Question

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8.0 mL of 0.10 M HC2H3O2 is titrated with 0.10 M NaOH. Perform the following calculations

1. pH of the acid before any NaOH is added 
2. Volume of 0.10 M NaOH needed to reach the equivalence point
3. pH at the equivalence point
4. Volume of 0.10 M NaOH needed to reach the half-way point
5. pH at the half-way point

Answer 1

Ans:

pH of the acid before any NaOH is added is

$pH = -log[H^+]\\pH = -log (0.10)=1$

Volume of $0.10$ M $NaOH$ needed to reach the equivalence point= $0.04398 L$

So the $pH$ at equivalence point will be

pH = 7.00