Exam Questions Ch17 Radioactivity and Nuclear Chemistry

Student name:__________

MULTIPLE CHOICE - Choose the one alternative that best completes the statement or answers the question.
1) Which is defined as the maximum amount of solute that will dissolve in a given quantity of solvent at a specific temperature?

A) precipitation
B) combustion
C) solubility
D) super saturation
E) dilution

2) Which substance is present in the smallest proportion in a solution?

A) liquid
B) gas
C) solvent
D) solid
E) solute

3) Which substance is present in the largest proportion in a solution?

A) salute
B) gas
C) solvent
D) solid
E) solute

4) Based on the solubility rules, which one of these compounds is insoluble in water?

A) NaCl
B) MgBr ₂
C) FeCl ₂
D) AgBr
E) ZnCl ₂

5) Based on the solubility rules, which one of these compounds is insoluble in water?

A) Na₂SO₄
B) BaSO ₄
C) CuSO ₄
D) MgSO ₄
E) Rb₂SO₄

6) Based on the solubility rules, which one of these compounds is soluble in water?

A) Hg₂Cl₂
B) Na₂S
C) Ag₂CO₃
D) Ag₂S
E) BaCO ₃

7) Based on the solubility rules, which one of these compounds is soluble in water?

A) AgBr
B) AgCl
C) Ag₂CO₃
D) AgNO ₃
E) Ag₂S

8) Based on the solubility rules, which one of these compounds is soluble in water?

A) CaSO ₄
B) BaSO ₄
C) PbSO ₄
D) K₂SO₄
E) Ag₂SO₄

9) Which of the following is insoluble in water?

A) Li₂CO₃
B) NaOH
C) PbCl ₂
D) Ba(OH) ₂
E) (NH₄)₂S

10) Which of the following is soluble in water?

A) AgCl
B) Rb₂CrO₄
C) Hg₂I₂
D) CaSO ₄
E) PbBr ₂

11) What mass of lithium phosphate is needed to prepare 500. mL of a solution having a lithium ion concentration of 0.125 M?

A) 2.41 g
B) 7.24 g
C) 14.5 g
D) 21.7 g
E) 43.4 g

12) Determine the molarity of a solution made by dissolving 11.7 g of NaNO₃ in water where the final volume of the solution is 250.0 mL.

A) 0.138 M
B) 0.551 M
C) 0.0468 M
D) 0.0311 M
E) 0.214 M

13) Determine the molarity of a solution made by dissolving 11.7 g of Ca(NO₃)₂ in water where the final volume of the solution is 250.0 mL.

A) 0.0713M
B) 0.351M
C) 0.285M
D) 0.0214M
E) 0.0468M

14) Determine the molarity of a solution made by dissolving 8.36 g of MgCl₂ in water where the final volume of the solution is 500.0 mL.

A) 0.0878 M
B) 0.569 M
C) 0.0167 M
D) 0.218 M
E) 0.176 M

15) Determine the molarity of a solution made by dissolving 9.51 g of K₂SO₄ in water where the final volume of the solution is 750.0 mL.

A) 0.789 M
B) 0.0546 M
C) 0.0127 M
D) 0.0728 M
E) 0.137 M

16) Potassium fluoride is used for frosting glass. Calculate the molarity of a solution prepared by dissolving 78.6 g of KF in enough water to produce 225 mL of solution.

A) 0.304 M
B) 0.349 M
C) 1.35 M
D) 3.29 M
E) 6.01 M

17) Determine the volume of a 0.0351 M Li₃PO₄ solution that contains 0.0164 moles of Li₃PO₄.

A) 467 mL
B) 214 mL
C) 576 mL
D) 174 mL
E) 345 mL

18) Determine the volume of a 0.175 M Al(NO₃)₃ solution that contains 0.0591 moles of Al(NO₃)₃.

