Solutions Test Review
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____1.Which of the following is a homogeneous mixture?
a. / water / c. / whole wheat breadb. / a sugar-water solution / d. / sugar
____2.Which of the following is a homogeneous mixture of substances in a single phase?
a. / a solution / c. / a compoundb. / a colloid / d. / a suspension
____3.Which is not an example of a colloid?
a. / paint / c. / butterb. / smoke / d. / sugar water
____4.Which mixture is made up of the smallest particles?
a. / milk / c. / shaving creamb. / salt water / d. / muddy water
____5.Colloids
a. / can be separated by filtering. / c. / scatter light.b. / settle out when allowed to stand. / d. / contain particles larger than 1000 nm.
____6.A substance whose water solution is a good conductor of electricity is a(n)
a. / nonelectrolyte. / c. / nonpolar substance.b. / electrolyte. / d. / solute.
____7.A substance whose water solution is a poor conductor of electricityis a(n)
a. / polar substance. / c. / electrolyte.b. / nonelectrolyte. / d. / ionic substance.
____8.Which of the following does not increase the rate of dissolving a solid in water?
a. / raising the temperature of the waterb. / stirring the solution
c. / using larger pieces of solid
d. / crushing the solid
____9.Increasing the surface area of the solute
a. / increases the rate of dissolution.b. / decreases the rate of dissolution.
c. / has no effect on the rate of dissolution.
d. / can increase, decrease, or have no effect on the rate of dissolution.
____10.Stirring increases the rate of dissolution because it
a. / raises the temperature.b. / lowers the temperature.
c. / brings fresh solvent into contact with the solute.
d. / decreases the surface area of the solute.
____11.If a solution is not agitated while it is being made, dissolved solute tends to
a. / mix uniformly. / c. / build up in the solvent near the solute.b. / build up in the solvent far from the solute. / d. / raise the temperature of the solvent.
____12.Which of the following is at equilibrium when undissolved solute is visible?
a. / a saturated solution / c. / a supersaturated solutionb. / an unsaturated solution / d. / All of the above
____13."Like dissolves like" is a very general rule used for predicting whether
a. / one substance will form a solution with another.b. / one substance will react with another.
c. / a reaction will reach equilibrium.
d. / a mixture will contain two or three phases.
____14.Which of the following is an example of a nonpolar solvent?
a. / water / c. / Both (a) and (b)b. / toluene / d. / Neither (a) nor (b)
____15.Which of the following is a solvent for both polar and nonpolar solutes?
a. / water / c. / ethanolb. / carbon tetrachloride / d. / benzene
____16.Which of the following releases energy?
a. / overcoming solute-solute attraction / c. / overcoming solvent-solvent attractionb. / forming solute-solvent attraction / d. / All of the above
____17.Increasing temperature favors dissolution when
a. / the enthalpy of solution is negative. / c. / dissolution occurs rapidly.b. / the enthalpy of solution is positive. / d. / the dissolution process is exothermic.
____18.The solubility of gases in liquids
a. / increases with increasing pressure. / c. / decreases with increasing pressure.b. / cannot reach equilibrium. / d. / does not depend on pressure.
____19.As temperature increases, solubility of solids in liquids
a. / always increases. / c. / usually increases.b. / always decreases. / d. / usually decreases.
____20.What is the molarity of a solution that contains 0.202 mol KCl in 7.98 L solution?
a. / 0.0132 M / c. / 0.459 Mb. / 0.0253 M / d. / 1.363 M
____21.What is the molarity of a solution that contains 125 g NaCl in 4.00 L solution? (molar mass of NaCl = 58.44 g/mol)
a. / 0.535 M / c. / 8.56 Mb. / 2.14 M / d. / 31.3 M
____22.How many milliliters of a 0.171 M solution contain 1.00 g of NaCl? (molar mass of NaCl = 58.44 g/mol)
a. / 100. mL / c. / 171 mLb. / 1000. mL / d. / 17.1 mL
____23.How many ions are produced by each formula unit of solid in a dissociation?
a. / zero / c. / twob. / one / d. / two or more
____24.How many moles of ions are produced by the dissociation of 1 mol of MgCl2?
a. / 0 / c. / 2 molb. / 1 mol / d. / 3 mol
____25.What is the net ionic equation for the precipitation reaction between BaCl2 and Na2SO4?
a. / BaCl2(aq) + Na2SO4(aq) ? BaSO4(s) + 2NaCl(aq)b. / Na+(aq) + Cl-(aq) ? NaCl(s)
c. / Ba2+(aq) + SO42-(aq) ? BaSO4(s)
d. / Ba2+(aq) + 2Cl-(aq) + 2 Na+(aq) + SO42-(aq) ? BaSO4(s) + 2Cl-(aq) + 2Na+(aq)
____26.What is the net ionic equation for the precipitation reaction between silver nitrate solution and sodium sulfide solution?
