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WorksheetsSolubility And Complex Ion Equilibria (zettyhafiqahizzah)
Total questions: 12
Worksheet time: 9mins
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-]
What type of solution that must be prepared to determine the solubility of solute in water?
saturated
unsaturated
concentrated
supersaturated
Which of the following is commonly used to describe the solubility of a compound?
mass of solution / volume of solute
mass of solute / moles of solute
moles of solution / mass of solute
mass of solute / volume of solution
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
Which of the following shows a net ionic equation?
Mg2+(aq) + CO32-(aq) → MgCO3 (s)
Mg2+(aq) + 2NO3-(aq) + 2Na+(aq) + CO32-(aq) → MgCO3 (s) + 2Na+(aq)
Mg2+(aq) + CO32-(aq) → MgCO3 (s) + Mg2+(aq)
Mg2+(aq) + 2NO3-(aq) + 2Na+(aq) + CO32-(aq) → MgCO3 (s) + 2Na+(aq) + 2NO3- (aq)
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 product constant of calcium chlorate, Ca(ClO3)2 of water is 7.1 x 10-7 at 25 oC. How many grams of Ca(ClO3)2 were dissolved in 750mL?
3.61 x 105 g
2.03 x 10-5 g
8.72 x 10-1 g
3.61 x 10-5 g
If 50.0 mL of 0.0010 M BaCl2 is added to 50.0mL of 0.00010 M Na2SO4, what is the ionic product value of BaSO4 ?
Q = 5.0 x 10-4
Q = 2.5 x 10-8
Q = 5.0 x 104
Q = 2.5 x 108
