An aqueous solution of ammonium carbonate is

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(B) Ammonium carbonate $(NH_4)_2CO_3$ is a salt of a weak base $(NH_4OH)$ and a weak acid $(H_2CO_3)$.In aqueous solution,it undergoes hydrolysis:$NH_

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Weakly basic

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(B) Ammonium carbonate $(NH_4)_2CO_3$ is a salt of a weak base $(NH_4OH)$ and a weak acid $(H_2CO_3)$.In aqueous solution,it undergoes hydrolysis:$NH_4^+ + H_2O ightleftharpoons NH_4OH + H^+$$CO_3^{2-} + H_2O ightleftharpoons HCO_3^- + OH^-$The dissociation constant of $NH_4OH$ $(K_b = 1.8 	imes 10^{-5})$ is slightly greater than the dissociation constant of $HCO_3^-$ $(K_a = 5.6 	imes 10^{-11})$,but the overall hydrolysis of the carbonate ion is more significant in determining the pH.Since the hydrolysis of the carbonate ion produces $OH^-$ ions,the resulting solution is weakly basic.

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