List the following in order of solubility in hexane: 1) CH3CH2C(O)CH3, 2) C6H6, 3) CH3CH2CH2CO2H, 4) CH3CH2CH2CH2CO2H

A) 2 < 1 < 3 < 4 B) 1 < 3 < 4 < 2 C) 3 < 4 < 1 < 2 D) 4 < 3 < 1 < 2 E) 1 < 2 < 3 < 4 A) 2 < 1 < 3 < 4 B) 1 < 3 < 4 < 2 C) 3 < 4 < 1 < 2 D) 4 < 3 < 1 < 2 E) 1 < 2 < 3 < 4

What is the mole fraction of CaCl2 in an aqueous solution that is 0.569 m CaCl2 (solution density 1.05 g/ml)?

A) 0.01 M B) 0.01 C) 0.57 D) 0.10 E) 9.6 x 10-3 A) 0.01 M B) 0.01 C) 0.57 D) 0.10 E) 9.6 x 10-3

Exam 9: Properties of Solutions

The problem with hot water heaters in some parts of the country is that a solid forms inside of them, CaCO₃. Predict if the solvation process for CaCO₃ is endothermic or exothermic and if it is more soluble or less soluble at colder temperatures.

(Essay)

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Question 21

A major component of cell membranes is the phospholipid bilayer. Which of the following statements is(are) FALSE? I. The bilayer provides a barrier to charged ions II. Polar molecules such as glucose can pass through the membrane III. Protein molecules act as gates in the phospholipid bilayer allowing nutrients to enter into the cell IV. The bilayer consists of two nearly parallel rows with the hydrophobic tails facing out toward the solution and acting as a barrier to water soluble species.

(Multiple Choice)

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Question 22

Which of the following statements regarding solubility as a function of temperature are correct? I. Gas solubility favours high temperature and high pressure. II. Gas solubility favours low temperature and high pressure. III. Since the dissolution of solids into liquids is exothermic, solid solubility favours high temperature. IV. Endothermic dissolution of solids in liquids is favoured by lower temperature. V. Endothermic dissolution of solids in liquids is favoured by higher temperature.

(Multiple Choice)

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Question 23

Solutions used for intravenous injections must be isotonic, that is, exert an osmotic pressure of 6.9 atm. An isotonic saline solution uses sodium chloride as the solute to achieve isotonic conditions. Use this value for the osmotic pressure to estimate the % NaCl by mass in an isotonic saline solution at 37°C (assume the solution has a density of 1.0 g/mL).

(Multiple Choice)

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Question 24

A mixture that does NOT settle out upon standing is

(Multiple Choice)

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Question 25

Which part of soap is responsible for its ability to mix with oily dirt?

(Multiple Choice)

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Question 26

Calculate and explain solubilities in water.

(Essay)

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Question 27

Which of the following statements regarding alloys is(are) true? I. Alloys are homogeneous solid solutions II. Alloys display metallic properties III. The solute component in the alloy can replace the solvent component in the solid crystalline structure IV. The solute component can be incorporated in between solvent atoms in the crystal structure

(Multiple Choice)

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Question 28

Consider a warm (30°) 355 mL can of soda, under 2.5 atm CO₂pressure. What volume of CO₂ will be released from the soda in order to reach equilibrium after opening to the room where the pressure of CO₂ = 3.25 x 10^-4 atm and the total pressure is 758 mm Hg (K_H = 1.6 x 10^-2 M/atm)?

(Multiple Choice)

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Question 29

According to Henry's Law, the solubility of a gas in a liquid

(Multiple Choice)

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Question 30

Industrial grade concentrated HCl is known as muriatic acid and is 31.45% by mass HCl in water. What is the molality of this solution?

(Short Answer)

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Question 31

List the following in order of solubility in hexane: 1) CH₃CH₂C(O)CH₃, 2) C₆H₆, 3) CH₃CH₂CH₂CO₂H, 4) CH₃CH₂CH₂CH₂CO₂H

(Multiple Choice)

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Question 32

What is the mole fraction of CaCl₂ in an aqueous solution that is 0.569 m CaCl₂ (solution density 1.05 g/ml)?

