The compound whose $0.1\mathrm{M}$ solution is basic?

The correct option is B

${\mathrm{CH}}_3\mathrm{COONa}$

The explanation for the correct option:

Option (B):${\mathrm{CH}}_3\mathrm{COONa}$

• ${\mathrm{CH}}_3\mathrm{COONa}$ is known as the mixture of the solution between a strong base i.e $\mathrm{NaOH}$ and a weak acid i.e ${\mathrm{CH}}_3\mathrm{COOH}$ , which can be given as:

$\underset{(\mathrm{Acetic}\mathrm{acid})}{{\mathrm{CH}}_3\mathrm{COOH}}+\underset{(\mathrm{Sodium}\mathrm{hydroxide})}{\mathrm{NaOH}}\to \underset{\left(\mathrm{Sodium}\mathrm{acetate}\right)}{{\mathrm{CH}}_3\mathrm{COONa}}+\underset{\left(\mathrm{Water}\right)}{{\mathrm{H}}_2\mathrm{O}}$

• We know that the mixture of a strong base with the weak acid gives out a basic solution.
• Hence, $0.1\mathrm{M}$ solution of Sodium acetate is a basic solution.

The explanation for the incorrect option:

Option (A):${\mathrm{NH}}_4\mathrm{Cl}$

• ${\mathrm{NH}}_4\mathrm{Cl}$ is known as the solution mixture between a weak base i.e ${\mathrm{NH}}_4\mathrm{OH}$ and the strong acid i.e $\mathrm{HCl}$, which makes it acidic in nature.
• Hence, the given option does not represent to the correct option.

Option (C):${\mathrm{Na}}_2{\mathrm{SO}}_4$

• ${\mathrm{Na}}_2{\mathrm{SO}}_4$ is known as the solution mixture between a strong base i.e $\mathrm{NaOH}$ and the strong acid i.e ${\mathrm{H}}_2{\mathrm{SO}}_4$,which makes it neutral in nature.
• Thus, the given option is not correct one.

Option (D):${\mathrm{CH}}_3{\mathrm{COONH}}_4$

• ${\mathrm{CH}}_3{\mathrm{COONH}}_4$is known as the solution mixture between a weak base i.e ${\mathrm{NH}}_4\mathrm{OH}$ and a weak acid ${\mathrm{CH}}_3\mathrm{COOH}$, for which the solution cant be basic in nature .
• Hence, the given option does not coincide with the correct option.

Hence,the compound whose $0.1\mathrm{M}$ solution is basic :${\mathrm{CH}}_3\mathrm{COONa}$, option (B) is correct.