Question 1

What is the percentage by mass of glycerol (C3H5(OH)3) in a 1.5 m solution?

Accepted Answer

Question 2

For each of the following solutions, would you expect it with respect to Raoult's law) to be relatively ideal, to show a positive deviation, or to show a negative deviation?
-hexane (C6H14) and octane (C8H18)

Accepted Answer

A)  positive deviation 
B)  negative deviation 
C)  relatively ideal 
A)  positive deviation 
B)  negative deviation 
C)  relatively ideal

Question 3

A salt solution sits in an open beaker. Assuming constant temperature and pressure, the vapor pressure of the solution

Accepted Answer

A)  stays the same over time. 
B)  We need to know which salt is in the solution to answer this. 
C)  increases over time. 
D)  We need to know the temperature and pressure to answer this. 
E)  decreases over time. 
A)  stays the same over time. 
B)  We need to know which salt is in the solution to answer this. 
C)  increases over time. 
D)  We need to know the temperature and pressure to answer this. 
E)  decreases over time.

Question 4

The solubility of the salt MxAy is 1.0 F1F1F1S1F1F1F10 10-2 mol/L at 25°C. The osmotic pressure exhibited by a solution saturated with MxAy at 25°C is 1.22 atm. Determine the values of x and y by assuming ideal behavior.

Accepted Answer

A)  x = 1, y =3 
B)  x = 2, y = 5 
C)  x = 1, y = 1 
D)  x = 2, y = 3 
E)  none of these 
A)  x = 1, y =3 
B)  x = 2, y = 5 
C)  x = 1, y = 1 
D)  x = 2, y = 3 
E)  none of these

Question 5

You use 2.0 g of solid MX to prepare a saturated solution in 250. g of water. You find the freezing point to be -0.028°C. Calculate Ksp for the solid.

Accepted Answer

A)  2.2 F1F1F1S1F1F1F10 10-4 
B)  5.6 F1F1F1S1F1F1F10 10-5 
C)  1.4 F1F1F1S1F1F1F10 10-5 
D)  3.5 F1F1F1S1F1F1F10 10-6 
E)  none of these 
A)  2.2 F1F1F1S1F1F1F10 10-4 
B)  5.6 F1F1F1S1F1F1F10 10-5 
C)  1.4 F1F1F1S1F1F1F10 10-5 
D)  3.5 F1F1F1S1F1F1F10 10-6 
E)  none of these

Question 6

When 0.800 g of NH4NO3 was added to 150.0 g of water in a styrofoam cup, the temperature dropped by 0.413°C. The heat capacity of H2O is 4.18 J/g°C. Assume the specific heat of the solution equals that of pure H2O and that the calorimeter neither absorbs nor leaks heat. What is the molar heat of solution of solid NH4NO3?

Accepted Answer

A)  +260. J/mol 
B)  -2.60 kJ/mol 
C)  +2.60 kJ/mol 
D)  +26.0 kJ/mol 
E)  none of these 
A)  +260. J/mol 
B)  -2.60 kJ/mol 
C)  +2.60 kJ/mol 
D)  +26.0 kJ/mol 
E)  none of these

Question 7

Thyroxine, an important hormone that controls the rate of metabolism in the body, can be isolated from the thyroid gland. If 0.455 g of thyroxine is dissolved in 10.0 g of benzene, the freezing point of the solution is 5.144°C. Pure benzene freezes at 5.444°C and has a value for the molal freezing-point-depression constant of Kf of 5.12°C/m. What is the molar mass of thyroxine?

Accepted Answer

A)  2330 g/mol 
B)  285 g/mol 
C)  777 g/mol 
D)  3760 g/mol 
E)  777,000 g/mol 
A)  2330 g/mol 
B)  285 g/mol 
C)  777 g/mol 
D)  3760 g/mol 
E)  777,000 g/mol

Question 8

A solution is composed of two liquids, A and B. For every 2.66 mol of A, there are 6.86 mol of B. What is the mole fraction of liquid A in the solution?

Accepted Answer

A)  0.721 
B)  0.612 
C)  0.388 
D)  0.279 
E)  0.633 
A)  0.721 
B)  0.612 
C)  0.388 
D)  0.279 
E)  0.633

Question 9

Which of the following chemical or physical changes is an endothermic process?

