Question

8.0 mL of 0.10 M NH3 is titrated with 0.10 M HCl. Perform the following calculations (15 points):

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

Answer 1

pH of the NH₃ before any HCl is added is

$PH = -log (0.10)=1$

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

$P_H = 4.3$