Question 1

How many grams of KBr are required to make 650.mL of a 0.115 M KBr solution?

Accepted Answer

A) 0)628 g 
B) 5)65 g 
C) 8)90 g 
D) 74.8 g 
A) 0)628 g 
B) 5)65 g 
C) 8)90 g 
D) 74.8 g

Question 2

In general,as the temperature increases,the solubility of gases in water ________ and the solubility of most solids in water ________.

Accepted Answer

A) decreases,decreases 
B) decreases,increases 
C) increases,decreases 
D) increases,increases 
A) decreases,decreases 
B) decreases,increases 
C) increases,decreases 
D) increases,increases

Question 3

If one mole of each is dissolved in 1.00 L of water,which will lower the vapor pressure the most?

Accepted Answer

A) C12H22O11 
B) NaNO3 
C) C3H7OH 
D) MgCl2 
A) C12H22O11 
B) NaNO3 
C) C3H7OH 
D) MgCl2

Question 4

The boiling point of a solution containing a nonvolatile solute will be ________ than the boiling point of the pure solvent,whereas the boiling point of a solution of two volatile liquids will be ________ than the boiling point of the more volatile liquid and ________ than the boiling point of the less volatile liquid.

Accepted Answer

The answer of The boiling point of a solution containing...

Question 5

A KCl solution is prepared by dissolving 40.0 g KCl in 250.0 g of water at 25°C.What is the vapor pressure of the solution if the vapor pressure of water at 25°C is 23.76 mm Hg?

Accepted Answer

A) 20.5 mm Hg 
B) 22.1 mm Hg 
C) 22.9 mm Hg 
D) 25.5 mm Hg 
A) 20.5 mm Hg 
B) 22.1 mm Hg 
C) 22.9 mm Hg 
D) 25.5 mm Hg

Question 6

An aqueous solution has a normal boiling point of 10 3.0°C.What is the freezing point of this solution? For water Kb = 0.51°C /m and Kf = 1.86°C /m.

Accepted Answer

A) -0.82°C 
B) - 3.0°C 
C) -3.6°C 
D) - 11°C 
A) -0.82°C 
B) - 3.0°C 
C) -3.6°C 
D) - 11°C

Question 7

Arrows in the energy diagram below represent enthalpy changes occurring in the exothermic formation of a solution:
ΔHS1U1B1solnS1U1B0 = enthalpy of solution
ΔHsolute-solute = enthalpy change involving solute-solute interactions
ΔHsolute-solvent = enthalpy change involving solute-solvent interactions
ΔHsolvent-solvent = enthalpy change involving solvent-solvent interactions  
-Which arrow represents ΔHsoln?

Accepted Answer

A) arrow (a) 
B) arrow (b) 
C) arrow (c) 
D) arrow (d) 
A) arrow (a) 
B) arrow (b) 
C) arrow (c) 
D) arrow (d)

Question 8

Most gases become less soluble in water as the temperature increases.What can be concluded about the signs of ΔHsoln and ΔSsoln in this case?

Accepted Answer

A) ΔHsoln is negative and ΔSsoln is negative. 
B) ΔHsoln is negative and ΔSsoln is positive. 
C) ΔHsoln is positive and ΔSsoln is negative. 
D) ΔHsoln is positive and ΔSsoln is positive. 
A) ΔHsoln is negative and ΔSsoln is negative. 
B) ΔHsoln is negative and ΔSsoln is positive. 
C) ΔHsoln is positive and ΔSsoln is negative. 
D) ΔHsoln is positive and ΔSsoln is positive.

Question 9

When a particular solid begins to dissolve in water,the temperature rises dramatically.For the dissolving of this solid in pure water

Accepted Answer

A) ΔHsoln is always negative and ΔSsoln may be negative or positive. 
B) ΔHsoln is always negative and ΔSsoln is always positive. 
C) ΔHsoln is always positive and ΔSsoln may be negative or positive. 
D) ΔHsoln is always positive and ΔSsoln is always positive. 
A) ΔHsoln is always negative and ΔSsoln may be negative or positive. 
B) ΔHsoln is always negative and ΔSsoln is always positive. 
C) ΔHsoln is always positive and ΔSsoln may be negative or positive. 
D) ΔHsoln is always positive and ΔSsoln is always positive.

