a)(3 pts) We have 500.0 mL of an aqueous solution of CaCl2 (CaCl2 is a strong electrolyte, molar mass =110.98 g/mol). We add an excess of AgNO3 to produce an AgCl(s) precipitate (AgCl has a molar mass of 143.32 g/mol). The mass of AgCl produced is 2.222 g. What was the original concentration of CaCl2? b)(5 pts) HA is a weak acid with a ionization constant, Ka, of 5.0 \times 10?5. We have 1.00 L of a buffer solution which is 0.377 M in HA and 0.455 M in NaA. To this buffer solution, we add 0.1000 mol of NaOH (assume the volume does not change). What was the pH of the solution before the addition of the NaOH? What is the pH of the solution after the addition of the NaOH? The temperature is 25.0?C.