A) 296 mL
B) 103 mL
C) 967 mL
D) 338 mL
E) 452 mL

19) Determine the volume of a 0.119 M AlPO₄ solution that contains 0.0247 moles of AlPO₄.

A) 340 mL
B) 208 mL
C) 482 mL
D) 294 mL
E) 132 mL

20) Determine the volume of a 0.119 M AlPO₄ solution that contains 21.3 grams of AlPO₄.

A) 0.681 L
B) 1.79 L
C) 0.559 L
D) 1.21 L
E) 1.47 L

21) Determine the volume of a 0.0246 M Li₃PO₄ solution that contains 11.8 grams of Li₃PO₄.

A) 2.41 L
B) 4.80 L
C) 4.14 L
D) 2.08 L
E) 3.19 L

22) Determine the molality of a solution formed by dissolving 0.187 moles of NaCl in 456 grams of water. The density of the solution is 1.44 g/mL.

A) 0.285 m
B) 0.410 m
C) 0.351 m
D) 0.244 m
E) 0.502 m

23) Determine the molality of a solution formed by dissolving 0.0257 moles of Li₃PO₄ in 735 grams of water. The density of the solution is 1.74 g/mL.

A) 0.0189 m
B) 0.0498 m
C) 0.0201 m
D) 0.0350 m
E) 0.0286 m

24) Determine the molality of ions in a solution formed by dissolving 0.0257 moles of Li₃PO₄ in 735 grams of water. The density of the solution is 1.74 g/mL.

A) 0.114 m
B) 0.280 m
C) 0.184 m
D) 0.402 m
E) 0.140 m

25) Determine the molality of ions in a solution formed by dissolving 0.187 moles of NaCl in 456 grams of water. The density of the solution is 1.44 g/mL.

A) 0.820 m
B) 0.702 m
C) 0.351 m
D) 0.410 m
E) 0.285 m

26) A 3.682-g sample of KClO3 is dissolved in enough water to give 375. mL of solution. What is the chlorate ion concentration in this solution?

A) 9.82 M
B) 1.60 × 10⁻¹ M
C) 8.01 ×10⁻² M
D) 9.82 × 10⁻³ M
E) 1.60 × 10⁻² M

27) A 4.691-g sample of MgCl2 is dissolved in enough water to give 750. mL of solution. What is the magnesium ion concentration in this solution?

A) 6.25 M
B) 6.57 × 10⁻² M
C) 4.38 × 10⁻² M
D) 3.29 × 10⁻² M
E) 2.19 ×10⁻² M

28) 35.0 mL of 0.255 M nitric acid is added to 45.0 mL of 0.328 M Mg(NO3)2. What is the concentration of nitrate ion in the final solution?

A) 0.296 M
B) 0.481 M
C) 0.583 M
D) 0.911 M
E) 0.148 M

29) How many sodium ions are present in 325 mL of 0.850 M Na2SO4?

A) 5.12 × 10²³ Na ions
B) 8.32 × 10²² Na ions
C) 1.02 × 10²⁴ Na ions
D) 1.66 × 10²³ Na ions
E) 3.33 × 10²³ Na ions

30) What is the percent CdSO4 by mass in a 1.00 molal aqueous CdSO4 solution?

A) 0.001%
B) 0.10%
C) 17.2%
D) 20.8%
E) 24.4%

31) Calculate the percent by mass of potassium nitrate in a solution made from 45.0 g KNO3 and 295 mL of water at 25ºC. At this temperature, the density of water is 0.997 g/mL.

A) 1.51%
B) 7.57%
C) 13.3%
D) 15.2%
E) 86.7%

32) Copper(II) bromide is used as a wood preservative. What mass of CuBr2 is needed to prepare 750.0 mL of a 1.25 M solution?

A) 134 g
B) 209 g
C) 372 g
D) 750 g
E) 938 g

33) What mass of LiOH is required to prepare 0.250 L of a 3.55 M solution?

