91Ó°ÊÓ

Design an Experiment Describe how you would design and perform a titration in which you use 0.250\(M \mathrm{HNO}_{3}\) to determine the molarity of a cesium hydroxide solution. Include the formula and net ionic equations.

In terms of ion concentrations, distinguish between acidic, neutral, and basic solutions.

Write a balanced chemical equation that represents the self-ionization of water.

Classify each compound as an Arrhenius acid or an Arrhenius base. \begin{equation} \begin{array}{ll}{\text { a. } \mathrm{H}_{2} \mathrm{S}} & {\text { c. } \mathrm{Mg}(\mathrm{OH})_{2}} \\ {\text { b. } \mathrm{RbOH}} & {\text { d. } \mathrm{H}_{3} \mathrm{PO}_{4}}\end{array} \end{equation}

Geology When a geologist adds a few drops of HCl to a rock, gas bubbles form. What might the geologist conclude about the nature of the gas and the rock?

Explain the difference between a monoprotic acid, a diprotic acid, and a triprotic acid. Give an example of each.

Why can \(\mathrm{H}^{+}\) and \(\mathrm{H}_{3} \mathrm{O}^{+}\) be used interchangeably in chemical equations?

Use the symbols \(<,>,\) and \(=\) to express the relationship between the concentrations of \(\mathrm{H}^{+}\) ions and \(\mathrm{OH}^{-}\) ions in acidic, neutral, and basic solutions.

Explain how the definition of a Lewis acid differs from the definition of a Bronsted-Lowry acid.

Write a balanced chemical equation for each of the following. \begin{equation} \begin{array}{l}{\text { a. the dissociation of solid magnesium hydroxide in }} \\ {\text { water }} \\ {\text { b. the reaction of magnesium metal and hydrobromic }} \\ {\text { acid }} \\ {\text { c. the ionization of propanoic acid (CH_ }_{3} \mathrm{CH}_{2} \mathrm{COOH} )} \\ {\text { in water }} \\ {\text { d. the second ionization of sulfuric acid in water }}\end{array} \end{equation}