Accepted Answer

A)  the mixing of sulfuric acid and water 
B)  the freezing of water 
C)  the evaporation of water 
D)  the combustion of gasoline 
E)  none of these 
A)  the mixing of sulfuric acid and water 
B)  the freezing of water 
C)  the evaporation of water 
D)  the combustion of gasoline 
E)  none of these

Question 10

Solid KF has a lattice energy of -804 kJ/mol and a heat of solution (in water) of -15 kJ/mol. RbF has a lattice energy of -768 kJ/mol and a heat of solution (in water) of -24 kJ/mol. Which salt forms stronger attractions with water?

Accepted Answer

A)  They form equally strong attractions with water, because they both have negative heats of mixing. 
B)  KF, because it has a more exothermic lattice energy 
C)  RbF, because it has a more negative heat of hydration 
D)  KF, because it has a more negative heat of hydration 
E)  RbF, because it has a less exothermic lattice energy 
A)  They form equally strong attractions with water, because they both have negative heats of mixing. 
B)  KF, because it has a more exothermic lattice energy 
C)  RbF, because it has a more negative heat of hydration 
D)  KF, because it has a more negative heat of hydration 
E)  RbF, because it has a less exothermic lattice energy

Question 11

For each of the following solutions, would you expect it with respect to Raoult's law) to be relatively ideal, to show a positive deviation, or to show a negative deviation?
-acetone (C3H6O) and water

Accepted Answer

A)  relatively ideal 
B)  positive deviation 
C)  negative deviation 
A)  relatively ideal 
B)  positive deviation 
C)  negative deviation

Question 12

A solution is prepared from 31.4 g of a nonvolatile, nondissociating solute and 85.0 g of water. The vapor pressure of the solution at 60°C is 142 torr. The vapor pressure of water at 60°C is 150. torr. What is the molar mass of the solute?

Accepted Answer

The answer of A solution is prepared from 31.4 g...

Question 13

A 0.2 molar solution of a solute X, in benzene, displays an osmotic pressure given by the formula F1F1F1S1F1F1F10 = (0.1)RT. Which of the following is most likely to be the case?

Accepted Answer

A)  X exists in benzene as X2. 
B)  X exists in benzene as X. 
C)  X exists in benzene dissociated into two particles. 
D)  This solution strongly deviates from ideal behavior. 
E)  None of these explanations is plausible. 
A)  X exists in benzene as X2. 
B)  X exists in benzene as X. 
C)  X exists in benzene dissociated into two particles. 
D)  This solution strongly deviates from ideal behavior. 
E)  None of these explanations is plausible.

Question 14

Calculate the mole fraction of KCl in a solution prepared by dissolving 2.50 g of KCl in 500.0 g of H2O.

Accepted Answer

1.21*10<su

Question 15

The molar mass of a solid as determined by freezing-point depression is 10% higher than the true molar mass. Which of the following experimental errors could not account for this discrepancy?

Accepted Answer

A)  Before the solution was prepared, the container was rinsed with solvent and not dried. 
B)  Some solid was left on the weighing paper. 
C)  Not all the solid was dissolved. 
D)  The solid dissociated slightly into two particles when it dissolved. 
E)  More than the recorded amount of solvent was pipetted into the solution. 
A)  Before the solution was prepared, the container was rinsed with solvent and not dried. 
B)  Some solid was left on the weighing paper. 
C)  Not all the solid was dissolved. 
D)  The solid dissociated slightly into two particles when it dissolved. 
E)  More than the recorded amount of solvent was pipetted into the solution.

Question 16

An aqueous solution is 1.00% NaCl by mass. Its density is 1.071 g/mL at 25°C. The observed osmotic pressure of this solution is 7.83 atm at 25°C. 
A) What fraction of the moles of NaCl in this solution are ion pairs?
B) Calculate the freezing point that would be observed for this solution; Kf for H2O = 1.86°C kg/mol.

Accepted Answer

Question 17

A mixture of solid NaCl and CaCl2 contains 10.0 g of NaCl, and an unknown amount of CaCl2. When the entire mixture is dissolved in 1.00 kg of water, the boiling point changes by 0.25 F1F1F1S1F1F1F10C. What mass of CaCl2 was in the original mixture? Kb for water is 0.512 K. kg . mol-1.

