) Bends C) Hyperoxia D) Nitrogen narcosis

9. The Henry’s Law constant (KH) value: A) Is the same for all gases B) Increases with an increase in temperature C) Decreases with an increase in temperature D) Is independent of the nature of the gas

10. Low blood oxygen levels in climbers at high altitudes (Anoxia) is caused by: A) High atmospheric pressure B) Low partial pressure of oxygen C) Low temperature D) High humidity

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Section 3: Raoult's Law & Ideal Solutions

11. Raoult's Law states that for a solution of volatile liquids, the partial vapor pressure of each component is proportional to its: A) Molarity B) Molality C) Mole fraction D) Weight percentage

12. For an ideal solution, which of the following is TRUE? A) ΔH_mixing > 0 B) ΔV_mixing < 0 C) ΔH_mixing = 0 and ΔV_mixing = 0 D) It obeys Henry’s law only

13. A mixture of Ethanol and Acetone shows: A) Positive deviation from Raoult's Law B) Negative deviation from Raoult's Law C) Ideal behavior D) No vapor pressure

14. A mixture of Chloroform and Acetone shows negative deviation because: A) Heat is absorbed B) Intermolecular H-bonding is formed between components C) Molecules repel each other D) Volume increases upon mixing

15. Constant boiling mixtures that distill without change in composition are called: A) Ideal solutions B) Azeotropes C) Isotonic solutions D) Saturated solutions

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Section 4: Colligative Properties

16. Colligative properties depend only on: A) Nature of the solute B) Nature of the solvent C) Number of solute particles D) Chemical properties of the solute

17. The relative lowering of vapor pressure is equal to: A) Molarity of solute B) Mole fraction of solute C) Molality of solute D) Mole fraction of solvent

18. The unit of Molal Elevation Constant (Kb) is: A) K kg mol B) K kg mol⁻¹ C) mol kg⁻¹ K⁻¹ D) K mol kg⁻¹

19. The process of movement of solvent molecules through a semi-permeable membrane is: A) Diffusion B) Osmosis C) Effusion D) Sedimentation

20. Isotonic solutions have the same: A) Boiling point B) Freezing point C) Osmotic pressure D) Vapor pressure

21. Which property is best used to determine the molecular mass of polymers and proteins? A) Elevation of boiling point B) Depression of freezing point C) Osmotic pressure D) Relative lowering of vapor pressure

22. The freezing point of a solution is ______ than that of the pure solvent. A) Higher B) Lower C) Equal D) Twice

23. Adding salt to ice helps in clearing snowy roads because it: A) Increases the melting point B) Lowers the freezing point of water C) Acts as a catalyst for melting D) Increases the vapor pressure

24. Reverse Osmosis (RO) occurs when the applied pressure is: A) Equal to osmotic pressure B) Less than osmotic pressure C) Greater than osmotic pressure D) Zero

25. The osmotic pressure (π) of a solution is given by the equation: A) π = MRT B) π = CRT (where C is molarity) C) π = nRT D) π = Kb × m

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Section 5: Van't Hoff Factor & Abnormal Molecular Mass

26. The Van't Hoff factor (i) for a non-electrolyte (like glucose) is: A) 0 B) 1 C) 2 D) 0.5

27. If a solute undergoes dissociation in a solution, the value of 'i' will be: A) i < 1 B) i > 1 C) i = 1 D) i = 0

28. The Van't Hoff factor (i) for BaCl₂ (assuming 100% dissociation) is: A) 1 B) 2 C) 3 D) 4

29. When acetic acid dimerizes in benzene, its Van't Hoff factor (i) is: A) More than 1 B) Less than 1 C) Equal to 1 D) Equal to 2

30. Abnormal molar mass is observed when: A) The solution is ideal B) Solute undergoes association or dissociation C) The solution is very dilute D) The solute is non-volatile

31. The correct relationship for 'i' is: A) i = Normal Molar Mass / Observed Molar Mass B) i = Observed Molar Mass / Normal Molar Mass C) i = Calculated Colligative Property / Observed Colligative Property D) i = Moles before dissociation / Moles after dissociation

