The plot of $pH$-metric titration of weak base $NH_4OH$ vs strong acid $HCl$ looks like:

The dissociation constant of acetic acid is $1.6 \times 10^{-5}$ and $\Lambda _{CH_3COOH}^o = 370.6 \times 10^{-4} \, S \, m^2 \, mol^{-1}$. The specific conductance of $0.01 \, M$ acetic acid solution will be approximately:

In a saturated solution of $Mg(OH)_2$,the degree of dissociation of $Mg(OH)_2$ is $\alpha$. Find the concentration $(C)$ of $Mg(OH)_2$ if the concentration of $[OH^{-}]$ is $2$.

$50 \ mL$ of $10^{-3} \ M \ HCl$ is mixed with $50 \ mL$ of $0.05 \ M \ CH_3COOH$ $(pK_a = 4.7)$. The degree of dissociation of water in the resulting solution is

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

The number of hydroxyl ions in $10 \text{ cm}^3$ of $0.2 \text{ M}$ $HCl$ solution is