0.6 mL of acetic acid (CH3COOH), having density 1.06 g mL-1, is dissolved in 1 litre of water. The depression in freezing point observed for this strength of acid was 0.0205°C. The van’t Hoff factor is

Question

0.6 mL of acetic acid (CH3COOH), having density 1.06 g mL-1, is dissolved in 1 litre of water. The depression in freezing point observed for this strength of acid was 0.0205°C. The van’t Hoff factor is (A) 1 (B) 2 (C) 5 (D) 7

Tardigrade Admin · Accepted Answer

Mass of acetic acid w2 = Volume × Density = 0.6 × 1.06 = 0.636 g We know, Δ T = i × Kf × (w2 × 1000/M2 × w1) ...(i) Given, Δ T = 0.0205, Kf = 1.86 K kg mol -1, w2 = 0.636 g M2 = 60 g mol -1, w1 = 1000 g (Mass of 1 litre water) Putting these values in eqn. (i), we get 0 .0205 = i × 1.86 × (0.636 × 1000/60 × 1000) i = 1.03397

Q. $0.6 m L$ of acetic acid $(C H_{3} COO H)$ , having density $1.06 g m L^{- 1}$ , is dissolved in $1$ litre of water. The depression in freezing point observed for this strength of acid was $0.020 5^{\circ} C$ . The van’t Hoff factor is

$1$

$2$

$5$

$7$

Q. 0.6mL of acetic acid (CH3​COOH), having density 1.06gmL−1, is dissolved in 1 litre of water. The depression in freezing point observed for this strength of acid was 0.0205∘C. The van’t Hoff factor is

1

2

5

7

Q. $0.6 m L$ of acetic acid $(C H_{3} COO H)$ , having density $1.06 g m L^{- 1}$ , is dissolved in $1$ litre of water. The depression in freezing point observed for this strength of acid was $0.020 5^{\circ} C$ . The van’t Hoff factor is

$1$

$2$

$5$

$7$