Which of the following will occur if a $0.1 \,M$ solution of a weak acid is diluted to $0.01\,M$ at constant temperature
$[{H^ + }]$ will decrease to $0.01 \,M$
$pH$ will decrease
Percentage ionization will increase
Both $(b)$ and $(c)$
The solution of $N{a_2}C{O_3}$ has $pH$
At $25\,^oC$, the dissociation constant of $CH_3COOH$ and $NH_4OH$ in aqueous solution are almost the same. The $pH$ of a solution $0.01\, N\, CH_3COOH$ is $4.0$ at $25\,^oC$. The $pH$ of $0.01\, N\, NH_4OH$ solution at the same temperature would be
${K_{C{H_3}COOH}} = 1.9 \times {10^{ - 5}}$. Calculate $pH$ at end point in titration of $0.1$ $M$ $C{H_3}COOH$ and $0.1$ $M$ $NaOH$.
The hydrogen ion concentration of $0.1\,N$ solution of $C{H_3}COOH,$ which is $30\%$ dissociated, is
The $pH$ of $ 0.1 \,M$ solution of a weak monoprotic acid $1\%$ ionized is