Test tasks

 

 

1. A compound has a solubility of 7.1 × 10-5 M at 25 oC. The compound is …
A. CuS
B. AgBr
C. CaCO3
D. CaSO4
2. A saturated solution of NaCl contains 36.5 g of solute in 0.100 L of solution. The solubility of the compound is
A. 0.062 M
B. 1.60 M
C. 3.65 M
D.24 M
3. Ksp expression for a saturated solution of Mg(OH)2 is
A. Ksp = [Mg(OH)2]
B. Ksp = [Mg2+][OH-]2
C. Ksp = [Mg2+][OH-]
D. Ksp = [Mg2+][2OH-]2
4. Which of the following will not produce a precipitate when equal volumes of 0.20 M solutions are combined?
A. KOH and CaCl2
B. Zn(NO3)2 and K3PO4
C. Sr(OH)2 and (NH4)2S
D. Na2SO4 and Pb(NO3)2
5. Which of the following will dissolve in water to produce a molecular solution?
A. CaCl2
B. NaOH
C. CH3OH
D. Sr(OH)2
6. In a solubility equilibrium, the …
A. rate of dissolving equals the rate of crystallization
B. neither dissolving or crystallization occurs
C. concentration of solute and solvent are equal
D. mass of dissolved solute is greater than the mass of the solution
7. Which of the following units could be used to describe solubility?
A. g/s
B. g/L
C. M/L
D. mol/s
8. Silver chloride, AgCl, would be least soluble in
A. 1.0 M HCl
B. 1.0 M NaNO3
C. 1.0 M ZnCl2
D. 1.0 M AgNO3
9. The Ksp expression for a saturated solution of AgCO3 is
A. Ksp = [Ag2+][CO32-]
B. Ksp = [Ag+]2[CO32-]
C. Ksp = [2Ag+][CO32-]
D. Ksp = [2Ag+]2[CO32-]
10. How many moles of solute are dissolved in 200.0 mL of a saturated solution of FeS?
A. 1.2 × 10-19
B. 6.0 × 10-19
C. 1.5 × 10-10
D. 7.7 × 10-10
11. Which of the following does not define solubility?
A. the concentration of solute in a saturated solution
B. the moles of solute dissolved in a given amount of solution
C. the maximum mass of solute that can dissolve in a given amount of solution
D. the minimum amount of solute required to produce one litre of saturated solution
12. The solubility of CdS is 2.8 × 10-14 M. The value of the Ksp is
A. 7.8 × 10-28
B. 2.8 × 10-14
C. 5.6 × 10-14
D. 1.7 × 10-7
13. What is observed when H2SO4 is added to a saturated solution of CaSO4?
A. CaSO4(s) dissolves
B. the [Ca2+] increases
C. bubbles of H2 are given off
D. additional CaSO4 precipitates
14. The solubility of SrF2 is
A. 4.3 × 10-9
B. 6.6 × 10-5
C. 1.0 × 10-3
D. 1.6 × 10-3
15. Calculate the [Li+] in 200.0 mL of 1.5 M Li2SO4.
A. 0.30 M
B. 0.60 M
C. 1.5 M
D. 3.0 M
16. Consider the following saturated solution solutions

CuSO4 BaSO4 CaSO4

The order of cation concentration, from highest to lowest, is
A. [Ba2+] > [Ca2+] > [Cu2+]
B. [Ca2+] > [Cu2+] > [Ba2+]
C. [Cu2+] > [Ca2+] > [Ba2+]
D. [Cu2+] > [Ba2+] > [Ca2+]
17. The ion concentrations in 0.25 M Al2(SO4)3 are

[Al3+] [SO42-]
A. 0.25 M; 0.25 M
B. 0.50 M; 0.75 M
C. 0.75 M; 0.50 M
D. 0.10 M; 0.15 M
18. Consider the following equilibrium: Mg(OH)2(s) ⇄ Mg2+(aq) + 2OH-(aq)

A compound that can be added to cause a shift to the right is
A. NaOH
B. HCl
C. Sr(OH)2
D. Mg(OH)2
19. A solution contains both Ag+ and Mg2+ ions. During selective precipitation, these ions are removed one at a time by adding
A. I- followed by OH-
B. OH- followed by S2-
C. SO42- followed by Cl-
D. NO3- followed by PO43-
20. The solubility of SnS is 3.2 × 10-3 M. The value of the Ksp is
A. 1.0 × 10-5
B. 3.2 × 10-3
C. 6.4 × 10-3
D. 5.7 × 10-2