Chemistry I - Ch 12 - 15 Study Guide
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____1.A heterogeneous mixture always contains
a. / only one substance.b. / more than two substances.
c. / two or more substances that are visibly distinguishable.
d. / two or more substances that are not visibly distinguishable.
____2.Which of the following is a heterogeneous mixture?
a. / water / c. / whole wheat breadb. / a sugar-water solution / d. / sugar
____3.Which of the following is a homogeneous mixture?
a. / water / c. / whole wheat breadb. / a sugar-water solution / d. / sugar
____4.All of the following are homogeneous mixtures except
a. / soil. / c. / gasoline.b. / a sugar-water solution. / d. / a salt-water solution.
____5.All of the following are heterogeneous mixtures except
a. / whole wheat bread. / c. / tap water.b. / granite. / d. / an oil-water mixture.
____6.Which mixture contains visible particles that settle out unless the mixture is stirred?
a. / a colloid / c. / a solutionb. / a homogeneous mixture / d. / a suspension
____7.Which mixture contains particles that are in a dispersed phase and do not settle out?
a. / a colloid / c. / a solutionb. / a homogeneous mixture / d. / a suspension
____8.A metal solution is a(n)
a. / colloid. / c. / suspension.b. / alloy. / d. / emulsion.
____9.A substance whose water solution is a good conductor of electricity is a(n)
a. / nonelectrolyte. / c. / nonpolar substance.b. / electrolyte. / d. / solute.
____10.Which of the following is an electrolyte?
a. / sodium chloride / c. / pure waterb. / sugar / d. / glass
____11.A substance whose water solution is a poor conductor of electricityis a(n)
a. / polar substance. / c. / electrolyte.b. / nonelectrolyte. / d. / ionic substance.
____12.Which of the following is a molecular substance whose aqueous solution carries an electric current?
a. / liquid hydrogen / c. / sugarb. / hydrogen chloride / d. / iron
____13.Which of the following is a nonelectrolyte?
a. / sodium chloride / c. / sugarb. / hydrogen chloride / d. / potassium chloride
____14.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
____15.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.
____16.Which of the following will dissolve most rapidly?
a. / sugar cubes in cold water / c. / powdered sugar in cold waterb. / sugar cubes in hot water / d. / powdered sugar in hot water
____17.Which of the following will dissolve most slowly?
a. / large salt crystals in unstirred water / c. / small salt crystals in unstirred waterb. / large salt crystals in stirred water / d. / small salt crystals in stirred water
____18.If the amount of solute present in a solution at a given temperature is less than the maximum amount that can dissolve at that temperature, the solution is said to be
a. / saturated. / c. / supersaturated.b. / unsaturated. / d. / concentrated.
____19.A solute crystal is dropped into a solution containing dissolved solute. It falls to the bottom of the beaker and does not dissolve after vigorous stirring. What does this indicate about the solution?
a. / It is probably unsaturated. / c. / It is probably saturated.b. / It is probably supersaturated. / d. / It is not at equilibrium.
____20.Which of the following is likely to produce crystals if disturbed?
a. / an unsaturated solution / c. / a saturated solutionb. / a supersaturated solution / d. / an electrolytic solution
____21.In the expression "like dissolves like," the word like refers to similarity in molecular
a. / mass. / c. / energy.b. / size. / d. / polarity.
____22.Two immiscible substances
a. / exist together in one phase.b. / will not separate on standing.
c. / dissolve freely in one another in any proportion.
d. / will not form a solution.
____23.Pressure has the greatest effect on the solubility of
a. / solids in liquids. / c. / gases in gases.b. / liquids in liquids. / d. / gases in liquids.
____24.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.
____25.As temperature increases, solubility of gases in liquids
a. / increases. / c. / can increase or decrease.b. / decreases. / d. / is not affected.
____26.As temperature increases, solubility of solids in liquids
a. / always increases. / c. / usually increases.b. / always decreases. / d. / usually decreases.
____27.Which of the following expresses concentration?
a. / molality / c. / moles of solute per liter of solutionb. / molarity / d. / All of the above
____28.The concentration of a water solution of NaCl is 2.48 m, and it contains 806 g of water. How much NaCl is in the solution? (molar mass of NaCl = 58.44 g/mol)
a. / 2.00 g / c. / 117 gb. / 89.3 g / d. / 224 g
____29.What mass of water must be used to make a 1.35 m solution that contains 8.20 mol of NaOH? (molar mass of NaOH = 40.00 g/mol)
a. / 6.07 kg / c. / 11.1 kgb. / 7.44 kg / d. / 14.5 kg
____30.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
____31.How many moles of ions are produced by the dissociation of 1 mol of Al2(CO3)3?
a. / 2 mol / c. / 5 molb. / 4 mol / d. / 11 mol
____32.Colligative properties depend on
a. / the identity of the solute particles.b. / the concentration of the solute particles.
c. / the physical properties of the solute particles.
d. / the boiling point and freezing point of the solution.
