Problem: Use the given molar solubilities in pure water to calculate Ksp for each compound. a. MX; molar solubility = 3.27 x 10-11 M b. PbF2; molar solubility = 5.63 x 10-3 M c. MgF2; molar solubility = 2.65 x 10-4 M

FREE Expert Solution

Recall that Ksp is an equilibrium constant related to slightly soluble ionic compounds


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

MnNm(s)  n Mm+(aq) + m Nn–(aq)


The Ksp expression then is:


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


where x = molar solubility of the compound.


Solve Ksp for each:

a. MX; molar solubility = 3.27 x 10-11

MX(s)  M+(aq) +X(aq)


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Problem Details

Use the given molar solubilities in pure water to calculate Ksp for each compound. 

a. MX; molar solubility = 3.27 x 10-11

b. PbF2; molar solubility = 5.63 x 10-3 

c. MgF2; molar solubility = 2.65 x 10-4 M

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