Compute the solubility from ksp and vice versa

Reference no: EM13170775

Learning Goal

To learn how to calculate the solubility from Ksp and vice versa. Consider the following equilibrium between a solid salt and its dissolved form (ions) in a saturated solution:

CaF2 (s) --> Ca + 2F

At equilibrium, the ion concentrations remain constant because the rate of dissolution of solid CaF2 equals the rate of the ion crystalllization. The equilibrium constant for the dissolution reaction is

Ksp = [Ca][F]2

Ksp is called the solubility product and can be determined experimentally by measuring the solubility, which is the amount of compound that dissolves perunit volume of saturated solution.

PartA

A saturated Solution of lead (II) fluoride, PbF2 in water. The concentration of Pb ion in the solution was found to be 2.08*10^-3 M

Calculate Ksp for PbF2

Part B

The Value of Ksp for silver carbonate, Ag2CO3, is 8.10*10^-12

Calculate the solubility of Ag2CO3 in grams per liter.

Reference no: EM13170775

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