The pH of 0.001( N ) acetic acid solution, which is 10 % dissociated. is

Question

The pH of 0.001( N ) acetic acid solution, which is 10 % dissociated. is (A) 3 (B) 1 (C) 4 (D) 2

Tardigrade Admin · Accepted Answer

Concentration of acetic acid =0.001 N for 10 % dissociation, the effective concentration of H + is one-tenth of total concentration. Therefore concentration =(1/10) × 0.001 N =0.0001 N ⇒ pH = - log [ H +]=4

Q. The pH of $0.001 (N)$ acetic acid solution, which is $10%$ dissociated. is

3

1

4

2

Concentration of acetic acid $= 0.001 N$ for $10%$ dissociation,

the effective concentration of $H^{+}$ is one-tenth of total concentration.

Therefore concentration $= \frac{1}{10} \times 0.001 N$

$= 0.0001 N$

$\Rightarrow p H = - lo g [H^{+}] = 4$

Q. The pH of 0.001(N) acetic acid solution, which is 10% dissociated. is

3

1

4

2

Concentration of acetic acid =0.001N for 10% dissociation, the effective concentration of H+ is one-tenth of total concentration. Therefore concentration =101​×0.001N =0.0001N ⇒pH=−log[H+]=4

Q. The pH of $0.001 (N)$ acetic acid solution, which is $10%$ dissociated. is

Concentration of acetic acid $= 0.001 N$ for $10%$ dissociation,

the effective concentration of $H^{+}$ is one-tenth of total concentration.

Therefore concentration $= \frac{1}{10} \times 0.001 N$

$= 0.0001 N$

$\Rightarrow p H = - lo g [H^{+}] = 4$