1. Complete and balance the following reactions:
a. HCO3–(aq) + KOH(aq)
b. HPO42–(aq) + H2O(l)
c. Co(NO3)2(aq) + H2O(l)
d. Cr(NO3)2(aq) + KOH(aq)
e. BaCl2(aq) + H2SO4(aq)
f. CuNO3(aq) + NaCN(aq)
2. On the titration curve shown, give estimates for the following: the pH at the equivalence point, the equivalence volume, and the pKa.
3. Consider a 0.65 M solution of dimethylamine, (CH3)2NH, at 25 °C.
a. What is the pH of the solution?
b. What is the pH of the solution if enough dimethylammonium hydrobromide, (CH3)2NH2Br , is added so that the dimethylammonium ion concentration becomes 0.65 M?
4. Consider copper(II) hydroxide at 25 °C.
a. What is the molar solubility in pure water?
b. What is the molar solubility in 1.0 M Cu(NO3)2 solution?
c. What is the molar solubility in 1.0 M NH3 solution?
5. You are given 1.0 M solutions of sodium dihydrogen phosphate and sodium hydrogen phosphate. How many mL of each solution are required to prepare 100.0 mL of a buffer with pH = 7.40 at 25 °C.