Chemistry 12 Mid-year Exam Review (Part 2)
1. Which of the following compounds produce ionic solutions when dissolved in water? Which of them
produce molecular solutions?
CH3OH
Ca(NO3)2
C12H22O11
SO2
Cu(OH)2
Na2SO4
HCl
2. What is each individual ion’s concentration when 250 mL of 0.36 M Sr(OH)2 are added to 750 mL of
water?
3. Which one of the following produces a saturated solution of the greatest [Pb2+]?
PbCl2
PbSO4
Pb(NO3)2
Pb(IO3)2
4. Devise a procedure to separate Be2+, Pb2+ and Sr2+ from an aqueous solution containing all three cations.
Write the relevant net ionic equations for each step.
5. Calculate the molar solubility of SrF2, if 0.054 g dissolves in 350.0 mL of water to form a saturated
solution.
6. The solubility of Ag2SO4 is 1.2 g per 100 mL. Calculate the molar solubility.
7. Write the balanced formula, complete and net ionic equation for the following mixtures:
a. FeCl3(aq) and AgNO3(aq)
b. MgBr2(aq) and Li2CO3(aq)
c. CuSO4(aq) and NaOH(aq)
8. Will a precipitate form in the following mixtures?
a. 10.0 mL of 0.20 M Pb(NO3)2 and 10.0 mL of 0.20 M NaI?
b. 10.0 mL of 0.20 M (NH4)2S and 10.0 mL of 0.20 M LiOH?
c. 10.0 mL of 0.20 M CaBr2 and 10.0 mL of 0.20 M K2SO3?
9. Write the Ksp expressions for the following salts:
a. BaCrO4
b. SrF2
c. Fe3(PO4)2
10. Calculate the solubility of silver chromate (in g/L).
11. Calculate the molar solubility of strontium carbonate.
12. Calculate the [Ca2+] (in mol/L) that exists in a saturated solution of CaSO4.
13. 1.2×10–3 mol of lead(II) iodide dissolves in 1.0 L of aqueous solution at 22ºC. What is the solubility
product constant at this temperature?
14. Calculate the molar solubility of Mg(OH)2.
15. If 25.0 mL of 4.00×10–4 M Pb(NO3)2(aq) is mixed with 35.0 mL of 1.89×10–5 M NaIO3, will a precipitate
form?
16. If 2.00 mL of 6.28×10–6 M CdCl2(aq) and 93.0 mL of 4.53×10–6 M NaOH(aq) are mixed, will a precipitate
form? Ksp of Cd(OH)2 is 2.5×10–14.
17. What is the [C2O42–] (in mol/L) in a saturated solution of CaC2O4?
18. Consider a saturated solution of PbI2:
PbI2(s)
Pb+(aq) + 2 I–(aq)
What is the maximum [Cu2+] that can exist in a saturated solution of PbI2 without forming a precipitate?
19. A 20.00 mL sample containing Cl– was titrated with 0.1600 M AgNO3, using Na2CrO4 as indicator. At
the equivalence point, 15.50 mL of AgNO3 had been added. What was the original [Cl–] in the sample?
20. What mass of MgCO3 is required to make 700.0 mL of a saturated solution?
21. A suspension of barium sulfate is used to improve the quality of X-rays in the digestive system. If a
patent is required to drink 0.400 L of this suspension, calculate the actual mass (in g) of dissolved
barium sulfate?
22. A 25.00 mL of a saturated ZnF2 solution was evaporated to dryness. The mass of the residue was
0.508 g. Calculate the solubility product constant of ZnF2.
23. In which of the following solutions is SrCO3 the most soluble?
0.1 M SrCl2
0.1 M Na2CO3
0.1 M HCl
24. Adding which of the following to a saturated solution of Fe(OH)3 will increase its solubility?
0.1 M FeCl3
0.1 M HNO3
0.1 M LiOH
0.1 M HBr
25. Define Arrhenius base.
26. Define Brønsted-Lowry acid.
27. Write and balance the neutralization reaction between H3PO4 and Mg(OH)2.
28. Write the neutralization reactions for the following mixtures. For each, identify the conjugate acid-base
pairs and which species (in the pairs) is the acid and which is the base. Note: Assume the transfer of
only one proton.
a. HSO4– and CN–
b. H3BO3 and HCO3–
c. OH– and H2S
29. How many of the following species are amphiprotic?
H3O+
HF
HPO42–
C2O42–
NO3–
HC6H5O7–
H2O
30. Which of the following is a strong and dilute base? Weak and dilute acid? Strong and concentrated acid?
2 M HCl
2 M NaOH
0.00010 M HF
0.00010 M HCl
0.00010 M Na2CO3