Chemistry Forum

50.0 ml of 0.100 M acetic acid are titrated with 0.200 M NaOH solution. a) Calculate the volume of NaOH solution required to neutralize the acetic acid. b) Calculate the pH of the neutralization solution.

(M here means molarity, ie the unit of concentration mol / l)

1. Calculate the mol in 0,1 M 50 ml Acetic acid. This must be equal to x ml 0,2 M NaOH. Solve for x.
2. pH of salt of weak acids
pH = ½ (pKs + log c + 14)
Solve for pH , look up the pKs for Acetic acid in table or internet