17. Acid and Base Equilibrium
Acids Introduction
17. Acid and Base Equilibrium Acids Introduction
141PRACTICE PROBLEM
Calculate the pH and the molarities of all species (H3AsO4, H2AsO3–, HAsO42–, AsO43–, H3O+, and OH–) in a 9.50 % (by mass) solution of arsenic acid with a density of 1.1033 g/mL. The equilibrium constants are:
Ka1 = 6.46×10–3
Ka2 = 1.14×10–7
Ka3 = 3.16×10–12
Calculate the pH and the molarities of all species (H3AsO4, H2AsO3–, HAsO42–, AsO43–, H3O+, and OH–) in a 9.50 % (by mass) solution of arsenic acid with a density of 1.1033 g/mL. The equilibrium constants are:
Ka1 = 6.46×10–3
Ka2 = 1.14×10–7
Ka3 = 3.16×10–12