Arrange the following $1 \ L$ aqueous solutions of equal concentration in increasing order of their $pH$:
$CH_3COONa, KI, NH_4Cl, HNO_3$

When $100 \ mL$ of $1 \ M$ $NaOH$ solution is mixed with $10 \ mL$ of $10 \ M$ $H_2SO_4$,the resulting mixture will be

For a concentrated solution of a weak electrolyte ($K_{eq} = $ equilibrium constant) $A_2B_3$ of concentration '$c$',the degree of dissociation '$\alpha$' is

$A$ solution of $0.1 \ M$ weak base $(B)$ is titrated with $0.1 \ M$ of a strong acid $(HA)$. The variation of $pH$ of the solution with the volume of $HA$ added is shown in the figure below. What is the $pK_{b}$ of the base? The neutralization reaction is given by $B + HA \rightarrow BH^{+} + A^{-}$.

Find the resulting $pH$ of the mixture of $200 \ mL$ of $HCl$ $(pH = 2)$ and $300 \ mL$ of $NaOH$ $(pH = 12.0)$.

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