Chapter 16

The pOH of a solution is \(9.40 .\) Calculate the hydrogen ion concentration of the solution.

Calculate the number of moles of \(\mathrm{KOH}\) in \(5.50 \mathrm{~mL}\) of a \(0.360 \mathrm{M}\) KOH solution. What is the \(\mathrm{pOH}\) of the solution?

A solution is made by dissolving \(18.4 \mathrm{~g}\) of \(\mathrm{HCl}\) in 662 \(\mathrm{mL}\) of water. Calculate the \(\mathrm{pH}\) of the solution. (Assume that the volume of the solution is also \(662 \mathrm{~mL} .)\)

Explain what is meant by the strength of an acid.

Without referring to the text, write the formulas of four strong acids and four weak acids.

What are the strongest acid and strongest base that can exist in water?

\(\mathrm{H}_{2} \mathrm{SO}_{4}\) 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 these 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) HCN, (i) \(\mathrm{HNO}_{2}\)

Classify each of these species as a weak or strong base: (a) LiOH, (b) \(\mathrm{CN}^{-}\) (c) \(\mathrm{H}_{2} \mathrm{O}\) (d) \(\mathrm{ClO}_{4}^{-},(\mathrm{e}) \mathrm{NH}_{2}^{-}\)

Which of these statements is/are true regarding a 1.0 \(M\) solution of a strong acid HA? (a) \(\left[\mathrm{A}^{-}\right]>\left[\mathrm{H}^{+}\right]\) (b) The \(\mathrm{pH}\) is 0.00 . (c) \(\left[\mathrm{H}^{+}\right]=1.0 \mathrm{M}\) (d) \([\mathrm{HA}]=1.0 \mathrm{M}\).