Ionic Equilibria and Acid-Base Theories

Identify the conjugate acid-base pairs of the reactions: a) HCl(g) + H2O → Cl–(aq) + H3O+(aq) b) NH3(aq) + H2O(l) ↔ NH4+(aq) + OH–(aq) c) H2S + NH3(aq) ↔ HS–(aq) + NH4+(aq)

Calculate the pH of 0.01M HCl solution at 25°C.

Calculate the pH, pOH, [H+] and [OH–] of 0.3 M HNO3 solution at 25°C.

Calculate the pH of (a) 0.02 M KOH solution and (b) 0.045 M Ba(OH)2 solution.

A solution of NaOH has a pH of 9.52. What is its pOH, [H+] and [OH–] at 25°C?

Calculate the pH, pOH, [H+] and [OH‒] of 0. 40 M CH3COOH solution at 250C. (Ka =1.8 10 ‒5)

Calculate the pH, pOH, [H+] and [OH‒] of 0.050 M HF solution at 250C. (use Ka = 6.8 ×10 ‒4)

Calculate the pH, pOH, [H+] and [OH‒] of 0.036 M nitrous acid (HNO2) solution at 250C. (use Ka = 7.1× 10 ‒4)

Calculate the pH, pOH, [H+] and [OH‒] of 0.15 M HCN solution at 250C. (use Ka =6.2 ×10 ‒10)

Calculate the percent ionization of a 0.036 M HNO2 solution.