What is the molarity of a solution of 10 % by mass cadmium sulfate, CdSO4 (molar mass = 208.46 g/mol)by mass? The density of the solution is 1.10 g/mL.

A) 0.528 M B) 0.436 M C) 0.479 M D) 0.048 M E) 22.9 M A) 0.528 M B) 0.436 M C) 0.479 M D) 0.048 M E) 22.9 M

Which response lists all the following pairs that are miscible liquids. Pair #1: octane (C8H18)and water Pair #2: acetic acid (CH3COOH)and water Pair #3: octane (C8H18)and carbon tetrachloride (CCl4)

A) 1, 3 B) 1, 2 C) 3 D) 2 E) 2, 3 A) 1, 3 B) 1, 2 C) 3 D) 2 E) 2, 3

A solution of carbon tetrachloride in benzene, C6H6, at 20°C has a total vapor pressure of 78.50 mmHg. (Assume that this solution is ideal.)The vapor pressure of pure benzene at this temperature is 74.61 mmHg and its density is 0.87865 g/cm3; the vapor pressure of pure carbon tetrachloride is 91.32 mmHg and its density is 1.5940 g/cm3. What percentage of the volume of this solution is due to carbon tetrachloride? (Hint: assume that you have 1.000 L of solution.)

A) 75.2% B) 76.7% C) 14.3% D) 24.8% E) 23.3% A) 75.2% B) 76.7% C) 14.3% D) 24.8% E) 23.3%

A 15.00 % by mass solution of lactose (C12H22O11, 342.30 g/mol)in water has a density of 1.0602 g/mL at 20°C. What is the molarity of this solution?

A) 0.03097 M B) 0.4133 M C) 0.4646 M D) 1.590 M E) 3.097 M A) 0.03097 M B) 0.4133 M C) 0.4646 M D) 1.590 M E) 3.097 M

What is the mass percent CH3OH of a 0.256 m CH3OH(aq)solution?

A) 0.814 % B) 0.992 % C) 1.23 % D) 1.29 % E) 1.51 % A) 0.814 % B) 0.992 % C) 1.23 % D) 1.29 % E) 1.51 %

Exam 13: Physical Properties of Solutions

Some KCl is dissolved in water 25°C, where it completely dissociates. The vapor pressure of pure water at 25°C is 28.3 mmHg. Estimate the mass in grams of KCl needed per liter of pure water to reduce the vapor pressure of water at 25°C by 5%.

(Short Answer)

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Question 21

Explain the following, on the basis of osmosis or osmotic pressure: In trees and plants water is drawn from the soil up into the branches and leaves.

(Essay)

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Question 22

What is the molarity of a solution of 10 % by mass cadmium sulfate, CdSO₄ (molar mass = 208.46 g/mol)by mass? The density of the solution is 1.10 g/mL.

(Multiple Choice)

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Question 23

What mass of ethanol, C₂H₅OH a nonelectrolyte, must be added to 10.0 L of water to give a solution that freezes at -10.0°C? Assume the density of water is 1.0 g/mL. K_f of water is 1.86°C/m.

(Multiple Choice)

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Question 24

Some KCl is dissolved in water 25°C, where it completely dissociates. The vapor pressure of pure water at 25°C is 28.3 mmHg. On the graph below, sketch the vapor pressure above the salt solution as a function of the mole fraction of H₂O, assuming that Raoult's law is obeyed. Explain how you arrived at your graph. $Some KCl is dissolved in water 25°C, where it completely dissociates. The vapor pressure of pure water at 25°C is 28.3 mmHg. On the graph below, sketch the vapor pressure above the salt solution as a function of the mole fraction of H<sub>2</sub>O, assuming that Raoult's law is obeyed. Explain how you arrived at your graph.$

(Essay)

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Question 25

What is the molality of a 0.142 M Na₃PO₄(aq)solution that has a density of 1.015 g/mL?

(Short Answer)

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Question 26

What is the molarity of a solution that is 7.00 % by mass magnesium sulfate and has a density of 1.071 g/mL?

