Calculate the pH of a solution prepared by mixing 0.080 0 mol of chloroacetic acid plus 0.040 0 mol of sodium chloroacetate in 1.00 L of water. (Assume pKa = 2.866 and Kw = 1.01 ✕ 10−14). (a) First do the calculation by assuming that the concentrations of [HA] and [A-] equal their formal concentrations.
(b) Then do the calculation, using the real values of [HA] and [A-] in the solution.
(c) Using f rst your head, and then the Henderson-Hasselbalch equation, f nd the pH of a solution prepared by dissolving all the all the following compounds in one beaker containing a total volume of 1.00 L: 0.174 mol ClCH2CO2H, 0.026 mol ClCH2CO2Na, 0.074 mol HNO3, and 0.074 mol Ca(OH)2. Assume that Ca(OH)2 dissociates completely.