Question

0.025 M CH3COOH is dissociated 9.5%.Hence the pH of the solution is-​

Answer 1

Answer:

the answer to ur question is 2.267

Answer 2

The pH of the acetic acid is 2.624 (option a).

Explanation:

• The concentration (molarity) of acetic acid is$, c = 0.025 M$
• The acid is undergoing a dissociation$,\alpha = 9.5\% = \frac{9.5}{100} = 0.095$
• Hence, the total hydrogen ion concentration will be $= c\times \alpha = 0.025\times 0.095= 0.002375 = 2.375\times 10^{-3}$
• Now, pH is defined as the negative logarithm of hydrogen ion concentration.
• Hence

$pH = -log (2.375\times 10^{-3})$

$pH = -log (2.375) - log10^{-3}$

$pH = -0.3756 + 3$

$pH = 2.624$

Hence, the pH of the given acetic acid solution is 2.624 ( option a)