The ionization constant of benzoic acid is $6.5 \times {10^{ - 5}}$ at $298$ $K$ temperature. Calculate $pH$ of its $0.15$ $M$ solution.
The ionization constant of benzoic acid is $6.5 \times {10^{ - 5}}$ at $298$ $K$ temperature. Calculate $pH$ of its $0.15$ $M$ solution.
$\left[\mathrm{H}^{+}\right]=3.12 \times 10^{-3} \mathrm{M}, \mathrm{pH}=2.5$
Similar Questions
Derive ${K_w} = {K_a} \times {K_b}$ and ${K_w} = p{K_a} \times p{K_b}$ for weak base $B$ and its conjugate acid ${B{H^ + }}$.
Derive ${K_w} = {K_a} \times {K_b}$ and ${K_w} = p{K_a} \times p{K_b}$ for weak base $B$ and its conjugate acid ${B{H^ + }}$.
For a weak acid $HA$ with dissociation constant ${10^{ - 9}},\,\,pOH$ of its $0.1 \,M$ solution is
For a weak acid $HA$ with dissociation constant ${10^{ - 9}},\,\,pOH$ of its $0.1 \,M$ solution is
- [AIPMT 1989]
${K_a} = 1.4 \times {10^{ - 5}}$ of propanoic acid. Calculate its $pH$ of $0.1$ $M$ solution.
${K_a} = 1.4 \times {10^{ - 5}}$ of propanoic acid. Calculate its $pH$ of $0.1$ $M$ solution.
The $pH$ of $ 0.1 \,M$ solution of a weak monoprotic acid $1\%$ ionized is
The $pH$ of $ 0.1 \,M$ solution of a weak monoprotic acid $1\%$ ionized is
A weak acid is $ 0.1\% $ ionised in $0.1\, M $ solution. Its $pH$ is
A weak acid is $ 0.1\% $ ionised in $0.1\, M $ solution. Its $pH$ is