Calculate the pH of a solution prepared by mixing 0.0800 mol of chloroacetic acid plus 0.0400 mol
Question:
(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: 0.180 mol ClCH2CO2H, 0.020 mol ClCH2CO2Na, 0.080 mol HNO3, and 0.080 mol Ca(OH)2. Assume that Ca(OH)2 dissociates completely.
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a b c pH 2865 log 00400080 256 Using Eqns 820 and 821 and neglecting OH we can ...View the full answer
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