(Multiple Choice)

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Question 27

Which response lists all the following pairs that are miscible liquids. Pair #1: octane (C₈H₁₈)and water Pair #2: acetic acid (CH₃COOH)and water Pair #3: octane (C₈H₁₈)and carbon tetrachloride (CCl₄)

(Multiple Choice)

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Question 28

A solution is prepared by adding 6.24 g of benzene (C₆H₆, 78.11 g/mol)to 80.74 g of cyclohexane (C₆H₁₂, 84.16 g/mol). Calculate the mole fraction and molality of benzene in this solution.

(Short Answer)

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Question 29

In the course of research, a chemist isolates a new compound with an empirical formula C₃H₃O₂. Dissolving 2.51 g of the compound in 100. g of water produces a solution with a freezing point of -0.325°C. What is the molecular formula of the compound? (For water, K_f = 1.86°C/m.)

(Short Answer)

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Question 30

Which of the following liquids would make a good solvent for iodine, I₂?

(Multiple Choice)

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Question 31

Calculate the molality of a solution containing 14.3 g of NaCl in 42.2 g of water.

(Multiple Choice)

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Question 32

Explain the following, on the basis of osmosis or osmotic pressure: When sprinkled with sugar, a dish of sliced fruit will form its own juice.

(Essay)

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Question 33

A 100. mL sample of water is taken from the Great Salt Lake, and the water is allowed to evaporate. The salts that remain (mostly NaCl)have a mass of 31.9 g Calculate the original concentration of NaCl, in g per liter, in each water sample.

(Short Answer)

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Question 34

Calculate the approximate freezing point of a solution made from 21.0 g NaCl and 1.00 * 10² g of H₂O. [K_f of water is 1.86°C/m.]

(Multiple Choice)

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Question 35

A solution of carbon tetrachloride in benzene, C₆H₆, at 20°C has a total vapor pressure of 78.50 mmHg. (Assume that this solution is ideal.)The vapor pressure of pure benzene at this temperature is 74.61 mmHg and its density is 0.87865 g/cm³; the vapor pressure of pure carbon tetrachloride is 91.32 mmHg and its density is 1.5940 g/cm³. What percentage of the volume of this solution is due to carbon tetrachloride? (Hint: assume that you have 1.000 L of solution.)

(Multiple Choice)

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Question 36

What is the molarity of a solution that is 5.50 % by mass oxalic acid (C₂H₂O₄)and has a density of 1.0244 g/mL?

(Short Answer)

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Question 37

A 15.00 % by mass solution of lactose (C₁₂H₂₂O₁₁, 342.30 g/mol)in water has a density of 1.0602 g/mL at 20°C. What is the molarity of this solution?

(Multiple Choice)

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Question 38

What is the mass percent CH₃OH of a 0.256 m CH₃OH(aq)solution?

(Multiple Choice)

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Question 39

To interconvert the concentration units molality (m)and mass percent, you must also know the density of the solution.

(True/False)

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Question 40

Showing 21 - 40 of 109

Some KCl is dissolved in water 25°C, where it completely dissociates. The vapor pressure of pure water at 25°C is 28.3 mmHg. Estimate the mass in grams of KCl needed per liter of pure water to reduce the vapor pressure of water at 25°C by 5%.

Explain the following, on the basis of osmosis or osmotic pressure: In trees and plants water is drawn from the soil up into the branches and leaves.

What is the molarity of a solution of 10 % by mass cadmium sulfate, CdSO₄ (molar mass = 208.46 g/mol)by mass? The density of the solution is 1.10 g/mL.

What mass of ethanol, C₂H₅OH a nonelectrolyte, must be added to 10.0 L of water to give a solution that freezes at -10.0°C? Assume the density of water is 1.0 g/mL. K_f of water is 1.86°C/m.

What is the molality of a 0.142 M Na₃PO₄(aq)solution that has a density of 1.015 g/mL?

