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WorksheetsSolubility
Total questions: 10
Worksheet time: 50mins
The Ksp expression for a saturated solution of Ca3(PO4)2 is
Ksp = [Ca2+][PO43-]
Ksp = [3Ca2+][2PO43-]
Ksp = [Ca2+]3[PO43-]2
Ksp = [3Ca2+]3[2PO43-]2
What is the Ksp expression for an ionic compund of BaSO4
Ksp= [Ba2+][SO42-]
Ksp= [Ba2+][4SO42-]4
Ksp= [Ba2+][4SO42-]
Ksp= [2Ba2+][4SO42-]
The molar solubility of silver sulphide is 5.0 x 10-17 mol/L. Calculate its solubility product.
Ksp = 5 x 1049
Ksp = 5 x 1033
Ksp = 5 x 10-49
Ksp = 5 x 10-33
The solubility product of silver chromate (VI) at room temperature is 2.4 x 10-12. Calculate the molar solubility of Ag+(aq) and CrO42-(aq) ions in a saturated solution of silver chromate (VI) at room temperature.
Ag+ = 1.68 x 104 M and CrO42- = 8.4 x 10-5 M
Ag+ = 1.68 x 104 M and CrO42- = 8.4 x 105 M
Ag+ = 1.68 x 10-4 M and CrO42- = 8.4 x 105 M
Ag+ = 1.68 x 10-4 M and CrO42- = 8.4 x 10-5 M
What will happen if some solid AgNO3 is added to a saturated solution of AgCl ?
The AgNO3 will not dissolve
More solid AgCl will dissolve
More solid AgCl will produced
There will be no effect on AgCl equilibrium
The Ksp value for PbF2 is 4 x 10-8. Calculate the molar solubility of solid PbF2 in a 0.5M NaF solution.
8 x 108
1.6 x 107
8 x 10-8
1.6 x 10-7
A person mixes 100.0 mL of 0.0015M CaCl2 and 50.0 mL of 0.0081M K2SO4. If the Ksp for CaSO4 is 2.4 x 10-5 , will a CaSO4 precipitate be observed?
No precipitate occur
Precipitate occur
The solubility of CuI is 2 × 10–6 molar. What is the solubility product constant, Ksp, for CuI?
1.4 × 10–3
2 × 10–6
4 × 10–12
2 × 10–12
Which of the following statements is held true about the common-ion effect on the equilibrium of solubility of salt ?
(you may choose more than one answer)
Adding common-ion to the solution containing dissolved salt cause the solubility equilibrium shifts to the formation of undissolved salt
Adding common-ion to the solution containing dissolved salt cause the numerical value of Ksp of corresponding salt changes
Solubility of salt in solution containing common-ion is greater than that of pure water.
Consider a beaker containing 100 ml of water, with solid AgCl on the bottom.
Which of the following statements is held true if NaCl is added to the solution?
(you may choose more than one answer)
The amount of AgCl solid at the bottom of the beaker increases
The amount of AgCl solid at the bottom of the beaker decreases
The concentration of dissolved Ag+ ion in the solution stays the same
The concentration of dissolved Ag+ ion in the solution changes