32. Which of the following will have the highest boiling point? A) 0.1 M Glucose B) 0.1 M NaCl C) 0.1 M Na₂SO₄ D) 0.1 M Urea

33. Which of the following 0.1 M aqueous solutions will have the lowest freezing point? A) Al₂(SO₄)₃ B) NaCl C) KCl D) Glucose

34. If i = 1 + α(n-1), what does 'α' represent? A) Mole fraction B) Degree of dissociation C) Molality D) Osmotic constant

35. The Van't Hoff factor for K₄[Fe(CN)₆] (complete dissociation) is: A) 4 B) 5 C) 6 D) 1

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Section 6: General Concepts & Calculations

36. Ebullioscopic constant is another name for: A) Cryoscopic constant B) Molal elevation constant C) Henry’s constant D) Gas constant

37. A plant cell shrinks when placed in a hypertonic solution due to: A) Endosmosis B) Exosmosis C) Diffusion D) Absorption

38. The vapor pressure of a pure solvent is ______ than the vapor pressure of its solution. A) Higher B) Lower C) Same D) Half

39. Cryoscopic constant (Kf) depends upon: A) Nature of solute B) Nature of solvent C) Pressure D) Concentration

40. For a non-volatile solute, which property is directly proportional to its molality? A) Relative lowering of vapor pressure B) Elevation of boiling point C) Osmotic pressure D) All of the above

41. 0.91% (w/v) NaCl solution is ______ with human blood. A) Hypertonic B) Hypotonic C) Isotonic D) Saturated

42. Maximum boiling azeotropes are formed by solutions showing: A) Positive deviation B) Negative deviation C) Ideal behavior D) No deviation

43. Semi-permeable membranes allow the passage of: A) Solute particles only B) Solvent molecules only C) Both solute and solvent D) Neither solute nor solvent

44. Which of the following is not a colligative property? A) Osmotic pressure B) Surface tension C) Depression in freezing point D) Relative lowering in vapor pressure

45. Parts per million (ppm) is used to express the concentration of: A) Concentrated acids B) Trace pollutants in water C) Solid alloys D) Saturated sugar solution

46. What is the molality of pure water? A) 18 B) 55.5 C) 100 D) 1

47. Camphor in Nitrogen gas is an example of: A) Gas in Liquid B) Solid in Gas C) Liquid in Gas D) Solid in Solid

48. Raoult's Law becomes a special case of Henry's Law when: A) KH = P° B) KH = 1 C) P° = 0 D) Molality is 1

49. Which of the following shows a decrease in volume on mixing? A) Ethanol + Water B) Chloroform + Acetone C) Benzene + Toluene D) n-Hexane + n-Heptane

50. The molar mass determined by colligative properties is 'abnormal' when the solute: A) Is non-volatile B) Associates or dissociates in the solvent C) Does not dissolve completely D) Is in the gaseous state

Unit 1: Solutions - NEET Level MCQs

I. Concentration Terms & Solubility

1. The molarity of a solution obtained by mixing 750 mL of 0.5 M HCl with 250 mL of 2 M HCl is: A) 0.875 M B) 1.0 M C) 1.75 M D) 0.975 M
2. What is the molality of a 15% (w/w) solution of $H_{2}S{O}_4$ (Molecular mass = 98)? A) 1.2 mol/kg B) 1.8 mol/kg C) 1.5 mol/kg D) 2.1 mol/kg
3. Density of a 2.03 M cane sugar solution is 1.063 g/mL. Its molality is: A) 2.97 m B) 3.12 m C) 2.03 m D) 2.51 m
4. The value of Henry's constant $K_H$ is: A) Greater for gases with higher solubility. B) Greater for gases with lower solubility. C) Constant for all gases. D) Not related to the nature of the gas.
5. Which of the following units is used for reporting the concentration of trace pollutants in water? A) Molarity B) Molality C) ppm D) Mole fraction

