The basicity of acetic acid is the same as the basicity of____. (a) \(\mathrm{HNO}_{3}\) (b) \(\mathrm{H}_{2} \mathrm{SO}_{4}\) (c) \(\mathrm{H}_{3} \mathrm{PO}_{4}\) (d) \(\mathrm{H}_{2} \mathrm{CO}_{3}\)

Let's write down the molecular formulas of the given acids (in addition to the formula of acetic acid) for easier comparison: - Acetic acid: \(\mathrm{CH}_{3}\mathrm{COOH}\) - (a) \(\mathrm{HNO}_{3}\) - (b) \(\mathrm{H}_{2} \mathrm{SO}_{4}\) - (c) \(\mathrm{H}_{3} \mathrm{PO}_{4}\) - (d) \(\mathrm{H}_{2} \mathrm{CO}_{3}\) Now that we have them all listed, let's analyze each acid to determine its basicity.

Since we're looking for the acid that has the same basicity as acetic acid, we need to determine the basicity of acetic acid first. Acetic acid is a weak acid, with one dissociable hydrogen ion. Its dissociation in water can be represented by the following equation: \(\mathrm{CH}_{3}\mathrm{COOH} \longleftrightarrow \mathrm{H}^{+} + \mathrm{CH}_{3}\mathrm{COO}^{-}\) Since only one hydrogen ion is released, the basicity of acetic acid is 1.

With the basicity of acetic acid determined, we can now compare it to the basicity of the other acids: - (a) \(\mathrm{HNO}_{3}\) is a strong acid with one dissociable hydrogen ion (\(\mathrm{NO}_{3}^{-}\) is the conjugate base). Its basicity is 1. - (b) \(\mathrm{H}_{2} \mathrm{SO}_{4}\) is a strong dibasic acid, meaning it has two dissociable hydrogen ions. Its basicity is 2. - (c) \(\mathrm{H}_{3} \mathrm{PO}_{4}\) is a weak tribasic acid, with three dissociable hydrogen ions. Its basicity is 3. - (d) \(\mathrm{H}_{2} \mathrm{CO}_{3}\) is a weak dibasic acid, with two dissociable hydrogen ions (\(\mathrm{HCO}_{3}^{-}\) and \(\mathrm{CO}_{3}^{2-}\) are the conjugate bases). Its basicity is 2. Considering the basicity values we calculated, the acid with the same basicity as acetic acid is: - (a) \(\mathrm{HNO}_{3}\) The correct answer is (a).