Chemistry Help?

Question

calculate the pH of a solution  at the equivalence point when 100 mL of a 0.100 M solution of acetic acid, which has a Ka value+ 1.8*10^(-5), is titrated with 0.10 M NaOH solution.

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.