II. Raoult's Law & Ideal/Non-Ideal Solutions

1. For an ideal solution, the correct condition is: A) $\Delta H_{mix}=0,\Delta V_{mix}=0,\Delta S_{mix}=0$ B) $\Delta H_{mix}=0,\Delta V_{mix}=0,\Delta G_{mix}<0$ C) $\Delta H_{mix}>0,\Delta V_{mix}>0$ D) $\Delta H_{mix}<0,\Delta V_{mix}<0$
2. A mixture of $CHC{l}_3$ and $C{H}_{3}COC{H}_3$ (acetone) shows negative deviation from Raoult's law because: A) $A-A$ and $B-B$ interactions are stronger than $A-B$. B) $A-B$ interaction is stronger than $A-A$ and $B-B$ due to H-bonding. C) It forms a minimum boiling azeotrope. D) The molecules are identical in size.
3. Which of the following liquid pairs shows a positive deviation from Raoult's law? A) Water + Nitric acid B) Benzene + Methanol C) Water + HCl D) Acetone + Chloroform
4. Maximum boiling azeotropes are formed by: A) Ideal solutions B) Solutions with positive deviation C) Solutions with negative deviation D) Non-volatile solutes
5. At a given temperature, the total vapor pressure of a solution containing components A and B is $P=120-75x_B$. The vapor pressure of pure A ($P_A^o$) is: A) 120 B) 75 C) 45 D) 195

III. Colligative Properties (VP, BP, FP)

1. Relative lowering of vapor pressure is a colligative property because: A) It depends on the concentration of a non-electrolyte solute. B) It depends on the number of particles of solute. C) It is the ratio of vapor pressure of solution to solvent. D) It depends on the nature of the solute.
2. The vapor pressure of water at $20^{o}C$ is 17.5 mm Hg. When 18 g of glucose is added to 178.2 g of water at $20^{o}C$, the vapor pressure of the solution will be: A) 17.675 mm Hg B) 17.325 mm Hg C) 15.5 mm Hg D) 17.0 mm Hg
3. Which solution will have the highest boiling point? A) 1% Glucose in water B) 1% $NaCl$ in water C) 1% $CaC{l}_2$ in water D) 1% Sucrose in water
4. The molal elevation constant ($K_b$) depends on: A) Nature of solute B) Nature of solvent C) Enthalpy of solution D) Molarity
5. If the elevation in boiling point of a solution of non-volatile, non-electrolyte solute in solvent is $0.8^{o}C$, then the depression in freezing point of the same solution would be ($K_b=0.52,K_f=1.86$): A) $2.86^{o}C$ B) $1.86^{o}C$ C) $0.8^{o}C$ D) $0.52^{o}C$
6. Why is the molecular mass of a polymer determined by osmotic pressure rather than other colligative properties? A) Change in freezing point is too large to measure. B) Osmotic pressure is large enough to be measured at room temperature. C) Polymers are insoluble at high temperatures. D) Polymers dissociate at high temperatures.
7. A $5\%$ solution of cane sugar (MW = 342) is isotonic with $0.877\%$ solution of urea. The molecular weight of urea is: A) 60 B) 30 C) 90 D) 120
8. The osmotic pressure of a solution can be increased by: A) Increasing volume B) Increasing temperature C) Decreasing solute amount D) Increasing solvent amount
9. Blood cells retain their normal shape in solution which are: A) Hypotonic to blood B) Isotonic to blood C) Hypertonic to blood D) Equimolar to blood
10. Which of the following $0.10$ M aqueous solutions will exhibit the largest freezing point depression? A) $KCl$ B) $C_6{H}_{12}{O}_6$ C) $A{l}_2(S{O}_4{)}_3$ D) $K_{2}S{O}_4$