A) 0.0371 g
B) 0.888 g
C) 21.3 g
D) 250. g
E) 340. g

34) What is the molality of a solution prepared by dissolving 84.7 g of KMnO4 in 165 g of water?

A) 0.339 m
B) 0.513 m
C) 0.536 m
D) 3.25 m
E) 81.1 m

35) Calcium nitrite is used as a corrosion inhibitor in lubricants. What is the molality of a solution prepared by dissolving 18.5 g of calcium nitrite in 83.5 g of distilled water?

A) 0.181 m
B) 0.222 m
C) 0.596 m
D) 1.35 m
E) 1.68 m

36) Cadmium bromide is used in photography and lithography. What is the molality of a solution prepared by dissolving 45.38 g of CdBr2 in 375.0 g of water?

A) 0.03035 m
B) 0.01600 m
C) 0.1210 m
D) 0.4446 m
E) 16.00 m

37) What mass of water is required to dissolve 27.8 g of ammonium nitrate NH4NO3 in order to prepare a 0.452 m solution?

A) 0.0615 kg
B) 0.100 kg
C) 0.177 kg
D) 0.768 kg
E) 1.30 kg

38) What mass of water is required to dissolve 25.31 g of potassium nitrate (KNO3) in order to prepare a 0.1982 m solution?

A) 0.5101 kg
B) 0.1277 kg
C) 1.000. kg
D) 1.263 kg
E) 0.7917 kg

39) The distinguishing characteristic of all electrolyte solutions is that they

A) contain molecules.
B) conduct electricity.
C) react with other solutions.
D) always contain acids.
E) conduct heat.

40) Which accurately characterizes all nonelectrolyte solutions?

A) Nonelectrolyte solutions contain molecules.
B) Nonelectrolyte solutions conduct electricity.
C) Nonelectrolyte solutions react with other solutions.
D) Nonelectrolyte solutions do not conduct electricity.
E) Nonelectrolyte solutions conduct heat.

41) Which process defines how an ionic compounds break apart into its constituent ions upon dissolution?

A) electrolysis
B) dissociation
C) division
D) ionization
E) decomposition

42) Which of these compounds is a nonelectrolyte?

A) NaF
B) HNO ₃
C) CH₃COOH (acetic acid)
D) NaOH
E) C₆H₁₂O₆ (glucose)

43) Which of these compounds is a nonelectrolyte?

A) NaOH
B) HNO ₃
C) C₂H₆O (ethanol)
D) KF
E) CH₃COOH (acetic acid)

44) The distinguishing characteristic of all nonelectrolyte solutions is that they

A) contain ions.
B) do not conduct electricity.
C) react with other solutions.
D) always contain acids.
E) conducts heat.

45) What volume of concentrated (14.7 M) phosphoric acid is needed to prepare 25.0 L of 3.0 M H3PO4?

A) 0.20 L
B) 0.57 L
C) 1.8 L
D) 3.6 L
E) 5.1 L

46) What volume of a 2.75 M solution of NaOH is required to make 500.0 mL of a 1.27 M solution of NaOH?

A) 231 mL
B) 1.72 L
C) 1.10 L
D) 440 mL
E) 909 mL

47) A 50.0 mL sample of 0.436 M NH4NO3 is diluted with water to a total volume of 250.0 mL. What is the ammonium nitrate concentration in the resulting solution?

A) 2.18 M
B) 0.523 M
C) 0.349 M
D) 0.174 M
E) 0.0872 M

48) What is the molarity of a solution prepared by diluting 1.85 L of 6.5 M KOH to 11.0 L?

A) 0.28 M
B) 0.91 M
C) 1.1 M
D) 3.1 M
E) 3.9 M

49) From the following list of aqueous solutions and water, select the one with the highest boiling point.

A) 1.0 M KNO₃
B) 0.75 M NaCl
C) 0.75 M CuCl₂
D) 2.0 M C₁₂H₂₂O₁₁ (sucrose)
E) pure water

50) From the following list of aqueous solutions and water, select the one with the highest freezing point.