(Multiple Choice)

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Question 33

To what minimum temperature would a radiator be protected if equal volumes of ethylene glycol (permanent antifreeze) (density 1.11 g/mL) and water were mixed? Assume that ethylene glycol does not dissociate and has a formula, C₂H₆O₂. (K_f = 1.85 ˚Cm^-1).

(Short Answer)

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Question 34

What is the concentration of chloride ions in a solution that is 0.569 m CaCl₂ (solution density 1.05 g/ml)?

(Multiple Choice)

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Question 35

Ben Franklin determined Avogadro's number within a factor of 5. He was able to do this by dropping 1 teaspoon of oil on a still pond and determined the area covered by the oil at about ¾ of an acre. You can simulate this by adding 1 drop of soap on the top of a greasy pan in the kitchen and watch the grease move to the sides. Sketch the interaction of the soap with the layer of water and sketch how the soap "dissolves" grease in water.

(Essay)

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Question 36

Understand the reasons for and calculate the magnitudes of colligative properties.

(Essay)

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Question 37

Pesticides have been found to accumulate and affect the growth of animals higher in food chain. Can you give some rational for this, including discussion of the solubility of pesticides in general?

(Essay)

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Question 38

When 0.64 g of adrenaline is dissolved in 36.0 g benzene (K_f = 5.12 °C), the freezing point is lowered by 0.50°C. Determine the molecular mass of adrenaline.

(Short Answer)

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Question 39

In the textbook it was discussed how the melting point is decreased and the boiling point is elevated for a solvent with a solute in it. What happens to the triple point of that solvent? Does the triple point

(Multiple Choice)

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Question 40

Showing 21 - 40 of 59

The problem with hot water heaters in some parts of the country is that a solid forms inside of them, CaCO₃. Predict if the solvation process for CaCO₃ is endothermic or exothermic and if it is more soluble or less soluble at colder temperatures.

A mixture that does NOT settle out upon standing is

Which part of soap is responsible for its ability to mix with oily dirt?

Calculate and explain solubilities in water.

Consider a warm (30°) 355 mL can of soda, under 2.5 atm CO₂pressure. What volume of CO₂ will be released from the soda in order to reach equilibrium after opening to the room where the pressure of CO₂ = 3.25 x 10^-4 atm and the total pressure is 758 mm Hg (K_H = 1.6 x 10^-2 M/atm)?

According to Henry's Law, the solubility of a gas in a liquid

Industrial grade concentrated HCl is known as muriatic acid and is 31.45% by mass HCl in water. What is the molality of this solution?

List the following in order of solubility in hexane: 1) CH₃CH₂C(O)CH₃, 2) C₆H₆, 3) CH₃CH₂CH₂CO₂H, 4) CH₃CH₂CH₂CH₂CO₂H

What is the mole fraction of CaCl₂ in an aqueous solution that is 0.569 m CaCl₂ (solution density 1.05 g/ml)?

To what minimum temperature would a radiator be protected if equal volumes of ethylene glycol (permanent antifreeze) (density 1.11 g/mL) and water were mixed? Assume that ethylene glycol does not dissociate and has a formula, C₂H₆O₂. (K_f = 1.85 ˚Cm^-1).

What is the concentration of chloride ions in a solution that is 0.569 m CaCl₂ (solution density 1.05 g/ml)?

Understand the reasons for and calculate the magnitudes of colligative properties.

Pesticides have been found to accumulate and affect the growth of animals higher in food chain. Can you give some rational for this, including discussion of the solubility of pesticides in general?

When 0.64 g of adrenaline is dissolved in 36.0 g benzene (K_f = 5.12 °C), the freezing point is lowered by 0.50°C. Determine the molecular mass of adrenaline.

In the textbook it was discussed how the melting point is decreased and the boiling point is elevated for a solvent with a solute in it. What happens to the triple point of that solvent? Does the triple point

Fundamental Concepts of Chemistry

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Energy and Its Conservation

Atoms and Light

Atomic Energies and Periodicity

Fundamentals of Chemical Bonding

Theories of Chemical Bonding

Effects of Intermolecular Forces

Organic Chemistrystructure

Organic Chemistryreactions

Spontaneity of Chemical Processes

Kinetics: Mechanisms and Rates of Reactions

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Applications of Aqueous Equilibria

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Exam 9: Properties of Solutions

The problem with hot water heaters in some parts of the country is that a solid forms inside of them, CaCO3. Predict if the solvation process for CaCO3 is endothermic or exothermic and if it is more soluble or less soluble at colder temperatures.

