Calculate the pH of a solution prepared by mixing 0.0800 mol of chloroacetic acid plus 0.0400 mol of sodium chloroacetate in 1.04 L of water. (pKa of chloroacetic acid = 2.865.)
(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 first your head, and then the Henderson-Hasselbalch equation, find the pH of a solution prepared by dissolving all the following compounds in one beaker containing a total volume of 1.00 L of 0.180 mol ClCHCO2H, 0.020 mol ClCH2CO2Na, 0.080 mol HNO3 and 0.080 mol Ca(OH) 2. Assume that Ca(OH) 2 dissociates completely