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

An aqueous solution of aluminium sulphate would show

On dilution,the $pH$ of $CH_3COONa$ solution:

The degree of hydrolysis in hydrolytic equilibrium $A^{-} + H_2O \rightleftharpoons HA + OH^{-}$ at salt concentration of $0.001 \ M$ is $(K_a = 1 \times 10^{-5})$

The $K_{a}$ for $CH_{3}COOH$ is $1.8 \times 10^{-5}$ and $K_{b}$ for $NH_{4}OH$ is $1.8 \times 10^{-5}$. The $pH$ of ammonium acetate solution will be

The degree of hydrolysis of a salt of weak acid and weak base in its $0.1 \, M$ solution is found to be $50 \%$. If the molarity of the solution is $0.2 \, M$,the percentage hydrolysis of the salt should be $...... \%$.