A 1.25 m solution of the weak acid ha is 9.2% dissociated. what is the ph of the solution?

Asked by maham237 @ 25/12/2020 in Chemistry viewed by 447 People

Answered by maham237 @ 25/12/2020

Answer:

0.94 is the pH of the solution.

Explanation:

The equilibrium reaction for dissociation of $HA$ (weak acid) is,

$HA+H_2O\rightleftharpoons A^-+H_3O^+$

initially conc. c 0 0

At eqm. $c(1-\alpha)$ $c\alpha$ $c\alpha$

Concentration (c) = 1.25 M

Degree of dissociation = $\alpha$ = 9.2% = 0.092

$[H_3O^+]=c\alpha$

$= 1.25 M\times 0.092=0.115 M$

The pH of the solution is :

$pH=-\log[H_3O^+]$

$=-\log[0.115 M}=0.94$

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