What is the $pH$ of a solution in which $10.0 \ mL$ of $0.010 \ M$ $Sr(OH)_2$ is added to $10.0 \ mL$ of $0.010 \ M$ $HCl$?

At $25^{\circ} C$, the molar conductance of $0.007 \ M$ hydrofluoric acid is $150 \ \text{mho} \ cm^{2} \ mol^{-1}$ and its $\Lambda_{m}^{\circ} = 500 \ \text{mho} \ cm^{2} \ mol^{-1}$. The value of the dissociation constant of the acid at the given concentration at $25^{\circ} C$ is

At $27^{\circ}C$,$100 \ mL$ of $0.4 \ M$ $HCl$ is mixed with $100 \ mL$ of $0.5 \ M$ $NaOH$ solution. To the resultant solution,$800 \ mL$ of distilled water is added. What is the $pH$ of the final solution?

Which of the following plots represents the graph of $pH$ against the volume of alkali added in the titration of $NaOH$ and $HCl$?

At $298 \, K$,a $0.1 \, M$ $CH_3COOH$ solution is $1.34 \%$ ionized. The ionization constant $K_a$ for acetic acid will be:

For the reaction in aqueous solution $Zn^{2+} + X^{-} \rightleftharpoons ZnX^{+}$,the $K_{eq}$ is greatest when $X$ is