Chemistry help?

Question

Calculate the pH of a solu$on at the equivalence point when 100.0 mL of a 0.100 M solu$on of acetic acid (HC2H3O2), which has a Ka value of 1.8 × 10–5, is titrated with a 0.10 M NaOH solu$on. 

 

Answer 1

Step 1:

The concentration of acetic acid is [HCH₂H₃O₂] is 0.100 M.

k_a for acetic acid is .

The concentration of sodium hydroxide is [NaOH] is 0.100 M.

The equation

Equilibrium Constant : .

Relation between k_a and k_b : .

Step 1:

generates one mole of  and one mole of .

Let then .

Step 2:

Find the pH of the solution.

Definition of pOH: .

Now .

The pH of the solution is 8.872.

Solution:

The pH of the solution is 8.872.