ASAP answer please with all steps

Question

ASAP answer please with all steps

1. 8.0 mL of 0.10 M HCl is titrated with 0.10 M NaOH. Perform the following calculations
2. pH of the acid before any NaOH is added
3. Volume of 0.10 M NaOH needed to reach the equivalence point
4. pH at the equivalence point
5. 8.0 mL of 0.10 M HC2H3O2 is titrated with 0.10 M NaOH. Perform the following calculations
6. pH of the acid before any NaOH is added 
7. Volume of 0.10 M NaOH needed to reach the equivalence point
8. pH at the equivalence point
9. Volume of 0.10 M NaOH needed to reach the half-way point
10. pH at the half-way point
11. 8.0 mL of 0.10 M NH3 is titrated with 0.10 M HCl. Perform the following calculations
12. pH of the base before any HCl is added
13. Volume of 0.10 M HCl needed to reach the equivalence point
14. pH at the equivalence point
15. Volume of 0.10 M HCl needed to reach the half-way point
16. pH at the half-way point

Answer 1

This is alot. I can help you with this.

To start:

1. 8.0 mL of 0.10 M HCl is titrated with 0.10 M NaOH. Perform the following calculations
2. pH of the acid before any NaOH is added

Just a strong acid problem. Use pH=-log[H+]

1. Volume of 0.10 M NaOH needed to reach the equivalence point

The ratio of acid to base is 1:1 by the equation:

HCl+NaOH-->NaCl+NaCl

So use M_acidV_acid=M_baseV_base

where

M=molarity, and

V=mL

1. pH at the equivalence point

pH at the equivalence point will be 7 since NaCl is a neutral salt, since HCl and NaOH are both strong