Ksp – practice problems
Key Point -- Solubility is relative
Types of Problems.
1- From Ksp, you can calculate the molar solubility of a substance
2- From Ksp, you can calculate the concentration of one of the dissolved ions.
3- From molar solubility, can calculate the Ksp.
4- Given the concentration of one of the dissolved ions – can calculate the Ksp
5- Given the concentrations of two solutions and the Ksp, you can predict whether
or not a ppt will form when the two solutions are mixed.
1) What is the molar solubility of lead (II) chloride if the Ksp for lead (II) chloride is 1.6 x 10-5?
What is the solubility in g/L?
2) What is the concentration of silver ion in a saturated solution of silver chloride?
The Ksp for silver chloride is 1.6 x 10-10.
3) The molar solubility of X2Y3 is 0.00056 M. Calculate the Ksp for X2Y3.
4) A saturated solution of magnesium fluoride contains 1.2 x 10-3 M of fluoride ion at equilibrium. What is the molar
solubility of the magnesium fluoride? What is the Ksp of magnesium fluoride?
5) 30.0 mL of 0.0010 M MgCl2 is mixed with 30.0 mL of 0.0010 M NaF. Will a ppt form?
6) A) QZ2 has a Ksp of 3.4 x 10-6. CD2 has a Ksp of 6.3 x 10-5. Which of these two substances has the greatest molar
solubility?
B) XY has a Ksp of 1.5 x 10-9. AB3 has a Ksp of 6.8 x 10-15. Which of these two substances has the greatest molar
solubility?
7) Will a ppt form if 50.0 mL of 0.50 M lead (II) nitrate and 30.0 mL of 0.015 M aluminum chloride are
mixed together? The Ksp of PbCl2 = 1.6 x 10-5.