What is the molarity of a solution that is 7.00 % by mass magnesium sulfate and has a density of 1.071 g/mL?

Which response lists all the following pairs that are miscible liquids. Pair #1: octane (C₈H₁₈)and water Pair #2: acetic acid (CH₃COOH)and water Pair #3: octane (C₈H₁₈)and carbon tetrachloride (CCl₄)

A solution is prepared by adding 6.24 g of benzene (C₆H₆, 78.11 g/mol)to 80.74 g of cyclohexane (C₆H₁₂, 84.16 g/mol). Calculate the mole fraction and molality of benzene in this solution.

In the course of research, a chemist isolates a new compound with an empirical formula C₃H₃O₂. Dissolving 2.51 g of the compound in 100. g of water produces a solution with a freezing point of -0.325°C. What is the molecular formula of the compound? (For water, K_f = 1.86°C/m.)

Which of the following liquids would make a good solvent for iodine, I₂?

Calculate the molality of a solution containing 14.3 g of NaCl in 42.2 g of water.

Explain the following, on the basis of osmosis or osmotic pressure: When sprinkled with sugar, a dish of sliced fruit will form its own juice.

A 100. mL sample of water is taken from the Great Salt Lake, and the water is allowed to evaporate. The salts that remain (mostly NaCl)have a mass of 31.9 g Calculate the original concentration of NaCl, in g per liter, in each water sample.

Calculate the approximate freezing point of a solution made from 21.0 g NaCl and 1.00 * 10² g of H₂O. [K_f of water is 1.86°C/m.]

What is the molarity of a solution that is 5.50 % by mass oxalic acid (C₂H₂O₄)and has a density of 1.0244 g/mL?

A 15.00 % by mass solution of lactose (C₁₂H₂₂O₁₁, 342.30 g/mol)in water has a density of 1.0602 g/mL at 20°C. What is the molarity of this solution?

What is the mass percent CH₃OH of a 0.256 m CH₃OH(aq)solution?

To interconvert the concentration units molality (m)and mass percent, you must also know the density of the solution.

Introduction

Atoms, Molecules, and Ions

Stoichiometry

Reactions in Aqueous Solution

Gases

Energy Relationships in Chemical Reactions

The Electronic Structure of Atoms

The Periodic Table

Chemical Bonding I: the Covalent Bond

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Introduction to Organic Chemistry

Intermolecular Forces and Liquids and Solids

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Thermodynamics

Redox Reactions and Electrochemistry

The Chemistry of Coordination Compounds

Nuclear Chemistry

Organic Polymerssynthetic and Natural

Filters

Exam 13: Physical Properties of Solutions

Some KCl is dissolved in water 25°C, where it completely dissociates. The vapor pressure of pure water at 25°C is 28.3 mmHg. Estimate the mass in grams of KCl needed per liter of pure water to reduce the vapor pressure of water at 25°C by 5%.

Explain the following, on the basis of osmosis or osmotic pressure: In trees and plants water is drawn from the soil up into the branches and leaves.

What is the molarity of a solution of 10 % by mass cadmium sulfate, CdSO4 (molar mass = 208.46 g/mol)by mass? The density of the solution is 1.10 g/mL.

What mass of ethanol, C2H5OH a nonelectrolyte, must be added to 10.0 L of water to give a solution that freezes at -10.0°C? Assume the density of water is 1.0 g/mL. Kf of water is 1.86°C/m.

What is the molality of a 0.142 M Na3PO4(aq)solution that has a density of 1.015 g/mL?

What is the molarity of a solution that is 7.00 % by mass magnesium sulfate and has a density of 1.071 g/mL?

Which response lists all the following pairs that are miscible liquids. Pair #1: octane (C8H18)and water Pair #2: acetic acid (CH3COOH)and water Pair #3: octane (C8H18)and carbon tetrachloride (CCl4)

A solution is prepared by adding 6.24 g of benzene (C6H6, 78.11 g/mol)to 80.74 g of cyclohexane (C6H12, 84.16 g/mol). Calculate the mole fraction and molality of benzene in this solution.

