PAP Test Review: Solutions
1. Determine if the following molecules are electrolytes or non-electrolytes.
a. NaCl
b. C2H5OH
c. MgCl2
d. CH4
e. C6H12O6
f. CuF2
g. (NH4)2S
2. Determine which of the following molecules conducts electricity.
a. NaCl
b. C2H5OH
c. MgCl2
d. CH4
e. C6H12O6
f. CuF2
g. (NH4)2S
3. What kind of compound conducts electricity? Why?
4. What kind of compounds are NOT conductive? Why?
5.
a.
b.
c.
d.
Which one of the following has the highest boiling point/conductivity?
0.2 M NaNO3
0.1 M CH4
0.25 M (NH4)Cl
0.2 M AlCl3
6.
a.
b.
c.
d.
Which one of the following has NO conductivity?
0.2 M Na2(CO3)
0.1 M C6H12O6
0.25 M (NH4)3(PO4)
0.2 M CaCl2
7.
a.
b.
c.
d.
Which of the following has the most ions in solution?
0.1 M NaCl
0.2 M C2H5OH
0.1 M MgCl2
0.1 M (NH4)3(PO4)
8.
a.
b.
c.
d.
Which of the following has no ions in solution?
0.1 M NaCl
0.2 M C2H5OH
0.1 M MgCl2
0.1 M (NH4)3(PO4)
9. Rank the following solutions in order of not conductive to most conductive:
0.1 M C12H22O11
0.1 M (NH4)(MnO4)
0.1 M MgCl2
0.1 M Al2S3
0.1 M Na3P
10. For the substances below, identify the solute and the solvent.
a. Iced tea sweetened with sugar
b. an aqueous solution of sodium chloride
c. adding 50 mL of oil to 350 mL of water
11. Calculate the molarity of a Na2(SO4) solution that contains 25.2 g of Na2(SO4) and 25 mL of water.
12. Calculate the volume of water that would be needed to make a 1.25 M solution with 12.6 grams of
CaCl2.
13. Calculate the mass of NaCl needed to make a 3.25 M solution with 215 mL of water.
14. How many mL of 2.56 M HNO3 must be diluted to obtain 250 mLs of a 1.25 M solution? How many
mL of H2O must be included?
15. 0.25 liters of a 6 M solution is diluted to 0.5 liters. What is the molarity of the new solution?
16. What does the phrase “like dissolves in like” mean? (What kind of substances will water dissolve?)
17. Determine whether the molecules below are polar or non-polar.
a. H2O
b. CCl4
18. Your teacher had 2 beakers set up in the laboratory and asked you to determine whether they are
saturated, unsaturated or supersaturated solutions. Based off the information provided below, label the
beakers, accordingly.
Accumulation of salt on
bottom of the beaker
19. If you had a container of 12.5 M hydrochloric acid, how much would be needed to make
0.5 liters of 2 M solution?
20. What are 3 ways to increase the solubility of a solution?
21. Two students were having a race in their Chemistry class. One claimed that if he dropped 2 grams of
granulated sugar in a 250 mL beaker, it would dissolve the fastest. His lab partner, however, claimed
that if he dropped a sugar cube (still 2 grams) into a 250 mL beaker of water, it would dissolve the
fastest.
Who do you think would win this race? Explain your answer.
22. If a solution has a high concentration of ions in solution, what can you determine about its:
Boiling point? __________________________________________
Conductivity? __________________________________________
23. Determine the solubility (soluble or insoluble) of the following compounds if they were products in a
reaction:
a. Ca3(PO4)2
b. NaCl
c. AgNO3
d. PbI2
e. Pb(NO3)2
f. Li2S
g. Na2CO3
h. CaSO4
i. CaCO3
j. (NH4)2S
k. K3PO4
24. Understand ALL labs we did this unit.
a. water, oil, and soap
b. mystery pen
c. Molarity murder
d. gravity flow machine
Using your solubility curve, answer the following questions.
25. How many grams of NH4Cl can be dissolved in 100 g of water at 50°C?
26. How many grams of NaNO3 can be dissolved in 105 g of water at 10°C?
27. Calculate how many grams of KCl will crystallize when 100 grams of water saturated with KCl at 80°C
and then is cooled to 10°C.
28. Determine if the following solutions are supersaturated, unsaturated, or saturated.
a. 120 g of NaNO3 in 100 g of H2O at 40°C.
b. 60 g of NH4Cl in 100 g of H2O at 60°C.
c. 80 g of KNO3 in 100 g of water at 50°C.
d. 30 g of NaCl in 100 g of water at 80°C.