A 0.150 M solution of nitrous acid (HNO2) is made. Ka = 4.5 x 10-4

Question

1. Show the equilibrium which occurs when this acid is dissolved in water.
2. What is the pH of the solution? Show all work clearly.
3. 100.0 mL of the solution is titrated against 0.150 M NaOH. What is the pH at the equivalence point?
4. What is true about the pH and pKa, and the [acid] and [conjugate base] at the half-equivalence point?

Answer 1

See your post below.