IV. Van't Hoff Factor & Abnormal Molar Mass

1. The Van't Hoff factor ($i$) for a dilute solution of $K_4[Fe(CN{)}_6]$ is: A) 4 B) 5 C) 3 D) 2
2. If '$\alpha$' is the degree of dissociation of $N{a}_{2}S{O}_4$, the Van't Hoff factor ($i$) used for calculating molecular mass is: A) $1+\alpha$ B) $1-\alpha$ C) $1+2\alpha$ D) $1-2\alpha$
3. The Van't Hoff factor ($i$) for a compound which undergoes dimerization in benzene is: A) 0.5 B) 1.5 C) 2 D) 1
4. Which of the following has $i=1$? A) $NaCl$ B) Urea C) $CaC{l}_2$ D) $C{H}_{3}COOH$ in water
5. The ratio of the colligative property of $BaC{l}_2$ solution to that of sucrose solution of same molar concentration is: A) 1 B) 2 C) 3 D) 0.5
6. For which of the following solutes is the observed molar mass less than the theoretical molar mass? A) Glucose B) $KCl$ C) Benzoic acid in benzene D) Sucrose
7. A $0.004$ M solution of $N{a}_{2}S{O}_4$ is isotonic with a $0.010$ M solution of glucose. The degree of dissociation of $N{a}_{2}S{O}_4$ is: A) $75\%$ B) $85\%$ C) $50\%$ D) $25\%$
8. The Van't Hoff factor ($i$) for a $0.1$ M $A{l}_2(S{O}_4{)}_3$ solution is $4.20$. The degree of dissociation is: A) $80\%$ B) $90\%$ C) $70\%$ D) $100\%$
9. Which property is used to calculate the degree of association or dissociation? A) Surface tension B) Viscosity C) Van't Hoff factor D) Refractive index
10. In the case of association, the observed colligative property is: A) Higher than calculated B) Lower than calculated C) Same as calculated D) Zero

