CHEM 112 Lecture Notes - Lecture 1: Silver Sulfide, Magnesium Fluoride, Zinc Hydroxide

• School: Queen's University
• Department: Chemistry
• Course: CHEM 112
• Professor: John Carran

Document Summary

Hco3 - (aq) + h2o(l) co3 2- (aq) + h3o+ (aq) The solubility product, ksp, of a solute in aqueous solution is the equilibrium constant for the solubility equilibrium between an ionic solid and its dissolved component ions. Ex. for copper (i) sulfide cu2s: cu2 s(s) 2 cu+ (aq) + s2- (aq) Ksp = (acu + ) 2 (as 2- ) = 1. 3 x 10-36 (at 25 oc) The activity of cu2 s(s) is 1, as it is a pure solid. With very low concentrations of cu+ and s2- , we can replace the activities with molar concentrations: There is usually a dependence of ksp on the match between the size (ionic radius) of the ions in the salt. The better the match, the less soluble is the salt (packs together better in the solid for) The molar solubility, s, of a salt can be used to determine the value of ksp, and vice-versa.