Accepted Answer

A)  5.4 g 
B)  8.1 g 
C)  35.2 g 
D)  Not enough data to answer the question 
E)  None of the above 
A)  5.4 g 
B)  8.1 g 
C)  35.2 g 
D)  Not enough data to answer the question 
E)  None of the above

Question 18

Determine the molarity of a solution containing 2.00 g of sodium hydroxide in 250.0 mL of solution.

Accepted Answer

The answer of Determine the molarity of a solution containing...

Question 19

A solution is made of 173.0 g of methanol (CH3OH) in 169.0 g of water. What is the mole fraction of methanol?

Accepted Answer

A)  0.0158 
B)  0.506 
C)  0.635 
D)  0.594 
E)  0.365 
A)  0.0158 
B)  0.506 
C)  0.635 
D)  0.594 
E)  0.365

What is the percentage by mass of glycerol (C₃H₅(OH)₃) in a 1.5 m solution?

For each of the following solutions, would you expect it with respect to Raoult's law) to be relatively ideal, to show a positive deviation, or to show a negative deviation? -hexane (C₆H₁₄) and octane (C₈H₁₈)

A salt solution sits in an open beaker. Assuming constant temperature and pressure, the vapor pressure of the solution

The solubility of the salt M_xA_y is 1.0  10^-² mol/L at 25°C. The osmotic pressure exhibited by a solution saturated with M_xA_y at 25°C is 1.22 atm. Determine the values of x and y by assuming ideal behavior.

You use 2.0 g of solid MX to prepare a saturated solution in 250. g of water. You find the freezing point to be -0.028°C. Calculate K_sp for the solid.

A solution is composed of two liquids, A and B. For every 2.66 mol of A, there are 6.86 mol of B. What is the mole fraction of liquid A in the solution?

Which of the following chemical or physical changes is an endothermic process?

Solid KF has a lattice energy of -804 kJ/mol and a heat of solution (in water) of -15 kJ/mol. RbF has a lattice energy of -768 kJ/mol and a heat of solution (in water) of -24 kJ/mol. Which salt forms stronger attractions with water?

For each of the following solutions, would you expect it with respect to Raoult's law) to be relatively ideal, to show a positive deviation, or to show a negative deviation? -acetone (C₃H₆O) and water

A solution is prepared from 31.4 g of a nonvolatile, nondissociating solute and 85.0 g of water. The vapor pressure of the solution at 60°C is 142 torr. The vapor pressure of water at 60°C is 150. torr. What is the molar mass of the solute?

A 0.2 molar solution of a solute X, in benzene, displays an osmotic pressure given by the formula  = (0.1)RT. Which of the following is most likely to be the case?

Calculate the mole fraction of KCl in a solution prepared by dissolving 2.50 g of KCl in 500.0 g of H₂O.

The molar mass of a solid as determined by freezing-point depression is 10% higher than the true molar mass. Which of the following experimental errors could not account for this discrepancy?

A mixture of solid NaCl and CaCl₂ contains 10.0 g of NaCl, and an unknown amount of CaCl₂. When the entire mixture is dissolved in 1.00 kg of water, the boiling point changes by 0.25 C. What mass of CaCl₂ was in the original mixture? K_b for water is 0.512 K^.kg ^.mol^-1.

Determine the molarity of a solution containing 2.00 g of sodium hydroxide in 250.0 mL of solution.

A solution is made of 173.0 g of methanol (CH₃OH) in 169.0 g of water. What is the mole fraction of methanol?

Atoms, Molecules, and Ions

Stoichiometry

Chemical Reactions and Solutions Stoichiometry

Gases

Chemical Equilibrium

Acids and Bases

Applications of Aqueous Equilibria

Energy, Enthalpy, and Thermochemistry

Spontaneity, Entropy, and Free Energy

Electrochemistry

Quantum Mechanics and Atomic Theory

Bonding: General Concepts

Covalent Bonding: Orbitals

Chemical Kinetics

Liquids and Solids

The Representative Elements

Transition Metals and Coordination Chemistry

The Nucleus: a Chemists View

Organic and Biochemical Molecules

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Exam 17: Properties of Solutions

What is the percentage by mass of glycerol (C3H5(OH)3) in a 1.5 m solution?

