Chemistry

Brittany Monroe

10 August, 03:12

Consider the dissolution of AB (s) : AB (s) ⇌A + (aq) + B - (aq) Le Châtelier's principle tells us that an increase in either [A+] or [B-] will shift this equilibrium to the left, reducing the solubility of AB. In other words, AB is more soluble in pure water than in a solution that already contains A + or B - ions. This is an example of the common-ion effect. The generic metal hydroxide M (OH) 2 has Ksp = 1.05*10-18. (NOTE: In this particular problem, because of the magnitude of the Ksp and the stoichiometry of the compound, the contribution of OH - from water can be ignored. However, this may not always be the case.) What is the solubility of M (OH) 2 in pure water?