Consider the following statements ( a ) The pH of a mixture...

Strong acid + Strong base mixture
$n\left[{H}_{2}S{O}_{4}\right] > n [ NaOH ]$ So ${H}^{+}$ will be more
\left[{H}^{+}\right] = \dfrac{2 \times 0.1 \times 400 - 0.1 \times 400}{800} = 0.05$<br/>$pH = - log {H}^{+} = - \log 0.05 = 1.3$<br/>(b) The ionic product of water is temperature dependent <br/>(c)$HCOOH ⇌ {H}^{+} + HCO{O}^{-}$(weak acid) <br/>${\text{k}}_{a} = \dfrac{C{\alpha}^{2}}{\left(1 - \alpha\right)}$<br/>${\text{k}}_{a} = \dfrac{C\alpha . \alpha}{\left(1 - \alpha\right)}$<br/>${\text{k}}_{a} = \dfrac{\left({H}^{+}\right)\alpha}{1 - \alpha}$<br/>${10}^{- 5} = {10}^{- 5} \times \dfrac{\alpha}{1 - \alpha}$<br/>$1 - \alpha = \alpha$<br/>$\alpha = \dfrac{1}{2} = 0.5
(d) Le-Chatelier’s Principle in applicable on Common Ion Effect