1. If the Kb of a weak base is 7.6x10^-6, what is the pH of a 0.25M solution of this base?
2. The Ka of a monoprotic weak acid is 3.8x10^-3. What percent ionization of a 0.161 M solution of this acid?
3. Enough of a monoprotic acid is dissolved in water to produce a 0.0156 M solution. The pH of the resulting solution is 6.22. Calculate the Ka for the acid.
4. Enough of a monoprotic acid is dissolved in water to produce a 0.0134 M solution. The pH of the resulting solution is 2.63. Calculate the Ka for the acid.
5. A certain weak base has a Kb of 8.60 × 10-7. What concentration of this base will produce a pH of 10.34?
6. Using chemical equations, show how the triprotic acid H3PO4 ionizes in water. Phases, such as (l) or (aq), are optional.
7. For the diprotic weak acid H2A, Ka1 = 3.0 × 10-5 and Ka2 = 5.4 × 10-7. What is the pH of a 0.0450 M solution of H2A? What are the equilibrium concentrations of H2A and A2– in this solution?