The Solubility Product, Ksp – Practice
Questions:
1) Write the ionic equation and solubility product for the following:
a) Ag2CO3
b) Barium carbonate
c) Magnesium phosphate
2) Determine the Kspvalue of the following
a) Copper(II) carbonate which has a solubility of 9.55 × 10-9 g/100mL
b) Barium hydroxide which has a solubility of 2.33 × 10-5 g/100mL
3) Determine the solubility of the following in mol/L and g/100mL:
a) Iron(II) carbonate which has a Ksp value of 3.13 × 10-11
b) Silver sulfate which has a Ksp value of 1.20 × 10-5
Quick Answers:
1a) Ag2CO3(s) ⇌ 2Ag+(aq) + CO32-(aq)
{ K }_{ sp }=[{ Ag }^{ + }]^{ 2 }[{ CO_{ 3 } }^{ 2- }]
1b) BaCO3(s) ⇌ Ba2+(aq) + CO32-(aq)
{ K }_{ sp }=[{ Ba }^{ 2+ }][{ CO_{ 3 } }^{ 2- }]
1c) Mg3(PO4)2(s) ⇌ 3Mg2+(aq) + PO43-(aq)
{ K }_{ sp }=[{ Mg }^{ 2+ }]^{ 3 }[{ PO_{ 4 } }^{ 3- }]^{ 2 }
2a) 1.4 × 10-10
b) 2.55 × 10-4
3a) 5.6 × 10-6 mol/L, 4.8 × 10-7 g/100mL
3b) 1.4 × 10-2 mol/L, 4.5 × 10-4 g/100mL
Worked Answers: (coming soon)