91Ó°ÊÓ

\(\mathrm{H}_{2} \mathrm{SO}_{4}\) is a strong acid, but \(\mathrm{HSO}_{4}^{-}\) is a weak acid. Account for the difference in strength of these two related species.

Classify each of the following species as a weak or strong acid: (a) \(\mathrm{HNO}_{3},\) (b) HF, (c) \(\mathrm{H}_{2} \mathrm{SO}_{4},\) (d) \(\mathrm{HSO}_{4}^{-}\), (e) \(\mathrm{H}_{2} \mathrm{CO}_{3},\) (f) \(\mathrm{HCO}_{3}^{-},(\mathrm{g}) \mathrm{HCl}\) (h) \(\mathrm{HCN}\), (i) \(\mathrm{HNO}_{2}\).

What does the ionization constant tell us about the strength of an acid?

List the factors on which the \(K_{\mathrm{a}}\) of a weak acid depends.

Why do we normally not quote \(K_{\mathrm{a}}\) values for strong acids such as \(\mathrm{HCl}\) and \(\mathrm{HNO}_{3}\) ? Why is it necessary to specify temperature when giving \(K_{\mathrm{a}}\) values?

The \(K_{\mathrm{a}}\) for benzoic acid is \(6.5 \times 10^{-5} .\) Calculate the \(\mathrm{pH}\) of a \(0.10 \mathrm{M}\) benzoic acid solution.

A \(0.040 M\) solution of a monoprotic acid is 14 percent ionized. Calculate the ionization constant of the acid.

Which of the following has a higher pH: (a) \(0.20 \mathrm{M}\) \(\mathrm{NH}_{3},\) (b) \(0.20 \mathrm{M} \mathrm{NaOH} ?\)

From the relationship \(K_{\mathrm{a}} K_{\mathrm{b}}=K_{\mathrm{w}},\) what can you deduce about the relative strengths of a weak acid and its conjugate base?

Carbonic acid is a diprotic acid. Explain what that means.