Solutions are made that contain 0.10 moles of each of the following compounds in 100 g of H2O. Choose the compound whose solution will have the highest freezing point.

A) K2SO4 B) NaI C) Mg(CH3CO2)2 D) Ca3(PO4)2 E) Sr(NO3)2 A) K2SO4 B) NaI C) Mg(CH3CO2)2 D) Ca3(PO4)2 E) Sr(NO3)2

An unknown compound is composed of 65.44% C, 29.07% O, and 5.49% H. A sample weighing 5.34 g, when dissolved in 60.00 g H2O, lowers the freezing point to -0.600°C. What is the molecular formula of the compound? (Kf for water = 1.86°C/m; C = 12.0, O = 16.0, H = 1.0 g/mol).

A) C3H3O B) CHO C) C14H11O6 D) C5H5O5 E) C7H5O3 A) C3H3O B) CHO C) C14H11O6 D) C5H5O5 E) C7H5O3

100 mL of LiNO3, 0.241 M is mixed with 240 mL of 0.618 M Ca(NO3)2. What is the final concentration of NO3- in the solution?

A) 0.508 M B) 1.01 M C) 0.943 M D) 0.756 M E) 1.38 M A) 0.508 M B) 1.01 M C) 0.943 M D) 0.756 M E) 1.38 M

Commercial perchloric acid is 70.0% by mass, HClO4(aq), and has a density of 1.67 g/mL. Calculate the mole fraction of perchloric acid in the solution.

A) 0.295 B) 0.420 C) 0.705 D) 0.697 A) 0.295 B) 0.420 C) 0.705 D) 0.697

Commercial perchloric acid is 70.0% by mass, HClO4(aq), and has a density of 1.67 g/mL. Calculate the molarity of perchloric acid in the solution.

A) 11.5 M B) 1.17 M C) 23.7 M D) 16.5 M A) 11.5 M B) 1.17 M C) 23.7 M D) 16.5 M

The freezing point of a solution made by dissolving 8.9 g of MgCl2 in 98 g H2O is -4.3°C. Kf for water is 1.86°C m-1. The van't Hoff i factor for this solution is ________.

A) 1.2 B) 2.3 C) 2.4 D) 2.0 E) 3.0 A) 1.2 B) 2.3 C) 2.4 D) 2.0 E) 3.0

A solution prepared by dissolving 4.00 g KCl in 36.0 g H2O is said to be:

A) 11.1% KCl by mass B) 0.100% KCl by mass C) 0.111% KCl by mass D) 10.0% KCl by mass E) 9.00% KCl by mass A) 11.1% KCl by mass B) 0.100% KCl by mass C) 0.111% KCl by mass D) 10.0% KCl by mass E) 9.00% KCl by mass

Two solutions contain the same amount of water as a solvent. One solution contains 0.5 mol glucose (C6H12O6) while the other one contains 0.2 mol of CaCl2 . If the freezing points of both solutions are the same, determine the van't Hoff i factor for CaCl2 solution.

A) 2.50 B) 3 C) 1.50 D) 2.75 E) 0.75 A) 2.50 B) 3 C) 1.50 D) 2.75 E) 0.75

Exam 13: Solutions and Their Physical Properties

The freezing point of pure benzene was measured as 5.49°C. With the same benzene and the same equipment, the freezing point of a solution containing 6.60 g of an unknown molecular compound in 140 g of benzene was found to be 2.35°C. The cryoscopic constant, Kf, for benzene is 5.12 deg-kg/mol. Calculate the mole weight of the unknown.

(Multiple Choice)

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Question 41

What is the mass/vol % ethanol in an ethanol-water solution with a density of 0.875 g/mL and containing 65.0% ethanol by volume? The density of pure ethanol is 0.789 g/mL.

(Multiple Choice)

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Question 42

Moles of solute per liter of solution is the definition of ________.

(Multiple Choice)

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Question 43

Which of the following is a correct statement about azeotropes?

(Multiple Choice)

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Question 44

Solutions are made that contain 0.10 moles of each of the following compounds in 100 g of H₂O. Choose the compound whose solution will have the highest freezing point.

(Multiple Choice)

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Question 45

An unknown compound is composed of 65.44% C, 29.07% O, and 5.49% H. A sample weighing 5.34 g, when dissolved in 60.00 g H₂O, lowers the freezing point to -0.600°C. What is the molecular formula of the compound? (Kf for water = 1.86°C/m; C = 12.0, O = 16.0, H = 1.0 g/mol).

