When $10 \, mL$ of $0.1 \, M$ acetic acid $(pK_a = 5.0)$ is titrated against $10 \, mL$ of $0.1 \, M$ ammonia solution $(pK_b = 5.0)$,the equivalence point occurs at $pH$:

One mole of ammonia was completely absorbed in one litre solution each of $(a)$ $1 \ M \ HCl$,$(b)$ $1 \ M \ CH_{3}COOH$,and $(c)$ $1 \ M \ H_{2}SO_{4}$ at $298 \ K$. The decreasing order for the $pH$ of the resulting solutions is (Given $pK_{b}(NH_{3}) = 4.74$)

Assign $A, B, C, D$ for the given type of reaction:
$Mg(OH)_2 \downarrow + 2HCl \longrightarrow MgCl_2 + 2H_2O$

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

$0.1 \, M$ acetic acid is $1\%$ ionized. If its ionization increases to $10\%$,what will be its new concentration (in $, M$)?

The first and second dissociation constants of a diprotic acid ${H_2}A$ are $1.0 \times 10^{-5}$ and $5.0 \times 10^{-10}$ respectively. The overall dissociation constant of the acid ${H_2}A$ is .......