The degree of hydrolysis of a $0.01 \ M$ ammonium acetate solution is = ........ [ $K_h = 3.175 \times 10^{-5}$ ]

If $0.1 \, M \, CH_3COONa$ undergoes $1 \%$ hydrolysis,then the values of $[OH^{-}]$,$[H^{+}]$,and $pH$ are respectively:

The $pK_{a}$ of acetic acid and $pK_{b}$ of ammonium hydroxide are $4.76$ and $4.75$ respectively. Calculate the $pH$ of ammonium acetate solution.

Which among the following salt solutions in water shows a $pH$ greater than $7$?

Explain the following with reasons:
$(i)$ $NaCl$ solution is neutral. The solution of strong acid and strong base salts is neutral.
$(ii)$ $NaCH_3COO$ solution is basic. The solution of strong base and weak acid salt is basic.
$(iii)$ $NH_4Cl$ solution is acidic. The solution of weak base and strong acid salt is acidic.
$(iv)$ The solution of $NH_4CH_3COO$ is (almost) neutral. The solution of weak acid - weak base salts is almost neutral.

Which of the following $0.1 \ M$ aqueous solutions will be basic?