[Nathaniel]

Please help me finish off each subquestion

If 25.00 mL of 0.20 mol/L HCO2H(aq) is titrated with 0.20 mol/L NaOH(aq) (the titrant), determine the pH
a) Before Titration begins

My work:
HCOOH -->H+ plus HCOO-
(HCOOH) = 0.2 - x
H+ = x
HCOO = x
Ka = (H+)(HCOO-)/(HCOOH)
Plug in the above variables into Ka and solve for H+

b) after 10.0 mL of NaOH has been added
NaOH has been added
HCOOH + NaOH --> HCOONa + H2O
mols HCOOH initiallt - M x L = ?
mols NaOH added = M x L = ?
mols HCOONa formed = ?
pH = pKa + log[(base)(acid)]


c) at the equivalence point
My work:
We have the salt HCOONa + H2O at the equivalence point
HCOO- plus HOH --> HCOOH plus OH-
Kb = kw/ka
    = (HCOOH)(OH-)/HCOO-
(HCOOH) = x
(OH-) = x
(HCOO-) = 0.2 - x
Plug into Kb and solve for x = (OH-), then convert to pH