A mixture that does NOT settle out upon standing is

Which part of soap is responsible for its ability to mix with oily dirt?

Calculate and explain solubilities in water.

Consider a warm (30°) 355 mL can of soda, under 2.5 atm CO2 pressure. What volume of CO2 will be released from the soda in order to reach equilibrium after opening to the room where the pressure of CO2 = 3.25 x 10-4 atm and the total pressure is 758 mm Hg (KH = 1.6 x 10-2 M/atm)?

According to Henry's Law, the solubility of a gas in a liquid

Industrial grade concentrated HCl is known as muriatic acid and is 31.45% by mass HCl in water. What is the molality of this solution?

List the following in order of solubility in hexane: 1) CH3CH2C(O)CH3, 2) C6H6, 3) CH3CH2CH2CO2H, 4) CH3CH2CH2CH2CO2H

What is the mole fraction of CaCl2 in an aqueous solution that is 0.569 m CaCl2 (solution density 1.05 g/ml)?

To what minimum temperature would a radiator be protected if equal volumes of ethylene glycol (permanent antifreeze) (density 1.11 g/mL) and water were mixed? Assume that ethylene glycol does not dissociate and has a formula, C2H6O2. (Kf = 1.85 ˚Cm-1).

What is the concentration of chloride ions in a solution that is 0.569 m CaCl2 (solution density 1.05 g/ml)?

Understand the reasons for and calculate the magnitudes of colligative properties.

Pesticides have been found to accumulate and affect the growth of animals higher in food chain. Can you give some rational for this, including discussion of the solubility of pesticides in general?

When 0.64 g of adrenaline is dissolved in 36.0 g benzene (Kf = 5.12 °C), the freezing point is lowered by 0.50°C. Determine the molecular mass of adrenaline.

In the textbook it was discussed how the melting point is decreased and the boiling point is elevated for a solvent with a solute in it. What happens to the triple point of that solvent? Does the triple point

Fundamental Concepts of Chemistry

The Behaviour of Gases

Energy and Its Conservation

Atoms and Light

Atomic Energies and Periodicity

Fundamentals of Chemical Bonding

Theories of Chemical Bonding

Effects of Intermolecular Forces

Organic Chemistrystructure

Organic Chemistryreactions

Spontaneity of Chemical Processes

Kinetics: Mechanisms and Rates of Reactions

Principles of Chemical Equilibrium

Aqueous Acidbase Equilibria

Applications of Aqueous Equilibria

Electron Transfer Reactions

Macromolecules

The Transition Metals

The Main Group Elements

Nuclear Chemistry and Radiochemistry

Filters

The problem with hot water heaters in some parts of the country is that a solid forms inside of them, CaCO₃. Predict if the solvation process for CaCO₃ is endothermic or exothermic and if it is more soluble or less soluble at colder temperatures.

Consider a warm (30°) 355 mL can of soda, under 2.5 atm CO₂pressure. What volume of CO₂ will be released from the soda in order to reach equilibrium after opening to the room where the pressure of CO₂ = 3.25 x 10^-4 atm and the total pressure is 758 mm Hg (K_H = 1.6 x 10^-2 M/atm)?

List the following in order of solubility in hexane: 1) CH₃CH₂C(O)CH₃, 2) C₆H₆, 3) CH₃CH₂CH₂CO₂H, 4) CH₃CH₂CH₂CH₂CO₂H

What is the mole fraction of CaCl₂ in an aqueous solution that is 0.569 m CaCl₂ (solution density 1.05 g/ml)?

To what minimum temperature would a radiator be protected if equal volumes of ethylene glycol (permanent antifreeze) (density 1.11 g/mL) and water were mixed? Assume that ethylene glycol does not dissociate and has a formula, C₂H₆O₂. (K_f = 1.85 ˚Cm^-1).

What is the concentration of chloride ions in a solution that is 0.569 m CaCl₂ (solution density 1.05 g/ml)?

When 0.64 g of adrenaline is dissolved in 36.0 g benzene (K_f = 5.12 °C), the freezing point is lowered by 0.50°C. Determine the molecular mass of adrenaline.