1. Complete and balance the following acid/base reactions.
a. aqueous sulfuric acid plus solid calcium hydroxide
b. aqueous hydrobromic acid plus water
c. HClO3(aq) + CO32–(aq)
d. HN3(aq) + H2O(l)
2. Write the chemical reaction needed to determine the pH and give the pH for the following solutions.
a. 0.0010 M perchloric acid.
b. 0.0010 M magnesium hydroxide
3. Indicate the stronger acid in each pair. Explain your reasoning in 5 words or less. For the stronger acid, write out the balanced reaction of the acid with water. label the conjugate acid/base pairs for each reaction
a. CCl3COOH vs. CH3COOH
b. H2SO4 vs. HNO3
c. HCrO4– vs. HMnO4
4. Pyrophosphoric acid is polyprotic, H4P2O7, with Ka1 = 3.0×10–2, Ka2 = 4.4×10–3, Ka3 = 2.5×10–7, and Ka4 = 5.6×10–10. Although it is a weak acid, a 0.010 M solution is greater than 100 % ionized and has a pH of about 1.9. Explain how this can happen, using chemical reactions to supplement your argument.
5. A 0.010 M solution of hydrogen selenate ion (HSeO4–, Ka = 2.2×10–2) was prepared. Find the pH.