V. Advanced Conceptual & Numerical Mix

1. $12$ g of a non-volatile solute dissolved in $108$ g of water produces a relative lowering of vapor pressure of $0.1$. The molecular mass of the solute is: A) 20 B) 40 C) 60 D) 80
2. A solution of $CaC{l}_2$ and $NaCl$ are both $0.1$ M. If the osmotic pressure of $NaCl$ is $P_1$ and that of $CaC{l}_2$ is $P_2$, then: A) $P_1=P_2$ B) $P_1>P_2$ C) $P_2>P_1$ D) $P_1=2P_2$
3. Which has the minimum freezing point? A) 1 M $NaCl$ B) 1 M $KCl$ C) 1 M $CaC{l}_2$ D) 1 M $AlC{l}_3$
4. If $K_f$ for water is $1.86$, the freezing point of $0.1$ m $NaCl$ solution (assuming $100\%$ ionization) is: A) $-1.86^{o}C$ B) $-0.372^{o}C$ C) $-0.186^{o}C$ D) $-3.72^{o}C$
5. The vapor pressure of pure benzene is $640$ mm Hg. $2.175$ g of a non-volatile solute is added to $39$ g of benzene, and the vapor pressure of the solution becomes $600$ mm Hg. The molar mass of the solute is: A) 65.25 B) 130.5 C) 45 D) 90
6. $0.1$ m solution of $Pt(N{H}_3{)}_{4}C{l}_4$ in water freezes at $-0.558^{o}C$. $K_f$ for water is $1.86$. The number of ions produced per molecule of the complex is: A) 1 B) 2 C) 3 D) 4
7. For a dilute solution, Raoult's law states that: A) The lowering of vapor pressure is equal to the mole fraction of solute. B) The relative lowering of vapor pressure is equal to the mole fraction of solute. C) The vapor pressure of solution is equal to the mole fraction of solvent. D) The vapor pressure of solution is proportional to the mole fraction of solute.
8. The unit of cryoscopic constant ($K_f$) is: A) $K$ B) $kg/mol$ C) $Kkg/mol$ D) $mol/kgK$
9. Henry's Law is NOT applicable if: A) The gas is highly soluble. B) The gas reacts chemically with the solvent. C) The pressure is very high. D) All of the above.
10. Equimolar solutions in the same solvent have: A) Different boiling points B) Same boiling points C) Same freezing points D) Both B and C (for non-electrolytes)
11. Direction of osmosis can be reversed by applying pressure: A) Lower than osmotic pressure on solution side. B) Higher than osmotic pressure on solution side. C) Equal to osmotic pressure on solvent side. D) Higher than atmospheric pressure on solvent side.
12. Azeotropic mixtures are: A) Liquid mixtures that boil at a constant temperature. B) Binary mixtures having the same composition in liquid and vapor phase. C) Also called constant boiling mixtures. D) All of the above.
13. Sea water can be converted into fresh water by: A) Osmosis B) Reverse Osmosis C) Diffusion D) Filtration
14. Which of the following is an example of a gas in solid solution? A) Solution of hydrogen in palladium B) Solution of camphor in nitrogen C) Solution of iodine in alcohol D) All of the above
15. When $Hg{I}_2$ is added to $KI$ solution, the freezing point: A) Lowers B) Increases C) Remains same D) Becomes zero
16. $0.6$ g of urea was dissolved in $9.9$ g of water. If the vapor pressure of pure water is $P^o$, the vapor pressure of solution is: A) $0.10P^o$ B) $1.10P^o$ C) $0.98P^o$ D) $0.90P^o$
17. The elevation in boiling point of $0.01$ M $BaC{l}_2$ solution is about ______ times that of $0.01$ M glucose solution. A) 1 B) 2 C) 3 D) 5
18. $X$ g of a non-electrolyte (MW = 40) is dissolved in $100$ g of water. If $\Delta T_b$ is $0.52^{o}C$ and $K_b$ for water is $0.52$, the value of $X$ is: A) 4 g B) 40 g C) 10 g D) 20 g
19. In cold countries, ethylene glycol is added to water in car radiators. This helps to: A) Reduce the boiling point B) Lower the freezing point C) Act as a fuel D) Clean the engine
20. At high altitudes, the boiling point of water decreases because: A) Atmospheric pressure is high. B) Atmospheric pressure is low. C) Temperature is low. D) Oxygen content is low.
