Problem: Use the Ksp values to calculate the molar solubility of each of the following compounds in pure water. a) MX (Ksp = 6.99 × 10−11) b) PbCl2 (Ksp = 1.17 × 10−5) c) Ca(OH)2 (Ksp = 4.68 × 10−6)

FREE Expert Solution

The dissociation of slightly soluble ionic compounds in solution is as follows:


MnNm(s)  n Mm+(aq) + m Nn–(aq)


ICE Chart: 



Ksp=productsreactants=[nx]n[mx]m


where x = molar solubility of the compound.


a) MX M+ + X-


Ksp=[x][x]6.99 × 1011 =x2

View Complete Written Solution
Problem Details

Use the Ksp values to calculate the molar solubility of each of the following compounds in pure water. 

a) MX (Ksp = 6.99 × 10−11

b) PbCl2 (Ksp = 1.17 × 10−5

c) Ca(OH)2 (Ksp = 4.68 × 10−6)

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Ksp concept. You can view video lessons to learn Ksp. Or if you need more Ksp practice, you can also practice Ksp practice problems.