Question 1

What is the freezing point of a solution prepared from 50.0 g ethylene glycol (C2H6O2) and 85.0 g H2O? (For water, Kf = 1.86°C/m)

Accepted Answer

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

Question 2

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

Accepted Answer

A) Hg2Cl2 
B) Na2S 
C) Ag2CO3 
D) Ag2S 
E) BaCO3 
A) Hg2Cl2 
B) Na2S 
C) Ag2CO3 
D) Ag2S 
E) BaCO3 B

Question 3

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

Accepted Answer

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

Question 4

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

Accepted Answer

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

Question 5

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?

Accepted Answer

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 
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

Question 6

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

Accepted Answer

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

Question 7

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.

Accepted Answer

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

Question 8

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?

Accepted Answer

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

Question 9

Which of the following is insoluble in water?

Accepted Answer

A) Li2CO3 
B) NaOH 
C) PbCl2 
D) Ba(OH)2 
E) (NH4)2S 
A) Li2CO3 
B) NaOH 
C) PbCl2 
D) Ba(OH)2 
E) (NH4)2S

Question 10

Which of these compounds is a nonelectrolyte?

Accepted Answer

A) NaF 
B) HNO3 
C) CH3COOH (acetic acid) 
D) NaOH 
E) C6H12O6 (glucose) 
A) NaF 
B) HNO3 
C) CH3COOH (acetic acid) 
D) NaOH 
E) C6H12O6 (glucose)

Question 11

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

Accepted Answer

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

Question 12

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?

Accepted Answer

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

Question 13

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

Accepted Answer

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

Question 14

The distinguishing characteristic of all electrolyte solutions is that they

Accepted Answer

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

Question 15

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

Accepted Answer

A) Freezing point 
B) freezing-point elevation 
C) freezing-point depression 
D) Subzero freezing 
E) Supercooling 
A) Freezing point 
B) freezing-point elevation 
C) freezing-point depression 
D) Subzero freezing 
E) Supercooling

Question 16

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

Accepted Answer

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

Question 17

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

Accepted Answer

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

Question 18

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

Accepted Answer

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

Question 19

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.

Accepted Answer

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

Question 20

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

Accepted Answer

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

What is the freezing point of a solution prepared from 50.0 g ethylene glycol (C₂H₆O₂) and 85.0 g H₂O? (For water, K_f = 1.86°C/m)

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

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

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

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?

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

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 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?

Which of the following is insoluble in water?

Which of these compounds is a nonelectrolyte?

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

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?

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

The distinguishing characteristic of all electrolyte solutions is that they

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

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)

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

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

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.

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

Atoms and Elements

Electrons and the Periodic Table

Compounds and Chemical Bonds

How Chemists Use Numbers

The Mole and Chemical Formulas

Molecular Shape

Solids, Liquids, and Phase Changes

Gases

Chemical Reactions and Chemical Equations

Using Balanced Chemical Equations

Acids and Bases

Equilibrium

Organic Chemistry

Biochemistry

Nuclear Chemistry

Electrochemistry

Filters

Exam 9: Physical Properties of Solutions

What is the freezing point of a solution prepared from 50.0 g ethylene glycol (C2H6O2) and 85.0 g H2O? (For water, Kf = 1.86°C/m)

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

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

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

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?

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

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 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?

Which of the following is insoluble in water?

Which of these compounds is a nonelectrolyte?

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

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?

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

The distinguishing characteristic of all electrolyte solutions is that they

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

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

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

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

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.

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

Atoms and Elements

Electrons and the Periodic Table

Compounds and Chemical Bonds

How Chemists Use Numbers

The Mole and Chemical Formulas

Molecular Shape

Solids, Liquids, and Phase Changes

Gases

Chemical Reactions and Chemical Equations

Using Balanced Chemical Equations

Acids and Bases

Equilibrium

Organic Chemistry

Biochemistry

Nuclear Chemistry

Electrochemistry

Filters

What is the freezing point of a solution prepared from 50.0 g ethylene glycol (C₂H₆O₂) and 85.0 g H₂O? (For water, K_f = 1.86°C/m)

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

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?

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

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 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?

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

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)

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

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

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.