Consider a titration of 43.8mL of 0.124M solution of formic acid [Ka(HCOOH)= 1.8
ID: 809137 • Letter: C
Question
Consider a titration of 43.8mL of 0.124M solution of formic acid [Ka(HCOOH)= 1.8*10^(-4)] with a 0.161M solution of sodium hydroxide. Calculate (show all work for full marks):
a) the pH of the formic acid solution before the titration,
b) the pH of the solution at half-equivalence point,
c) the pH of the solution at the equivalence point,
d) the pH of the solution when 1.00mL of the NaOH have been added after the equivalence point was reached.
e) What would have been the volume (in mL) of 0.161M solution of barium hydroxide added at the equivalence point if it were used instead of the 0.161M NaOH solution?
Explanation / Answer
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