A) 1.0 M KNO₃
B) 0.75 M NaCl
C) 0.75 M CuCl₂
D) 2.0 M C₁₂H₂₂O₁₁ (sucrose)
E) 2.0 M KNO₃

51) In the following diagrams, the black circles represent a solute in solution. Which diagram represents a saturated solution?

A)

B)

C)

D)

E)

52) What is defined as the difference between the freezing point of a pure solvent and the freezing point of the solution?

A) freezing point
B) freezing-point elevation
C) freezing-point depression
D) subzero freezing
E) supercooling

53)

A) 17.6°C
B) −176°C
C) −1.50°C
D) 1.50°C
E) −17.6°C

54) Determine the freezing point of a solution thatcontains 0.31 mol of sucrose in 175 g of water. (For water, Kf = 1.86°C/m)

A) 3.3°C
B) 1.1°C
C) 0.0°C
D) −1.1°C
E) −3.3°C

55) Determine the freezing point of a solution formed by dissolving 0.187 moles of glucose in 456 grams of water. (For water, K_f = 1.86°C/m)

A) −0.410°C
B) −0.351°C
C) −3.48°C
D) –0.763°C
E) –0.528°C

56)

A) 2.5°C
B) −2.5°C
C) −0.70°C
D) 0.70°C
E) −8.9°C

57) Determine the boiling point of a solution formed by dissolving 0.187 moles of glucose in 456 grams of water. (For water, K_b = 0.512°C/m)

A) 100.957°C
B) 101.25°C
C) 100.210°C
D) 100.476°C
E) 100.365°C

58) Determine the boiling point of a solution formed by dissolving 0.312 moles of sugar in 275 grams of water. (For water, K_b = 0.512°C/m)

A) 100.160°C
B) 100.581°C
C) 103.17°C
D) 101.86°C
E) 101.41°C

59) Determine the boiling point of a solution formed by dissolving 0.593 moles of ethanol in 100.0 grams of water. (For water, K_b = 0.512°C/m)

A) 100.329°C
B) 101.58°C
C) 103.04°C
D) 105.93°C
E) 102.91°C

60) What is defined as the selective passage of solvent molecules through a porous membrane from a more dilute solution to a more concentrated solution?

A) permeability
B) semipermeability
C) osmotic pressure
D) osmosis
E) vapor pressure

61) Place the following aqueous solutions in order of increasing osmotic pressure.0.100 m MgCl₂ 0.100 m CH₃OH 0.100 m NaCl

A) 0.100 m CH₃OH < 0.100 m NaCl < 0.100 m MgCl₂
B) 0.100 m MgCl₂ < 0.100 m NaCl < 0.100 m CH₃OH
C) 0.100 m NaCl < 0.100 m MgCl₂ < 0.100 m CH₃OH
D) 0.100 m NaCl < 0.100 m CH₃OH < 0.100 m MgCl₂
E) 0.100 m MgCl₂ < 0.100 m CH₃OH < 0.100 m NaCl

62) Place the following aqueous solutions in order of increasing osmotic pressure.0.100 m Al(NO₃)₃ 0.100 m LiF 0.100 m Ca(C₂H₃O₂)₂

A) 0.100 m Al(NO₃)₃ < 0.100 m Ca(C₂H₃O₂)₂ < 0.100 m LiF
B) 0.100 m Ca(C₂H₃O₂)₂ < 0.100 m Al(NO₃)₃ < 0.100 m LiF
C) 0.100 m Ca(C₂H₃O₂)₂ < 0.100 m LiF < 0.100 m Al(NO₃)₃
D) 0.100 m Al(NO₃)₃ < 0.100 m LiF < 0.100 m Ca(C₂H₃O₂)₂
E) 0.100 m LiF < 0.100 m Ca(C₂H₃O₂)₂ < 0.100 m Al(NO₃)₃