21. JEE Level MCQs: Unit 1 - Solutions
    I. Advanced Concentration & Mixing
    1. A 1000g sample of a solution contains 0.1 moles of solute. If the density of the solution is $d$ g/mL, the molarity ($M$) and molality ($m$) are related by: A) $M=m(1000d/(1000+m\cdot MW))$ B) $m=1000M/(1000d-M\cdot MW)$ C) Both A and B D) $M=m\cdot d$
    2. Calculate the mole fraction of a solute in a 2.0 m aqueous solution. A) 0.0347 B) 0.036 C) 0.045 D) 0.018
    3. How many grams of $N{a}_{2}C{O}_3$ (MW=106) should be dissolved in 250g of water to prepare a 0.1 m solution? A) 2.65g B) 1.06g C) 5.30g D) 0.265g
    4. Which concentration term changes with temperature for a solution containing a volatile solute and a non-volatile solvent? A) Mole fraction B) Molality C) Weight percentage D) Molarity
    5. A solution of $H_{2}S{O}_4$ is 98% by weight and has a density of 1.84 g/mL. The volume of this acid required to make 1L of 0.1 M $H_{2}S{O}_4$ is: A) 10 mL B) 5.43 mL C) 18.4 mL D) 2.5 mL
    II. Solubility & Henry’s Law
    1. The Henry's law constant for $O_2$ in water is $4.34\times 10^4$ atm at 25°C. If the partial pressure of $O_2$ in air is 0.2 atm, calculate the concentration (in mole fraction) of dissolved $O_2$. A) $4.6\times 10^{-6}$ B) $2.1\times 10^{-4}$ C) $1.5\times 10^{-5}$ D) $8.6\times 10^{-5}$
    2. A gas $X$ is bubbled through water at 293 K. $K_H$ for $X$ is 100 kbar. If the gas exerts a partial pressure of 0.98 bar, how many millimoles of $X$ dissolve in 1L of water? A) 0.54 B) 0.45 C) 0.98 D) 1.2
    3. Considering Henry's law, which of the following is correct for a gas dissolving in a liquid? A) $\Delta G<0,\Delta S<0,\Delta H<0$ B) $\Delta G<0,\Delta S>0,\Delta H<0$ C) $\Delta G<0,\Delta S<0,\Delta H>0$ D) $\Delta G>0,\Delta S<0,\Delta H<0$
    III. Raoult’s Law & Binary Mixtures
    1. Two liquids A and B form an ideal solution. At 300 K, the vapor pressure of a solution containing 1 mole of A and 3 moles of B is 550 mm Hg. At the same temperature, if 1 more mole of B is added, the vapor pressure increases to 560 mm Hg. The vapor pressures of pure A and B ($P_A^o,P_B^o$) are: A) 400, 600 B) 600, 400 C) 500, 500 D) 450, 550
    2. The vapor pressure of a pure liquid A is 40 mm Hg at 310 K. The vapor pressure of this liquid in a solution with liquid B is 32 mm Hg. If the solution obeys Raoult's law, the mole fraction of B in the solution is: A) 0.8 B) 0.2 C) 0.4 D) 0.5
    3. For a non-ideal solution showing positive deviation from Raoult's law: A) $P_{total}>P_A^o{X}_A+P_B^o{X}_B$ B) $\Delta V_{mix}>0$ C) $\Delta H_{mix}>0$ D) All of the above
    4. In a binary solution of A and B, if $A-B$ interactions are weaker than $A-A$ and $B-B$ interactions, then: A) The solution will show negative deviation. B) The boiling point will be higher than expected. C) The vapor pressure will be higher than predicted by Raoult's law. D) Mixing will be exothermic.
    5. Benzene and Toluene form an ideal solution. The vapor pressure of pure benzene is 100 torr and pure toluene is 40 torr. In a solution where the mole fraction of benzene is 0.5, the mole fraction of benzene in the vapor phase ($Y_{benzene}$) is: A) 0.50 B) 0.71 C) 0.29 D) 0.60
    IV. Azeotropes & Non-Ideal Behavior
    1. A mixture of two liquids A and B has a boiling point higher than the boiling points of both A and B. This mixture is: A) An ideal solution. B) A minimum boiling azeotrope. C) A maximum boiling azeotrope. D) A solution showing positive deviation.
    2. Which of the following forms a maximum boiling azeotrope? A) $H_{2}O+C_2{H}_{5}OH$ B) $C_6{H}_6+C_6{H}_{5}C{H}_3$ C) $HCl+H_{2}O$ D) $C_2{H}_{5}Br+C_2{H}_{5}I$