In the course of research, a chemist isolates a new compound with an empirical formula C3H3O2. Dissolving 2.51 g of the compound in 100. g of water produces a solution with a freezing point of -0.325°C. What is the molecular formula of the compound? (For water, Kf = 1.86°C/m.)

Which of the following liquids would make a good solvent for iodine, I2?

Calculate the molality of a solution containing 14.3 g of NaCl in 42.2 g of water.

Explain the following, on the basis of osmosis or osmotic pressure: When sprinkled with sugar, a dish of sliced fruit will form its own juice.

A 100. mL sample of water is taken from the Great Salt Lake, and the water is allowed to evaporate. The salts that remain (mostly NaCl)have a mass of 31.9 g Calculate the original concentration of NaCl, in g per liter, in each water sample.

Calculate the approximate freezing point of a solution made from 21.0 g NaCl and 1.00 * 102 g of H2O. [Kf of water is 1.86°C/m.]

What is the molarity of a solution that is 5.50 % by mass oxalic acid (C2H2O4)and has a density of 1.0244 g/mL?

A 15.00 % by mass solution of lactose (C12H22O11, 342.30 g/mol)in water has a density of 1.0602 g/mL at 20°C. What is the molarity of this solution?

What is the mass percent CH3OH of a 0.256 m CH3OH(aq)solution?

To interconvert the concentration units molality (m)and mass percent, you must also know the density of the solution.

Introduction

Atoms, Molecules, and Ions

Stoichiometry

Reactions in Aqueous Solution

Gases

Energy Relationships in Chemical Reactions

The Electronic Structure of Atoms

The Periodic Table

Chemical Bonding I: the Covalent Bond

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Introduction to Organic Chemistry

Intermolecular Forces and Liquids and Solids

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Thermodynamics

Redox Reactions and Electrochemistry

The Chemistry of Coordination Compounds

Nuclear Chemistry

Organic Polymerssynthetic and Natural

Filters

What is the molarity of a solution of 10 % by mass cadmium sulfate, CdSO₄ (molar mass = 208.46 g/mol)by mass? The density of the solution is 1.10 g/mL.

What mass of ethanol, C₂H₅OH a nonelectrolyte, must be added to 10.0 L of water to give a solution that freezes at -10.0°C? Assume the density of water is 1.0 g/mL. K_f of water is 1.86°C/m.

What is the molality of a 0.142 M Na₃PO₄(aq)solution that has a density of 1.015 g/mL?

Which response lists all the following pairs that are miscible liquids. Pair #1: octane (C₈H₁₈)and water Pair #2: acetic acid (CH₃COOH)and water Pair #3: octane (C₈H₁₈)and carbon tetrachloride (CCl₄)

A solution is prepared by adding 6.24 g of benzene (C₆H₆, 78.11 g/mol)to 80.74 g of cyclohexane (C₆H₁₂, 84.16 g/mol). Calculate the mole fraction and molality of benzene in this solution.

In the course of research, a chemist isolates a new compound with an empirical formula C₃H₃O₂. Dissolving 2.51 g of the compound in 100. g of water produces a solution with a freezing point of -0.325°C. What is the molecular formula of the compound? (For water, K_f = 1.86°C/m.)

Which of the following liquids would make a good solvent for iodine, I₂?

Calculate the approximate freezing point of a solution made from 21.0 g NaCl and 1.00 * 10² g of H₂O. [K_f of water is 1.86°C/m.]

What is the molarity of a solution that is 5.50 % by mass oxalic acid (C₂H₂O₄)and has a density of 1.0244 g/mL?

A 15.00 % by mass solution of lactose (C₁₂H₂₂O₁₁, 342.30 g/mol)in water has a density of 1.0602 g/mL at 20°C. What is the molarity of this solution?

What is the mass percent CH₃OH of a 0.256 m CH₃OH(aq)solution?