# MCQ | Liquid Solution

Practice Test-I
Q:1. Which salt may show the same value of vant Hoff factor (i) as that of K4Fe(CN)6 in very dilute solution state:
(A) Al2(SO4)3

(B) NaCl

(C) Al(NO3)3

(D) Na2SO4

Ans: (A)

Q:2. Two solutions of KNO3 and CH3COOH are prepared separately. Molarity of both is 0.1 M and osmotic pressures are P1 and P2 respectively. The correct relationship between the osmotic pressures is:

(A) P2 > P1

(B) P1 = P2

(C) P1 > P2

(D) $\large \frac{P_1}{P_1 + P_2} = \frac{P_2}{P_1 + P_2}$

Ans: (C)

Q:3. The process of getting fresh water from sea water is known as

(A) Osmosis

(B) Filtration

(C) Desaltation

(D) Reverse Osmosis

Ans: (D)

Q:4. Equimolal solutions of A and B show depression in freezing point in the ratio 2:1. A remains in its normal state in solution. B will be …….. state

(A) Normal

(B) Dissociated

(C) Associated

(D) Hydrolysis

Ans: (C)

Q:5. The wt. of urea dissolved in 100 ml solution which produce an osmotic pressure of 20.4 atm, will be

(A) 5 g

(B) 4 g

(C) 3 g

(D) 6 g

Ans: (A)

Q:6. Which of the following solution will have highest freezing point ?

(A) 2 M NaCl solution

(B) 1.5 M AlCl3 solution

(C) 1 M Al2(SO4)3 Solution

(D) 3 M Urea Solution

Ans: (D)

Q:7. The degree of dissociation (α) of a weak electrolyte AxBy is related to Vant’s Hoff factor(i) by the expression

(A) $\large \alpha = \frac{i+1}{x+y-1}$

(B) $\large \alpha = \frac{i-1}{x+y-1}$

(C) $\large \alpha = \frac{x+y-1}{i-1}$

(D) $\large \alpha = \frac{x+y+1}{i-1}$

Ans: (B)

Q:8. The freezing point of 0.05 m solutions of a non-electrolyte in water is

(A) –1.86°C

(B) –0.93°C

(C) –0.093°C

(D) 0.93°C

Ans: (C)

Q:9. Which of the following aqueous solutions has osmotic pressure nearest to that of an equimolar solution of K4[Fe(CN)6]

(A) Na2SO4

(B) BaCl2

(C) Al2(SO4)3

(D)C12H22O11

Ans: (C)

Q:10. 0.48 g of a substance is dissolved in 10.6 g of C6H6 . The freezing point of benzene is lowered by 1.8°C. What will be the mol. wt. of the substance (Kf for benzene = 5)

(A) 250.2

(B) 90.8

(C) 125.79

(D) 102.5

Ans: (C)

Q:11. Which aqueous solution would posses the lowest boiling point.

(A) 1 \$ NaCl solution

(B) 1 % Urea solution

(B) 1 % Glucose solution

(D) 1 % Sucrose solution

Ans: (D)

Q:12. The relationship between Osmotic pressure at 273 K when 10 gm of glucose (P1), 10 gm urea (P2) and 10 gm sucrose (P3) are dissolved in 250 ml of water is

(A) P1 > P2 > P3

(B) P3 > P1 > P2

(C) P2 > P1 > P3

(D) P2 > P3 > P1

Ans: (C)

Q:13. In which mode of expression of concentration of a solution remains independent of temperature ?

(A) Molarity

(B) Normality

(C) Formality

(D) Molality

Ans: (D)

Q:14. An aqueous solution boils at 100.50°C. The freezing point of the solution would be (Kb for water = 0.51°C/m), (Kf for water = 1.86°C/m) [No association or dissociation]

(A) 0°C

(B) -1.86°C

(C) -1.82°C

(D) +1.82°C

Ans: (B)

Q:15. An ideal solution has equal mol-fractions of two volatile components A and B. In the vapour above the solution, the mol-fractions of A and B:

(A) Are both 0.50

(B) Are equal but necessarily 0.50

(C) Are not very likely to be equal

(D) Are 1.00 and 0.00 respectively