Answer:
The pH of solution is 2.88 .
Explanation:
The reaction is :
[tex]CH_3COOH-->CH_3COO^-+H^+[/tex]
We know, [tex]K_a[/tex] for this reaction is = [tex]1.76\times 10^{-5}.[/tex]
Also, since volume of water is 1 L.
Therefore, molarity of solution is equal to number of moles.
Also, [tex]K_a=\dfrac{[CH_3COO^-][H^+]}{[CH_3COOH]}[/tex]
Let, amount of [tex]CH_3COO^- and\ H^+[/tex] produce is x.
So,
[tex]K_a=\dfrac{[x][x]}{[0.1]}\\1.76\times 10^{-5}=\dfrac{[x][x]}{[0.1]}[/tex]
[tex]x=0.0013\ mol.[/tex]
We know, [tex]pH=-log{x}=-log(0.0013)=2.88[/tex]
Therefore, pH of solution is 2.88 .
Hence, this is the required solution.
