solubility product constants?

Question

Zn(OH)^2?
AgI?
Cu(OH)^2?
Ni(OH)^2?

a sample of BaSO^4 (s) is added to pure water and allowed to come to equilibrium at 25 degrees celsius. The concentration of Ba^2+ is 1.05 * 10^-5 M at equilibrium. What is the value of ksp for BaSO^4?

At 25 degrees celsius, the concentration of Ag+ ions in a saturated solution of AgBr is 7.07 * 10^-7 M. What is the value of ksp for AgBr?

A sample of MgCO^3(s) is added to pure water and allowed to come to equilibrium at 25 degrees celsius. The concentration of Mg^2+ is 6.3 * 10^-3 M at equilibrium. What is the value of ksp for mgCO^3?

Answer 1

Here is a list of some constants:

http://www.ktf-split.hr/periodni/en/abc/kpt.html

As mentioned, for these binary salt systems you can simply square the concentration at saturation in order to determine the Ksp.

Answer 2

The solubility product constant is the product of the concentrations of EACH cation and anion raised to the power of their charge. i.e. for MgCO^3, Ksp= (conc. Mg 2+)^2 * (conc. CO3 2-)^2. Best of luck!

Answer 3

For each of these numerical problems, simply square the molar solubility to get Ksp.