(Multiple Choice)

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Question 46

The solubilities of ammonium bromide, NH₄Br, in water at 0°C, 20°C, and 80°C are as follows: $The solubilities of ammonium bromide, NH<sub>4</sub>Br, in water at 0°C, 20°C, and 80°C are as follows: Which of the following fractional crystallization schemes would produce the highest percent yield for the recrystallization of ammonium bromide?$ Which of the following fractional crystallization schemes would produce the highest percent yield for the recrystallization of ammonium bromide?

(Multiple Choice)

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Question 47

100 mL of LiNO₃, 0.241 M is mixed with 240 mL of 0.618 M Ca(NO₃)₂. What is the final concentration of NO₃^- in the solution?

(Multiple Choice)

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Question 48

Commercial perchloric acid is 70.0% by mass, HClO₄(aq), and has a density of 1.67 g/mL. Calculate the mole fraction of perchloric acid in the solution.

(Multiple Choice)

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Question 49

The van't Hoff factor is due to ions being attracted to each other enough that they don't react as individual molecules.

(True/False)

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Question 50

Arrange the following three water solutions (all 250 cm3 in volume) according to decreasing osmotic pressure at 273 K: 5 g of C₂H₅OH, 5 g C₆H₁₂O₆ ,and 5 g C₁₂H₂₂O₁₁.

(Multiple Choice)

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Question 51

Commercial perchloric acid is 70.0% by mass, HClO₄(aq), and has a density of 1.67 g/mL. Calculate the molarity of perchloric acid in the solution.

(Multiple Choice)

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Question 52

The vapor pressures of pure propyl alcohol and isopropyl alcohol are 21.0 mmHg and 45.2 mmHg, respectively, at 25°C. What is the composition of the vapor in equilibrium with a propyl alcohol - isopropyl alcohol solution in which the mole fraction of propyl alcohol is 0.250?

(Multiple Choice)

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Question 53

A crystal is placed into a solution and the solution seems to solidify while getting much warmer at the same time. The solution must have been:

(Multiple Choice)

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Question 54

The vapor pressures of pure propyl alcohol and isopropyl alcohol are 21.0 mmHg and 45.2 mmHg, respectively, at 25°C. Calculate the partial pressure of isopropyl alcohol above a solution in which the mole fraction of propyl alcohol is 0.250.

(Multiple Choice)

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Question 55

The freezing point of a solution made by dissolving 8.9 g of MgCl₂ in 98 g H₂O is -4.3°C. Kf for water is 1.86°C m-1. The van't Hoff i factor for this solution is ________.

(Multiple Choice)

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Question 56

A solution prepared by dissolving 4.00 g KCl in 36.0 g H₂O is said to be:

(Multiple Choice)

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Question 57

A solution component present in lesser quantity than the solvent is called ________.

(Multiple Choice)

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Question 58

The solubility of ammonium permanganate is 7.90 g/100 mL of water. 29.0 grams of ammonium permanganate are placed in a container and 220 mL of water is added. The liquid is allowed to stand in contact with the solid until equilibrium is achieved and then the liquid is poured off. What is the weight of solid left?

(Multiple Choice)

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Question 59

Two solutions contain the same amount of water as a solvent. One solution contains 0.5 mol glucose (C₆H₁₂O₆) while the other one contains 0.2 mol of CaCl₂ . If the freezing points of both solutions are the same, determine the van't Hoff i factor for CaCl₂ solution.

(Multiple Choice)

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Question 60

Showing 41 - 60 of 100

Exam 13: Solutions and Their Physical Properties

What is the mass/vol % ethanol in an ethanol-water solution with a density of 0.875 g/mL and containing 65.0% ethanol by volume? The density of pure ethanol is 0.789 g/mL.

Moles of solute per liter of solution is the definition of ________.

Which of the following is a correct statement about azeotropes?

Solutions are made that contain 0.10 moles of each of the following compounds in 100 g of H2O. Choose the compound whose solution will have the highest freezing point.

An unknown compound is composed of 65.44% C, 29.07% O, and 5.49% H. A sample weighing 5.34 g, when dissolved in 60.00 g H2O, lowers the freezing point to -0.600°C. What is the molecular formula of the compound? (Kf for water = 1.86°C/m; C = 12.0, O = 16.0, H = 1.0 g/mol).

The solubilities of ammonium bromide, NH4Br, in water at 0°C, 20°C, and 80°C are as follows: Which of the following fractional crystallization schemes would produce the highest percent yield for the recrystallization of ammonium bromide?

100 mL of LiNO3, 0.241 M is mixed with 240 mL of 0.618 M Ca(NO3)2. What is the final concentration of NO3- in the solution?

