Problem 1
This chapter opens with a discussion of ocean acidification. a. Seawater contains many salts, including sodium chloride. Write its chemical formula. b. Sodium chloride is soluble in water. What chemical process takes place when solid sodium chloride dissolves?
Problem 2
Calcium carbonate is another salt. Write its chemical formula. Would you expect calcium carbonate to be soluble or insoluble in water?
Problem 3
Carbon dioxide is a gas found in our atmosphere. a. What is the approximate concentration? b. Why is its concentration in the atmosphere increasing? c. Draw the Lewis structure for the \(\mathrm{CO}_{2}\) molecule. d. Would you expect carbon dioxide to be highly soluble in seawater? Explain.
Problem 5
a. Draw the Lewis structure for the water molecule. b. Draw Lewis structures for the hydrogen ion and the hydroxide ion. c. Write a chemical reaction that relates all three structures from parts a and b.
Problem 6
a. Give names and chemical formulas for five acids of your choice. b. Name three observable properties generally associated with acids.
Problem 9
Write a chemical equation that shows the release of hydroxide ions as each of these bases dissolves in water. a. \(\mathrm{KOH}(s)\), potassium hydroxide b. \(\mathrm{Ba}(\mathrm{OH})_{2}(s)\), barium hydroxide
Problem 10
Which gas dissolved in water to produce each of these acids? a. carbonic acid, \(\mathrm{H}_{2} \mathrm{CO}_{3}\) b. sulfurous acid, \(\mathrm{H}_{2} \mathrm{SO}_{3}\)
Problem 11
Consider these ions: nitrate, sulfate, carbonate, and ammonium. a. Give the chemical formula for each. b. Write a chemical equation in which the ion (in aqueous form) appears as a product.
Problem 12
Write a balanced chemical equation for each acid-base reaction. a. Potassium hydroxide is neutralized by nitric acid. b. Hydrochloric acid is neutralized by barium hydroxide. c. Sulfuric acid is neutralized by ammonium hydroxide.
Problem 13
In each pair, the \(\left[\mathrm{H}^{+}\right]\)is different. By what factor of 10 ? a. \(\mathrm{pH}=6\) and \(\mathrm{pH}=8\) b. \(\mathrm{pH}=5.5\) and \(\mathrm{pH}=6.5\) c. \(\left[\mathrm{H}^{+}\right]=1 \times 10^{-8} \mathrm{M}\) and \(\left[\mathrm{H}^{+}\right]=1 \times 10^{-6} \mathrm{M}\) d. \(\left[\mathrm{OH}^{-}\right]=1 \times 10^{-2} \mathrm{M}\) and \([\mathrm{OH}]=1 \times 10^{-3} \mathrm{M}\)