____33.The freezing point of an aqueous solution that contains a nonelectrolyte is –8.0ºC. What is the molal concentration of the solution? The molal freezing-point constant for water is
–1.86°C/m.
a. / 1.86 m / c. / 4.5 mb. / 4.3 m / d. / 14.8 m
____34.What is the freezing-point depression of an aqueous solution of an electrolyte that produces three ions for every formula unit that dissociates if the electrolyte's concentration is 1.25 m?
Kf = –1.86°C/m.
a. / –1.25°C / c. / –5.58°Cb. / –1.86°C / d. / –6.98°C
____35.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.
____36.As electrolyte concentration decreases, freezing-point depression
a. / approaches the value calculated by assuming complete ionization.b. / gets farther from the value calculated by assuming complete ionization.
c. / remains exactly equal to the value calculated by assuming complete ionization.
d. / approaches 0ºC.
____37.An Arrhenius acid contains
a. / hydrogen that does not ionize.b. / hydrogen that ionizes to form hydrogen ions.
c. / oxygen that ionizes to form hydroxide ions.
d. / oxygen that ionizes to form oxygen ions.
____38.Which of the following is a strong acid?
a. / / c. / CH3COOHb. / H2SO4 / d. / H3PO4
____39.Which of the following is a weak base?
a. / NH3 / c. / NaOHb. / KOH / d. / Ba(OH)2
____40.A Brønsted-Lowry acid is a(n)
a. / electron-pair acceptor. / c. / proton acceptor.b. / electron-pair donor. / d. / proton donor.
____41.A Brønsted-Lowry base is a(n)
a. / producer of OH– ions. / c. / electron-pair donor.b. / proton acceptor. / d. / electron-pair acceptor.
____42.A Lewis acid is
a. / an electron-pair acceptor. / c. / a proton acceptor.b. / an electron-pair donor. / d. / a proton donor.
____43.A Lewis base is a(n)
a. / producer of OH– ions. / c. / electron-pair donor.b. / proton acceptor. / d. / electron-pair acceptor.
____44.In the reaction represented by the equation the conjugate acid of NH3 is
a. / HClO3. / c. / .b. / . / d. / not shown.
____45.In the reaction represented by the equation , the conjugate base of H3O+ is
a. / H2O. / c. / CH3COO–.b. / CH3COOH. / d. / not shown.
____46.In the reaction represented by the equation acts as a(n)
a. / acid. / c. / spectator species.b. / base. / d. / salt.
____47.What is the pH of a neutral solution at 25ºC?
a. / 0 / c. / 7b. / 1 / d. / 14
____48.The pH of an acidic solution is
a. / less than 0. / c. / greater than 7.b. / less than 7. / d. / greater than 14.
____49.The pH of a basic solution is
a. / less than 0. / c. / greater than 7.b. / less than 7. / d. / greater than 14.
Completion
Complete each statement.
50.When a liquid is insoluble in another liquid, the liquids are said to be ______.
51.A substance that does not dissolve in a solvent is said to be ______in that solvent.
52.The maximum amount of solute that can dissolve in a given amount of solvent at a specific temperature and pressure is called ______.
Problem
53.How many grams of NaOH are required to prepare 200. mL of a 0.450 M solution? (molar mass of NaOH = 40.00 g/mol)
54.Calculate the boiling-point elevation of a solution made from 15.0 g of a nonelectrolyte solute and 250.0 g of water. The molar mass of the solute is 50.0 g and Kb=0.51°C/m.
55.What concentration of ethylene glycol is needed to raise the boiling point of water to 105°C? (Kb=0.51°C/m)
56.Use the solubility curve to answer the following: (2 points each)
a.) What type of solution is formed when 50 g of KCl are added to 100 g of water at 30°C?
b.) How many grams of ammonium chloride are needed to make a saturated solution at 60°C in 100 grams of water?
c.) At what temperature is 80g of sodium nitrate soluble?
d.) Which salt has the lowest solubility at 40°C?
57.What is the molarity of a methanol solution that contains 25 g of methanol in 3.5 L of a solution? The molar mass of methanol is 32 g/mol.
58.Calculate the moles of camphor dissolved in 1.32 L of phenol. The molar mass of camphor is 152 g/mol and the molarity of phenol is 6.01 M.