The ionization constant of benzoic acid is $6.5 \times 10^{-5}$ at $298 \ K$ temperature. Calculate $pH$ of its $0.15 \ M$ solution. (in $.5$)

$pH$ of $0.05 \ M$ aqueous solution of diethyl amine is $10$. The value of equilibrium constant $(K_b)$ is:

For a $10 \ M \ CH_3COOH$ solution,if $K_a = 10^{-5}$,what will be the values of $[H^{+}]$ and $pH$ respectively?

At $25 \, ^\circ C$,the dissociation constant of a base $BOH$ is $1.0 \times 10^{-12}$. The concentration of hydroxyl ions in $0.01 \, M$ aqueous solution of the base would be:

The $pH$ of $0.1 \, M$ acetic acid solution is closest to $.....$ [Dissociation constant of the acid,$K_{a} = 1.8 \times 10^{-5}$]

The $pH$ of a $0.1 \ M$ solution of $NH_{4}OH$ (having $K_{b} = 1.0 \times 10^{-5}$) is equal to