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- 1. Multiple Choice
How does a solution become supersaturated?dissolve lots of solute in it.dissolve a little solute in it.dissolve more solute than you should be able to.dissolve a super amount of solvent in it. - 2. Multiple ChoiceSolution where more solute can still be dissolved at the given temperature.SaturatedUnsaturatedSupersaturatedHomogeneous solution
- 3. Multiple Choice
The amount of solute actually dissolved in a given amount of solvent is known as______________________.
dilution
solubility or concentration
saturated solution
supersaturated mixture
- 4. Multiple ChoiceWhen a solvent contains as much of the solute as it can hold, the solution is said to besupersaturateddilutedsaturatedunsaturated
- 5. Multiple ChoiceYou can make a solution more concentrated by adding __________.solutesolventwater
- 6. Multiple ChoiceSolution where more solute can still be dissolved at the given temperature.SaturatedUnsaturatedSupersaturatedHomogeneous solution
- 7. Multiple Choice
Which of the following shows the correct dissolution reaction for BaCl2?
- 8. Multiple Choice
Given that the molar solubility of Sn(OH)2 is "s".
The correct mathematical expression for solubility product constant of Sn(OH)2 is:
2s2 = Ksp
2s3 = Ksp
4s3 = Ksp
8s3 = Ksp
- 9. Multiple Choice
Which of the following is the correct units of the solubility product, Ksp for AgCl?
mol dm-3
mol2 dm-6
mol3 dm-9
mol4 dm-12
no unit
- 10. Multiple Choice
Which of the following is the correct units of the solubility product, Ksp for PbI2?
mol dm-3
mol2 dm-6
mol3 dm-9
mol4 dm-12
no unit
- 11. Multiple Choice
Which of the following is the correct units of the solubility product, Ksp for BaSO4?
mol dm-3
mol2 dm-6
mol3 dm-9
mol4 dm-12
no unit
- 12. Multiple Choice
Which of the following is the correct units of the solubility product, Ksp for Ag2CO3?
mol dm-3
mol2 dm-6
mol3 dm-9
mol4 dm-12
no unit
- 13. Multiple Choice
"As temperature increases, the solubility for a slightly soluble salt will also increases."
Is the above statement correct?
Yes, because as the temperature increases, solubility of the ionic compound increases.
No, because the Ksp is the same at all the temperature.
No, because the Ksp will change as the temperature change and it is depends on the type of reaction (endothermic or exothermic reaction)
Yes, because as the temperature increases, solubility of ionic compound decreases and Ksp increases.
- 14. Multiple Choice
For an exothermic reaction,
as the temperature of the solution increases,
solubility of the salt increases ; Ksp increases
solubility of the salt increases ; Ksp decreases
solubility of the salt decreases ; Ksp increases
solubility of the salt decreases ; Ksp decreases
- 15. Multiple Choice
For an endothermic reaction,
as the temperature of the solution increases,
solubility of the salt increases ; Ksp increases
solubility of the salt increases ; Ksp decreases
solubility of the salt decreases ; Ksp increases
solubility of the salt decreases ; Ksp decreases
- 16. Multiple Choice
The molar solubility of PbI2 is 1.52 x 10-3 M. Calculate the value of Ksp for PbI2.
3.51 x 10-9 mol3 dm- 9
1.40 x 10-8 mol3 dm- 9
4.62 x 10-6 mol3 dm- 9
1.52 x 10-3 mol3 dm- 9
- 17. Multiple ChoiceSilver chromate, Ag2CrO4, has a Ksp of 8.96 x 10-12. Calculate the solubility in mol/L of silver chromate.1.31 x 10-4M1.65 x 10-4M2.25 x 10-12M2.08 x 10-4M
- 18. Multiple Choice
An unknown salt, M2Z, has a Ksp of 3.3 x 10-9. Calculate the solubility in mol/L of M2Z.
2.9 x 10-4 M
5.7 x 10-4 M
9.4 x 10-4 M
3.7 x 10-4 M
- 19. Multiple Choice
A saturated solution is formed when
Qsp = Ksp
Qsp > Ksp
Qsp < Ksp
- 20. Multiple Choice
Precipitation of silver chloride , AgCl will occur when
Qsp = Ksp
Qsp > Ksp
Qsp < Ksp
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