Write the solubility product constant expressions for:
calcium fluoride
copper(II) arsenate
silver phosphate
The solubility of lithium phosphate (115.79 g/mol) at 18°C is
0.034 g/100 mL. What is Ksp for this salt at this temperature?
Copper(II) arsenate (468.48 g/mol) has a Ksp of 7.6 x 10-36 at
25°C. What is the molar solubility of this salt at this
temperature?
Lead(II) iodide (461 g/mol) has a Ksp of 7.1 x 10-9 at 25°C.
What is the molar solubility of this salt at this temperature?
What is the molar solubility of lead(II) iodide in a 0.100 M
solution of potassium iodide at 25°C?
Which of the following has the highest molar solubility? (look
up Ksp values)
MgF2
MgCO3
Mg3(PO4)2
Li3PO4
Ag2CrO4 will have the highest solubility in which of the
following?
Pure H2O
0.1 M K2CrO4
0.25 M KNO3
0.40M AgNO3
Excess Ca(OH)2 is shaken with water to produce a saturated
solution. A 50.00 mL sample of the clear saturated solution is
removed and requires 10.7 mL of 0.1032 M HCl for its titration.
What is the pH of saturated Ca(OH)2?
What is Ksp for this salt?
The solubility of Mg(OH)2 (58.32 g/mol) in a particular buffer
solution is 0.65 g/L. What must be the pH of the buffer
solution?
Mg(OH)2 Ksp = 1.8 x 10-11
Which of the following solids will be more soluble in an acidic
solution than in pure water?
MgCO3
Mg(OH)2
BaSO4
PbBr2
MnS
CaF2
A sample of magnesium oxide (40.30 g/mol) was dissolved in
50.0 mL of 0.183 M HCl. Excess acid was then titrated to a
phenolphthalein endpoint with 13.4 mL of 0.105 M sodium
hydroxide. What was the mass of the magnesium oxide
sample?
Will a precipitate form if 22.5 mg of MgCl2·6H2O (203.3 g/mol)
is added to 325 mL of 0.035 M KF?
MgF2 Ksp = 3.7 x 10-8
A solution is 0.05 M in: Cu2+, Hg2+, and Mn2+. If it is made 0.10
M H2S and 0.10 M HCl what metal sulfides will precipitate?
CuS Kspa = 6 x 10-16
HgS Kspa = 2 x 10-32
MnS Kspa = 3 x 107
A 2.00 M solution of AgNO3 is slowly added to a solution
containing 0.0100 M Cl‾ and 0.250 M I‾. Which ion will
precipitate first?
AgCl Ksp = 1.8 x 10-10
AgI Ksp = 8.5 x 10-17
What is the concentration of this ion when the second begins
to precipitate?
What percentage remains in the solution?