a. / 2Ag+(aq) + 2NO3–(aq) + 2Na+(aq) + S2–(aq) Ag2S(s) + 2Na+(aq) + 2NO3–(aq)b. / 2Ag+(aq) + S2–(aq) Ag2S(s)
c. / Na+(aq) + NO3–(aq) NaNO3(s)
d. / 2Ag+(aq) + 2NO3–(aq) + 2Na+(aq) + S2–(aq) Ag2S(s) + 2NaNO3(s)
____27.What is the net ionic equation for the precipitation reaction between copper(II) chloride and sodium hydroxide?
a. / Cu2+(aq) + 2OH–(aq) Cu(OH)2(s)b. / Na+(aq) + Cl–(aq) NaCl(s)
c. / Cu2+(aq) + 2OH–(aq) + 2Cl–(aq) Cu(OH)2(s) + 2Cl–(aq)
d. / Cu2+(aq) + 2Cl–(aq) + 2Na+(aq) + 2OH–(aq) Cu(OH)2(s) + 2NaCl(s)
____28.Ions are formed from solute molecules by the action of the solvent in a process called
a. / ionization. / c. / precipitation.b. / dissociation. / d. / oxidation.
____29.Which of the following is a molecular compound that ionizes in water?
a. / NaCl / c. / HClb. / Cl2 / d. / C6H6
____30.Why is vapor-pressure lowering a colligative property?
a. / It is independent of the concentration of a nonelectrolyte solute and does not depend on solute identity.b. / It depends on the concentration of an electrolyte solute and does not depend on solute identity.
c. / It depends on the concentration of a nonelectrolyte solute and on solute identity.
d. / It depends on the concentration of an electrolyte solute and on solute identity.
____31.A water solution containing an unknown quantity of a nonelectrolyte solute has a freezing point of –0.665C. What is the molal concentration of the solution if Kf = –1.86C/m?
a. / 0.010 m / c. / 0.358 mb. / 0.355 m / d. / 2.66 m
____32.Compared with a 0.01 m sugar solution, a 0.01 m KCl solution has
a. / the same freezing-point depression.b. / about twice the freezing-point depression.
c. / the same freezing-point elevation.
d. / about six times the freezing-point elevation.
____33.Compared with a 0.01 m sugar solution, a 0.01 m MgCl2 solution has
a. / the same freezing-point depression.b. / about twice the freezing-point depression.
c. / about three times the freezing-point depression.
d. / about four times the freezing-point depression.
Solutions Test Review
Answer Section
MULTIPLE CHOICE
1.ANS:BPTS:1DIF:IIREF:1
OBJ:1STA:PS.9.9
2.ANS:APTS:1DIF:IREF:1
OBJ:1STA:PS.9.9
3.ANS:DPTS:1DIF:IREF:1
OBJ:3STA:PS.9.9
4.ANS:BPTS:1DIF:IIREF:1
OBJ:3STA:PS.9.9
5.ANS:CPTS:1DIF:IREF:1
OBJ:3STA:PS.9.9
6.ANS:BPTS:1DIF:IREF:1
OBJ:4STA:PS.9.9
7.ANS:BPTS:1DIF:IREF:1
OBJ:4STA:PS.9.9
8.ANS:CPTS:1DIF:IREF:2
OBJ:1
9.ANS:APTS:1DIF:IREF:2
OBJ:1
10.ANS:CPTS:1DIF:IREF:2
OBJ:1
11.ANS:CPTS:1DIF:IREF:2
OBJ:1
12.ANS:APTS:1DIF:IREF:2
OBJ:2STA:PS.12.2
13.ANS:APTS:1DIF:IREF:2
OBJ:3STA:PS.9.9
14.ANS:BPTS:1DIF:IIREF:2
OBJ:3STA:PS.9.9
15.ANS:CPTS:1DIF:IREF:2
OBJ:3STA:PS.9.9
16.ANS:BPTS:1DIF:IREF:2
OBJ:4STA:PS.9.16
17.ANS:BPTS:1DIF:IREF:2
OBJ:4STA:PS.9.16
18.ANS:APTS:1DIF:IREF:2
OBJ:5STA:PS.12.2
19.ANS:CPTS:1DIF:IREF:2
OBJ:5STA:PS.12.2
20.ANS:B
Solution:
PTS:1DIF:IIIREF:3OBJ:1
21.ANS:A
Solution:
PTS:1DIF:IIIREF:3OBJ:1
22.ANS:A
Solution:
PTS:1DIF:IIIREF:3OBJ:3
23.ANS:DPTS:1DIF:IREF:1
OBJ:1STA:PS.9.5
24.ANS:DPTS:1DIF:IIREF:1
OBJ:1STA:PS.9.5
25.ANS:CPTS:1DIF:IIREF:1
OBJ:2STA:PS.9.5
26.ANS:BPTS:1DIF:IIREF:1
OBJ:2STA:PS.9.5
27.ANS:APTS:1DIF:IIREF:1
OBJ:2STA:PS.9.5
28.ANS:APTS:1DIF:IREF:1
OBJ:3STA:PS.9.5
29.ANS:CPTS:1DIF:IIREF:1
OBJ:3STA:PS.9.5
30.ANS:APTS:1DIF:IREF:2
OBJ:1STA:PS.9.9
31.ANS:CPTS:1DIF:IIIREF:2
OBJ:2STA:PS.9.9
32.ANS:BPTS:1DIF:IIREF:2
OBJ:3STA:PS.9.9
33.ANS:CPTS:1DIF:IIREF:2
OBJ:3STA:PS.9.9