Question 10

-Which drawing above represents the system with the second highest entropy?

Accepted Answer

A) drawing (a) 
B) drawing (b) 
C) drawing (c) 
D) drawing (d) 
A) drawing (a) 
B) drawing (b) 
C) drawing (c) 
D) drawing (d)

Question 11

The change in the Gibbs free energy for dissolving more solute in a supersaturated solution is

Accepted Answer

A) negative. 
B) zero. 
C) positive. 
D) positive at low temperatures and negative at high temperatures. 
A) negative. 
B) zero. 
C) positive. 
D) positive at low temperatures and negative at high temperatures.

Question 12

Arrows in the energy diagram below represent enthalpy changes occurring in the exothermic formation of a solution:
ΔHS1U1B1solnS1U1B0 = enthalpy of solution
ΔHsolute-solute = enthalpy change involving solute-solute interactions
ΔHsolute-solvent = enthalpy change involving solute-solvent interactions
ΔHsolvent-solvent = enthalpy change involving solvent-solvent interactions  
-Which arrow represents ΔHsolute-solvent?

Accepted Answer

A) arrow (a) 
B) arrow (b) 
C) arrow (c) 
D) arrow (d) 
A) arrow (a) 
B) arrow (b) 
C) arrow (c) 
D) arrow (d)

Question 13

In the process of dissolving ionic compounds,the cations and anions are separated from the crystal lattice and surrounded by an ordered shell of solvent molecules.If the solvent is water,the dissolved ions are said to be

Accepted Answer

A) halogenated. 
B) homogenized. 
C) hybridized. 
D) hydrated. 
A) halogenated. 
B) homogenized. 
C) hybridized. 
D) hydrated.

Question 14

A solution of LiCl in water is 18.0 wt% LiCl.What is the mole fraction of LiCl?

Accepted Answer

A) 0)0853 
B) 0)0933 
C) 0)425 
D) 4)56 
A) 0)0853 
B) 0)0933 
C) 0)425 
D) 4)56

Question 15

Which concentration becomes smaller as the temperature is increased from 20°C to 80°C?

Accepted Answer

A) mass % 
B) molality 
C) molarity 
D) mole fraction 
A) mass % 
B) molality 
C) molarity 
D) mole fraction

Question 16

What is the molality of a glucose solution prepared by dissolving 18.0 g of glucose,C6H12O6,in 125.9 g of water?

Accepted Answer

A) 7)94 × 10- 4 m 
B) 0)143 m 
C) 0)695 m 
D) 0)794 m 
A) 7)94 × 10- 4 m 
B) 0)143 m 
C) 0)695 m 
D) 0)794 m

Question 17

What are the major solute-solvent interactions created when HOCH2CH2OH dissolves in water?

Accepted Answer

A) dipole-dipole 
B) dispersion 
C) hydrogen bonding 
D) ion-dipole 
A) dipole-dipole 
B) dispersion 
C) hydrogen bonding 
D) ion-dipole

Question 18

The normal boiling point of pure benzene is found to be 80.10°C.What is the approximate molecular weight of a nonionizing substance if a solution of 3.55 g of the substance dissolved in 100.g of benzene has a normal boiling point of 80.19°C? Kb = 5.12°C/m for benzene,C6H6.

Accepted Answer

A) 20 amu 
B) 500 amu 
C) 2000 amu 
D) 20,000 amu 
A) 20 amu 
B) 500 amu 
C) 2000 amu 
D) 20,000 amu

Question 19

To make a 2.0 M solution,one could take 2.00 moles of solute and add

Accepted Answer

A) 1)00 L of solvent. 
B) 1)00 kg of solvent. 
C) enough solvent to make 1.00 L of solution. 
D) enough solvent to make 1.00 kg of solution. 
A) 1)00 L of solvent. 
B) 1)00 kg of solvent. 
C) enough solvent to make 1.00 L of solution. 
D) enough solvent to make 1.00 kg of solution.

Question 20

The osmotic pressure of a 100-mL solution containing 1.0 g of sucrose,C12H22O11 will be ________ (equal to,greater than,less than)the osmotic pressure of a 100-mL solution containing 1.0 g of fructose,C6H12O6.

