EXERCISE-1

The solubility product $\mathrm{Mg}{\left(\mathrm{OH}\right)}_2$ in water at $25°\mathrm{C}$ is $8.9\times {10}^{-13}{\left(\mathrm{mole} {\mathrm{dm}}^{-3}\right)}^3$ While that of $\mathrm{AI}{\left(\mathrm{OH}\right)}_3$ is $5\times {10}^{-33}{\left(\mathrm{mol} {\mathrm{dm}}^{-3}\right)}^4.$ If ${\mathrm{S}}_1 \mathrm{and} {\mathrm{S}}_2$ are thesolubilities of $\mathrm{Mg}{\left(\mathrm{OH}\right)}_2 \mathrm{and} \mathrm{AI}{\left(\mathrm{OH}\right)}_3$ in water in $\mathrm{mol} {\mathrm{dm}}^{-3}$ at $25°\mathrm{C}$, what is the order of order of magnitude of the ratio, ${\mathrm{S}}_1/{\mathrm{S}}_2?$

When $\mathrm{HCI}$ gas is passed through a saturated solution of common salt, pure $\mathrm{NaCI}$ is precipitated because-

An acid-base indicator which is a weak acid has a ${\mathrm{pK}}_{\mathrm{a}}$ value $=5.5.$ At what concentration ratio of sodium acetate to acetic acid would the indicator show a colour half-way between those of its acid and conjugate base  forms? ${\mathrm{pK}}_{\mathrm{a}}$ of acetic acid $=4.75$

The degree of hydrolysis of $0.1\mathrm{M}$ solution of ${{\mathrm{ArNH}}_3}^{+}{\mathrm{CI}}^{-} \mathrm{is} 0.01$. Find the  ${\mathrm{H}}^{+}$ concentration in $0.4\mathrm{M}$ solution of ${{\mathrm{ArNH}}_3}^{+}{\mathrm{CI}}^{-}$

What is the ${\mathrm{pK}}_{\mathrm{b}}$ of a weak base whose $0.1\mathrm{M}$ solution has $\mathrm{pH}=9.5?$

Which of the following orders regarding the base strength of a leaving group in a reaction of an acid derivative with a nucleophile is correct:

At $25°\mathrm{C}$ dissociation constant of acid $\mathrm{HA}$ and base $\mathrm{BOH}$ in aqueous solution is same. The $\mathrm{pH}$ of $0.1\mathrm{M}$ solution of $\mathrm{HA}$ is $5$. The $\mathrm{pH} \mathrm{of} 0.1\mathrm{M}$ solution of $\mathrm{BOH}$ at the same temperature is 

The degree of hydrolysis of  $0.1\mathrm{M}$ solution of conjugate base of $\mathrm{HA} \mathrm{is} 0.01$. Find the ${\mathrm{H}}^{+}$ concentration in $0.4\mathrm{M}$ solution of ${\mathrm{A}}^{-}$