$A$ $20 \ mL$ sample of a $0.1 \ M$ solution of the weak monoprotic acid $HA$ is titrated with $0.25 \ M \ NaOH$. The volume of $NaOH$ solution required to reach the equivalence point is: ............. $mL$

In a solution,$0.02 \ M$ acetic acid is $4 \%$ dissociated. The $[OH^{-}]$ in the solution is

Assign $A, B, C, D$ from the given type of reaction.
$Zn(OH)_2 \downarrow + 2NaOH \longrightarrow Na_2ZnO_2 + 2H_2O$

The hydrolysis constants of salts $NaA$ and $NaB$ (of weak acids $HA$ and $HB$) are $10^{-8}$ and $10^{-10}$ respectively. If the dissociation constant of weak acid $HC$ is $10^{-5}$,what is the decreasing order of acidic strength?

Which will not affect the degree of ionisation?

At $25 \, ^oC$,the concentration of $H^{+}$ and $OH^{-}$ ions in pure water is $1 \times 10^{-7} \, M$ each. Which of the following is equal to $2 \times 10^{-7} \, M$?