    3. At a specific composition, a solution of $HN{O}_3$ and $H_{2}O$ behaves like a pure liquid. This implies: A) It is an ideal solution. B) The vapor has the same composition as the liquid. C) It can be separated by simple distillation. D) $\Delta H_{mix}=0$.
    V. Colligative Properties & Van't Hoff Factor
    1. The Van't Hoff factor for a $0.1$ M $Ba(N{O}_3{)}_2$ solution is 2.74. The degree of dissociation ($\alpha$) is: A) 87% B) 74% C) 91% D) 100%
    2. Which of the following aqueous solutions will have the highest boiling point? A) 0.1 M $N{a}_{2}S{O}_4$ B) 0.1 M $K_4[Fe(CN{)}_6]$ C) 0.1 M $A{l}_2(S{O}_4{)}_3$ D) 0.1 M $NaCl$
    3. If the elevation in boiling point of a solution of a non-volatile solute in a solvent ($K_b=0.52$) is $0.156^{o}C$, then the depression in freezing point of the same solution ($K_f=1.86$) will be: A) $0.558^{o}C$ B) $0.156^{o}C$ C) $1.86^{o}C$ D) $0.052^{o}C$
    4. The osmotic pressure of a decinormal ($0.1$ N) solution of $BaC{l}_2$ at 27°C is (assume $i=2.5$): A) 3.08 atm B) 6.15 atm C) 1.23 atm D) 4.56 atm
    5. $1.0$ g of a non-electrolyte solute (MW = 250) was dissolved in $51.2$ g of benzene. If $K_f$ for benzene is $5.12$ K kg/mol, the freezing point depression ($\Delta T_f$) is: A) 0.2 K B) 0.4 K C) 0.5 K D) 0.8 K
    6. What is the freezing point of a solution containing $0.5$ g $KCl$ in $100$ g water ($K_f=1.86$)? Assume $KCl$ is 100% ionized. A) $-0.25^{o}C$ B) $-0.124^{o}C$ C) $-0.248^{o}C$ D) $-0.496^{o}C$
    7. The molar mass of a solute determined by measuring the elevation of boiling point is found to be double the actual molar mass. This indicates the solute has: A) Dissociated into two particles. B) Associated into a dimer. C) Remained unchanged. D) Reacted with the solvent.
    8. For a $1$ m aqueous solution of the following compounds, which one will show the maximum freezing point depression? A) $[Co(N{H}_3{)}_6]C{l}_3$ B) $[Co(N{H}_3{)}_{5}Cl]C{l}_2$ C) $[Co(N{H}_3{)}_{4}C{l}_2]Cl$ D) $[Co(N{H}_3{)}_{3}C{l}_3]$
    9. The relative lowering of vapor pressure of a dilute aqueous solution of glucose is 0.018. The molality of the solution is: A) 1.01 m B) 1.0 m C) 0.18 m D) 0.018 m
    10. Calculate the osmotic pressure of a solution obtained by mixing 100 mL of 0.1 M $CaC{l}_2$ and 100 mL of 0.1 M $N{a}_{2}S{O}_4$ at 300 K (assume complete dissociation and no precipitation). A) 7.38 atm B) 4.92 atm C) 3.69 atm D) 12.3 atm
    11. A certain non-volatile solute associates in benzene. If the degree of association is 0.8 and it forms tetramers, the Van't Hoff factor $i$ is: A) 0.2 B) 0.4 C) 0.6 D) 0.8
    12. Which of the following has the lowest freezing point? A) 0.1 m $C{a}_3(P{O}_4{)}_2$ B) 0.1 m $A{l}_2(S{O}_4{)}_3$ C) 0.1 m $K_3[Fe(CN{)}_6]$ D) 0.1 m $MgS{O}_4$
    13. At 25°C, the highest osmotic pressure is exhibited by 0.1 M solution of: A) $CaC{l}_2$ B) $KCl$ C) Glucose D) Urea
    14. If $K_b$ of a solvent is $X$ K kg/mol, then the elevation in boiling point of a $0.2$ m solution of a non-electrolyte solute is: A) $0.1X$ B) $0.2X$ C) $0.5X$ D) $X$
    VI. Thermodynamic & Complex Numericals
    1. For the process of dissolving a non-volatile solute in a liquid solvent, which of the following is always TRUE? A) $\Delta H_{soln}<0$ B) $\Delta S_{soln}>0$ C) $\Delta G_{soln}<0$ D) $\Delta V_{soln}=0$
    2. A solution of two volatile liquids A and B obeys $P_{total}=100+50X_A$. The ratio of $P_A^o/P_B^o$ is: A) 1.5 B) 0.5 C) 2.0 D) 3.0
    3. The vapor pressure of water at 25°C is 24 mm Hg. If 1 mole of a non-ionic solute is dissolved in 9 moles of water, the vapor pressure of the solution is: A) 21.6 mm Hg B) 2.4 mm Hg C) 24 mm Hg D) 20 mm Hg
