91Ó°ÊÓ

Of the following conditions, which indicate a basic solution? a. \(\mathrm{pOH}=12.53\) b. \(\mathrm{pH}=3.64\) c. \(\mathrm{pOH}<\left[\mathrm{H}^{+}\right]\) d. \(\left[\mathrm{OH}^{-}\right]>1.0 \times 10^{-7} M\)

Buffered solutions are mixtures of a weak acid and its conjugate base. Explain why a mixture of a strong acid and its conjugate base (such as \(\mathrm{HCl}\) and \(\mathrm{Cl}^{-}\) ) is not buffered.

Of the following acids, which have relatively strong conjugate bases? a. \(\mathrm{HNO}_{2}\) b. HCOOH c. \(\mathrm{HClO}_{4}\) d. \(\mathrm{HNO}_{3}\)

Is it possible for a solution to have \(\left[\mathrm{H}^{+}\right]=0.002 \mathrm{M}\) and \(\left[\mathrm{OH}^{-}\right]=5.2 \times 10^{-6} M\) at 25 C \(?\) Explain.

Despite \(\mathrm{HCl}\) 's being a strong acid, the \(\mathrm{pH}\) of \(1.00 \times 10^{-7} \mathrm{M} \mathrm{HCl}\) is not exactly 7.00 . Can you suggest a reason why?

According to Arrhenius, bases are species that produce ions in aqueous solution.

A conjugate acid-base pair consists of two substances related by the donating and accepting of a(n)

Acetate ion, \(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}^{-},\) has a stronger affinity for protons than does water. Therefore, when dissolved in water, acetate ion behaves as a(n)

An acid such as \(\mathrm{HCl}\) that strongly conducts an electric current when dissolved in water is said to be a(n) acid.

Draw the structure of the carboxyl group, \(-\mathrm{COOH}\). Show how a molecule containing the carboxyl group behaves as an acid when dissolved in water.