Accepted Answer

Exam 11: Solutions and Their Properties

How many grams of KBr are required to make 650.mL of a 0.115 M KBr solution?

In general,as the temperature increases,the solubility of gases in water ________ and the solubility of most solids in water ________.

If one mole of each is dissolved in 1.00 L of water,which will lower the vapor pressure the most?

A KCl solution is prepared by dissolving 40.0 g KCl in 250.0 g of water at 25°C.What is the vapor pressure of the solution if the vapor pressure of water at 25°C is 23.76 mm Hg?

An aqueous solution has a normal boiling point of 10 3.0°C.What is the freezing point of this solution? For water Kb = 0.51°C /m and Kf = 1.86°C /m.

Most gases become less soluble in water as the temperature increases.What can be concluded about the signs of ΔHsoln and ΔSsoln in this case?

When a particular solid begins to dissolve in water,the temperature rises dramatically.For the dissolving of this solid in pure water

-Which drawing above represents the system with the second highest entropy?

The change in the Gibbs free energy for dissolving more solute in a supersaturated solution is

In the process of dissolving ionic compounds,the cations and anions are separated from the crystal lattice and surrounded by an ordered shell of solvent molecules.If the solvent is water,the dissolved ions are said to be

A solution of LiCl in water is 18.0 wt% LiCl.What is the mole fraction of LiCl?

Which concentration becomes smaller as the temperature is increased from 20°C to 80°C?

What is the molality of a glucose solution prepared by dissolving 18.0 g of glucose,C6H12O6,in 125.9 g of water?

What are the major solute-solvent interactions created when HOCH2CH2OH dissolves in water?

The normal boiling point of pure benzene is found to be 80.10°C.What is the approximate molecular weight of a nonionizing substance if a solution of 3.55 g of the substance dissolved in 100.g of benzene has a normal boiling point of 80.19°C? Kb = 5.12°C/m for benzene,C6H6.

To make a 2.0 M solution,one could take 2.00 moles of solute and add

The osmotic pressure of a 100-mL solution containing 1.0 g of sucrose,C12H22O11 will be ________ (equal to,greater than,less than)the osmotic pressure of a 100-mL solution containing 1.0 g of fructose,C6H12O6.

Chemistry: Matter and Measurement

Atoms, molecules, and Ions

Formulas, equations, and Moles

Reactions in Aqueous Solutions

Periodicity and the Atomic Structure of Atoms

Ionic Bonds and Some Main-Group Chemistry

Covalent Bonds and Molecular Structure

Thermochemistry: Chemical Energy

Gases: Their Properties and Behavior

Liquids,solids,and Phase Changes

Chemical Kinetics

Chemical Equilibrium

Aqueous Equilibria: Acids and Bases

Applications of Aqueous Equilibria

Thermodynamics: Entropy, free Energy, and Equilibrium

Electrochemistry

Hydrogen, oxygen, and Water

The Main-Group Elements

Transition Elements and Coordination Chemistry

Metals and Solid-State Materials

Nuclear Chemistry

Organic and Biological Chemistry

Filters

In general,as the temperature increases,the solubility of gases in water and the solubility of most solids in water .

An aqueous solution has a normal boiling point of 10 3.0°C.What is the freezing point of this solution? For water K_b= 0.51°C /m and K_f= 1.86°C /m.

Most gases become less soluble in water as the temperature increases.What can be concluded about the signs of ΔH_soln and ΔS_soln in this case?

What is the molality of a glucose solution prepared by dissolving 18.0 g of glucose,C₆H₁₂O₆,in 125.9 g of water?

What are the major solute-solvent interactions created when HOCH₂CH₂OH dissolves in water?

The normal boiling point of pure benzene is found to be 80.10°C.What is the approximate molecular weight of a nonionizing substance if a solution of 3.55 g of the substance dissolved in 100.g of benzene has a normal boiling point of 80.19°C? K_b = 5.12°C/m for benzene,C₆H₆.

The osmotic pressure of a 100-mL solution containing 1.0 g of sucrose,C₁₂H₂₂O₁₁will be ________ (equal to,greater than,less than)the osmotic pressure of a 100-mL solution containing 1.0 g of fructose,C₆H₁₂O₆.