Statement $A$: $pH$ of a buffer increases with increasing temperature. Statement $B$: The value of $K_W$ of water decreases with decreasing temperature.

In which of the following equations will $\alpha_1$ or $\alpha_2$ be higher?
$(i) \, NH_4OH + H_2O \rightarrow \alpha_1$
$(ii) \, NH_4OH + D_2O \rightarrow \alpha_2$

The degree of dissociation of a $0.1 \, M$ $CH_3COOH$ solution is $1.32 \times 10^{-2}$. What will be its dissociation constant $(K_a)$?

Assuming complete dissociation,which of the following aqueous solutions will have the same $pH$ value?

Assign $A, B, C, D$ from the given type of reaction.
$Cu(OH)_2 \downarrow + 4NH_3(soln.) \longrightarrow [Cu(NH_3)_4]^{2+} + 2OH^{-}$

The conductivity of a weak acid $HA$ of concentration $0.001 \, mol \, L^{-1}$ is $2.0 \times 10^{-5} \, S \, cm^{-1} .$ If $\Lambda_{m}^{\circ} (HA)=190 \, S \, cm^{2} \, mol^{-1}$,the ionization constant $(K_{a})$ of $HA$ is equal to $....\, \times 10^{-6} .$ (Round off to the Nearest Integer)