Commercial perchloric acid is 70.0% by mass, HClO4(aq), and has a density of 1.67 g/mL. Calculate the mole fraction of perchloric acid in the solution.

The van't Hoff factor is due to ions being attracted to each other enough that they don't react as individual molecules.

Arrange the following three water solutions (all 250 cm3 in volume) according to decreasing osmotic pressure at 273 K: 5 g of C2H5OH, 5 g C6H12O6 ,and 5 g C12H22O11.

Commercial perchloric acid is 70.0% by mass, HClO4(aq), and has a density of 1.67 g/mL. Calculate the molarity of perchloric acid in the solution.

The vapor pressures of pure propyl alcohol and isopropyl alcohol are 21.0 mmHg and 45.2 mmHg, respectively, at 25°C. What is the composition of the vapor in equilibrium with a propyl alcohol - isopropyl alcohol solution in which the mole fraction of propyl alcohol is 0.250?

A crystal is placed into a solution and the solution seems to solidify while getting much warmer at the same time. The solution must have been:

The vapor pressures of pure propyl alcohol and isopropyl alcohol are 21.0 mmHg and 45.2 mmHg, respectively, at 25°C. Calculate the partial pressure of isopropyl alcohol above a solution in which the mole fraction of propyl alcohol is 0.250.

The freezing point of a solution made by dissolving 8.9 g of MgCl2 in 98 g H2O is -4.3°C. Kf for water is 1.86°C m-1. The van't Hoff i factor for this solution is ________.

A solution prepared by dissolving 4.00 g KCl in 36.0 g H2O is said to be:

A solution component present in lesser quantity than the solvent is called ________.

Two solutions contain the same amount of water as a solvent. One solution contains 0.5 mol glucose (C6H12O6) while the other one contains 0.2 mol of CaCl2 . If the freezing points of both solutions are the same, determine the van't Hoff i factor for CaCl2 solution.

Matter - Its Properties and Measurement

Atoms and the Atomic Theory

Chemical Compounds

Chemical Reactions

Introduction to Reactions in Aqueous Solutions

Gases

Thermochemistry

Electrons in Atoms

The Periodic Table and Some Atomic Properties

Chemical Bonding I: Basic Concepts

Chemical Bonding II: Additional Aspects

Intermolecular Forces: Liquids and Solids

Chemical Kinetics

Principles of Chemical Equilibrium

Acids and Bases

Additional Aspects of Acid-Base Equilibria

Solubility and Complex-Ion Equilibria

Spontaneous Change: Entropy and Free Energy

Electrochemistry

Main Group Elements I: Groups 1, 2, 13, and 14

Main Group Elements II: Groups 18, 17, 16, 15, and Hydrogen

The Transition Elements

Complex Ions and Coordination Compounds

Nuclear Chemistry 1-41

Structures of Organic Compounds

Reactions of Organic Compounds

Chemistry of the Living State

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Solutions are made that contain 0.10 moles of each of the following compounds in 100 g of H₂O. Choose the compound whose solution will have the highest freezing point.

An unknown compound is composed of 65.44% C, 29.07% O, and 5.49% H. A sample weighing 5.34 g, when dissolved in 60.00 g H₂O, lowers the freezing point to -0.600°C. What is the molecular formula of the compound? (Kf for water = 1.86°C/m; C = 12.0, O = 16.0, H = 1.0 g/mol).

100 mL of LiNO₃, 0.241 M is mixed with 240 mL of 0.618 M Ca(NO₃)₂. What is the final concentration of NO₃^- in the solution?

Commercial perchloric acid is 70.0% by mass, HClO₄(aq), and has a density of 1.67 g/mL. Calculate the mole fraction of perchloric acid in the solution.

Arrange the following three water solutions (all 250 cm3 in volume) according to decreasing osmotic pressure at 273 K: 5 g of C₂H₅OH, 5 g C₆H₁₂O₆ ,and 5 g C₁₂H₂₂O₁₁.

Commercial perchloric acid is 70.0% by mass, HClO₄(aq), and has a density of 1.67 g/mL. Calculate the molarity of perchloric acid in the solution.

The freezing point of a solution made by dissolving 8.9 g of MgCl₂ in 98 g H₂O is -4.3°C. Kf for water is 1.86°C m-1. The van't Hoff i factor for this solution is ________.

A solution prepared by dissolving 4.00 g KCl in 36.0 g H₂O is said to be:

Two solutions contain the same amount of water as a solvent. One solution contains 0.5 mol glucose (C₆H₁₂O₆) while the other one contains 0.2 mol of CaCl₂ . If the freezing points of both solutions are the same, determine the van't Hoff i factor for CaCl₂ solution.