    4. The cryoscopic constant ($K_f$) of water is $1.86$ K kg/mol. A $0.01$ molal solution of a complex $CoC{l}_3\cdot 6N{H}_3$ freezes at $-0.0744^{o}C$. The number of chloride ions in the coordination sphere is: A) 0 B) 1 C) 2 D) 3
    5. The freezing point of a $0.08$ molal solution of $NaHS{O}_4$ is $-0.372^{o}C$. $K_f$ for water is $1.86$. The Van't Hoff factor is: A) 2.0 B) 2.5 C) 3.0 D) 1.5
    6. Two solutions, 0.1 M urea and 0.1 M sucrose, are separated by a semi-permeable membrane. Which of the following will occur? A) Water flows from urea to sucrose. B) Water flows from sucrose to urea. C) There is no net movement of water. D) Urea moves to the sucrose side.
    7. A $1.17\%$ NaCl solution is isotonic with a $7.2\%$ solution of a non-electrolyte. The molar mass of the non-electrolyte is: A) 180 B) 342 C) 60 D) 120
    8. Which of the following will have the same boiling point as 0.1 M $NaCl$ solution? A) 0.1 M $N{a}_{2}S{O}_4$ B) 0.1 M Glucose C) 0.1 M $MgC{l}_2$ D) 0.1 M $KCl$
    9. The vapor pressure of a solution of a non-volatile solute is 90% of the vapor pressure of the pure solvent. The molality of the solution is: A) 6.17 m B) 5.55 m C) 1.11 m D) 0.9 m
    10. The molal elevation constant of a solvent is the elevation in boiling point produced by dissolving: A) 1g solute in 100g solvent. B) 1 mole solute in 1L solvent. C) 1 mole solute in 1kg solvent. D) 1 mole solute in 1kg solution.
    11. Reverse osmosis is used in: A) Water purification B) Determining MW of protein C) Concentration of fruit juices D) Both A and C
    12. An ideal solution is formed when its components: A) Have the same molecular size. B) Have similar intermolecular forces. C) Show no volume change on mixing. D) All of the above.
    13. A $0.2$ M aqueous solution of a weak acid (HX) is 20% ionized. The freezing point of this solution is ($K_f=1.86$): A) $-0.45^{o}C$ B) $-0.37^{o}C$ C) $-0.53^{o}C$ D) $-0.22^{o}C$
    14. The elevation of boiling point for $13.44$ g of $CuC{l}_2$ (MW = 134.4) in 1 kg of water using $K_b=0.52$ is (assume $i=3$): A) $0.052$ B) $0.156$ C) $0.104$ D) $0.208$
    15. Which of the following statements about $K_b$ is FALSE? A) It is called the Ebullioscopic constant. B) It depends on the boiling point of the solvent. C) It is a property of the solute. D) Its units are K kg/mol.
    16. The degree of dissociation of $Ca(N{O}_3{)}_2$ in a dilute aqueous solution, containing $7$ g of the salt per $100$ g of water at 100°C, is 70%. If the vapor pressure of water at 100°C is 760 mm Hg, the vapor pressure of the solution is: A) 746 mm Hg B) 750 mm Hg C) 740 mm Hg D) 755 mm Hg
    17. $1$ mole of liquid A and $2$ moles of liquid B are mixed. The vapor pressure of the solution is found to be 300 torr. $P_A^o=400$ torr and $P_B^o=200$ torr. The solution is: A) Ideal B) Showing positive deviation C) Showing negative deviation D) Saturated
    18. Calculate the percentage of $N{a}_{2}S{O}_4$ in a mixture of $N{a}_{2}S{O}_4$ and glucose if the mixture is isotonic with $1$ M $MgC{l}_2$ (assume 100% ionization for salts). A) Insufficient data B) 50% C) 25% D) 75%
    19. In the depression of freezing point experiment, it is found that: A) The vapor pressure of the solution is less than that of pure solvent. B) Only solvent molecules solidify at the freezing point. C) Only solute molecules solidify at the freezing point. D) Both A and B.
    20. At high altitude, water boils at 95°C. To make water boil at 100°C, the amount of $NaCl$ added to 1 kg of water ($K_b=0.52$) should be approximately: A) 280g B) 140g C) 58.5g D) 100g