For each of the following solutions, would you expect it with respect to Raoult's law) to be relatively ideal, to show a positive deviation, or to show a negative deviation? -hexane (C6H14) and octane (C8H18)

A salt solution sits in an open beaker. Assuming constant temperature and pressure, the vapor pressure of the solution

The solubility of the salt MxAy is 1.0  10-2 mol/L at 25°C. The osmotic pressure exhibited by a solution saturated with MxAy at 25°C is 1.22 atm. Determine the values of x and y by assuming ideal behavior.

You use 2.0 g of solid MX to prepare a saturated solution in 250. g of water. You find the freezing point to be -0.028°C. Calculate Ksp for the solid.

A solution is composed of two liquids, A and B. For every 2.66 mol of A, there are 6.86 mol of B. What is the mole fraction of liquid A in the solution?

Which of the following chemical or physical changes is an endothermic process?

Solid KF has a lattice energy of -804 kJ/mol and a heat of solution (in water) of -15 kJ/mol. RbF has a lattice energy of -768 kJ/mol and a heat of solution (in water) of -24 kJ/mol. Which salt forms stronger attractions with water?

For each of the following solutions, would you expect it with respect to Raoult's law) to be relatively ideal, to show a positive deviation, or to show a negative deviation? -acetone (C3H6O) and water

A solution is prepared from 31.4 g of a nonvolatile, nondissociating solute and 85.0 g of water. The vapor pressure of the solution at 60°C is 142 torr. The vapor pressure of water at 60°C is 150. torr. What is the molar mass of the solute?

A 0.2 molar solution of a solute X, in benzene, displays an osmotic pressure given by the formula  = (0.1)RT. Which of the following is most likely to be the case?

Calculate the mole fraction of KCl in a solution prepared by dissolving 2.50 g of KCl in 500.0 g of H2O.

The molar mass of a solid as determined by freezing-point depression is 10% higher than the true molar mass. Which of the following experimental errors could not account for this discrepancy?

A mixture of solid NaCl and CaCl2 contains 10.0 g of NaCl, and an unknown amount of CaCl2. When the entire mixture is dissolved in 1.00 kg of water, the boiling point changes by 0.25 C. What mass of CaCl2 was in the original mixture? Kb for water is 0.512 K. kg . mol-1.

Determine the molarity of a solution containing 2.00 g of sodium hydroxide in 250.0 mL of solution.

A solution is made of 173.0 g of methanol (CH3OH) in 169.0 g of water. What is the mole fraction of methanol?

Atoms, Molecules, and Ions

Stoichiometry

Chemical Reactions and Solutions Stoichiometry

Gases

Chemical Equilibrium

Acids and Bases

Applications of Aqueous Equilibria

Energy, Enthalpy, and Thermochemistry

Spontaneity, Entropy, and Free Energy

Electrochemistry

Quantum Mechanics and Atomic Theory

Bonding: General Concepts

Covalent Bonding: Orbitals

Chemical Kinetics

Liquids and Solids

The Representative Elements

Transition Metals and Coordination Chemistry

The Nucleus: a Chemists View

Organic and Biochemical Molecules

Filters

What is the percentage by mass of glycerol (C₃H₅(OH)₃) in a 1.5 m solution?

For each of the following solutions, would you expect it with respect to Raoult's law) to be relatively ideal, to show a positive deviation, or to show a negative deviation? -hexane (C₆H₁₄) and octane (C₈H₁₈)

The solubility of the salt M_xA_y is 1.0  10^-² mol/L at 25°C. The osmotic pressure exhibited by a solution saturated with M_xA_y at 25°C is 1.22 atm. Determine the values of x and y by assuming ideal behavior.

You use 2.0 g of solid MX to prepare a saturated solution in 250. g of water. You find the freezing point to be -0.028°C. Calculate K_sp for the solid.

For each of the following solutions, would you expect it with respect to Raoult's law) to be relatively ideal, to show a positive deviation, or to show a negative deviation? -acetone (C₃H₆O) and water

Calculate the mole fraction of KCl in a solution prepared by dissolving 2.50 g of KCl in 500.0 g of H₂O.

A mixture of solid NaCl and CaCl₂ contains 10.0 g of NaCl, and an unknown amount of CaCl₂. When the entire mixture is dissolved in 1.00 kg of water, the boiling point changes by 0.25 C. What mass of CaCl₂ was in the original mixture? K_b for water is 0.512 K^.kg ^.mol^-1.

A solution is made of 173.0 g of methanol (CH₃OH) in 169.0 g of water. What is the mole fraction of methanol?