Question 1

If the solubility of O2 at 0.360 bar and 25S1U1P1$\circ$S1S1P0C is 15.0 g/100 g H2O,what is the solubility of O2 at a pressure of 1.72 bar and 25S1U1P1$\circ$S1S1P0C?

Accepted Answer

A)  71.7 g/100 g H2O 
B)  24.2 g/100 g H2O 
C)  0.319 g/100 g H2O 
D)  0.0140 g/100 g H2O 
E)  3.14 g/100 g H2O 
A)  71.7 g/100 g H2O 
B)  24.2 g/100 g H2O 
C)  0.319 g/100 g H2O 
D)  0.0140 g/100 g H2O 
E)  3.14 g/100 g H2O

Question 2

What concentration unit is used in the calculation of osmotic pressure for a dilute solution?

Accepted Answer

A)  molality 
B)  weight percent 
C)  mass fraction 
D)  mole fraction 
E)  molarity 
A)  molality 
B)  weight percent 
C)  mass fraction 
D)  mole fraction 
E)  molarity

Question 3

Which action(s)will decrease the equilibrium concentration of an inert gas (such as N2)in water?
1)decreasing the temperature of the water
2)increasing the volume of water
3)decreasing the pressure of the gas above the liquid

Accepted Answer

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

Question 4

At a particular temperature the solubility of O2 in water is 0.590 g/L at an oxygen pressure of 15.2 atm.What is the Henry's law constant for O2?

Accepted Answer

A)  3.88 $\times$ 10-2 L·atm/mol 
B)  8.24 $\times$ 102 L·atm/mol 
C)  2.80 $\times$ 10-1 L·atm/mol 
D)  1.21 $\times$ 10-3 L·atm/mol 
E)  None of the above. 
A)  3.88 $\times$ 10-2 L·atm/mol 
B)  8.24 $\times$ 102 L·atm/mol 
C)  2.80 $\times$ 10-1 L·atm/mol 
D)  1.21 $\times$ 10-3 L·atm/mol 
E)  None of the above.

Question 5

How many milliliters of 15.7 M H2SO4 are needed to prepare 600.0 mL of 0.10 M H2SO4?

Accepted Answer

A)  0.26 mL 
B)  94 mL 
C)  3.8 mL 
D)  1.9 mL 
E)  4.8 mL 
A)  0.26 mL 
B)  94 mL 
C)  3.8 mL 
D)  1.9 mL 
E)  4.8 mL

Question 6

The solubility of 1-hexanol in water is 0.60 g per 100 g of water at 25°C.What is the maximum amount of 1-hexanol that will dissolve in 5.3 g of water at 25°C?

Accepted Answer

A)  0.032 g 
B)  0.11 g 
C)  0.60 g 
D)  3.2 g 
E)  0.0011 g 
A)  0.032 g 
B)  0.11 g 
C)  0.60 g 
D)  3.2 g 
E)  0.0011 g

Question 7

Which of the following statements is INCORRECT?

Accepted Answer

A)  The solubility of a gas in water decreases with increasing temperature. 
B)  The solubility of a gas in water is proportional to the partial pressure of the gas above the water. 
C)  The dissolution of a gas in water is usually an exothermic process. 
D)  The relationship between the solubility of a gas and its partial pressure is known as Henry's law. 
E)  The solubility of a gas in water is inversely proportional to the molar mass of the gas. 
A)  The solubility of a gas in water decreases with increasing temperature. 
B)  The solubility of a gas in water is proportional to the partial pressure of the gas above the water. 
C)  The dissolution of a gas in water is usually an exothermic process. 
D)  The relationship between the solubility of a gas and its partial pressure is known as Henry's law. 
E)  The solubility of a gas in water is inversely proportional to the molar mass of the gas.

Question 8

What is the mole fraction of urea,CH4N2O,in an aqueous solution that is 54% urea by mass?

Accepted Answer

A)  0.26 
B)  0.74 
C)  0.54 
D)  0.37 
E)  0.80 
A)  0.26 
B)  0.74 
C)  0.54 
D)  0.37 
E)  0.80

Question 9

The lattice enthalpy of KF is -808 kJ/mol and the enthalpy of solution of KF is -17.7 kJ/mol.Calculate the enthalpy of hydration of KF(s).

Accepted Answer

A)  -790.3 kJ/mol 
B)  -35.4 kJ/mol 
C)  -825.7 kJ/mol 
D)  790.3 kJ/mol 
E)  825.7 kJ/mol 
A)  -790.3 kJ/mol 
B)  -35.4 kJ/mol 
C)  -825.7 kJ/mol 
D)  790.3 kJ/mol 
E)  825.7 kJ/mol

Question 10

What is the equilibrium partial pressure of water vapor above a mixture of 37.5 g H2O and 62.5 g HOCH2CH2OH at 55 S1U1P1$\circ$S1S1P0C.The partial pressure of pure water at 55.0 S1U1P1$\circ$S1S1P0C is 118.0 mm Hg.Assume ideal behavior for the solution.

Accepted Answer

A)  3.54 mm Hg 
B)  31.7 mm Hg 
C)  38.5 mm Hg 
D)  79.5 mm Hg 
E)  175 mm Hg 
A)  3.54 mm Hg 
B)  31.7 mm Hg 
C)  38.5 mm Hg 
D)  79.5 mm Hg 
E)  175 mm Hg

Question 11

Because ________ particles are relatively large (say,1000 nm in diameter)they scatter visible light,making the mixtures containing these particles appear cloudy.This scattering is known as the Tyndall effect.

Accepted Answer

The answer of Because ________ particles are relatively large (say,1000...

Question 12

Colloids are described by all of the following   $\textbf{     except:      }$

Accepted Answer

A)  The particles in a colloid are so small that settling is negligible. 
B)  The mixture appears cloudy. 
C)  Only combinations of liquids and gases can form colloids. 
D)  Colloids are not suspensions or homogeneous mixtures. 
E)  Mayonnaise,whipped cream and fog are all examples of colloids. 
A)  The particles in a colloid are so small that settling is negligible. 
B)  The mixture appears cloudy. 
C)  Only combinations of liquids and gases can form colloids. 
D)  Colloids are not suspensions or homogeneous mixtures. 
E)  Mayonnaise,whipped cream and fog are all examples of colloids.

Question 13

Which of the following solutions has the lowest osmotic pressure?

Accepted Answer

A)  0.10 M Al(NO3)3 
B)  0.20 M NH3 
C)  0.15 M Ba(NO2)2 
D)  0.10 M CaCl2 
E)  0.15 M NaCl 
A)  0.10 M Al(NO3)3 
B)  0.20 M NH3 
C)  0.15 M Ba(NO2)2 
D)  0.10 M CaCl2 
E)  0.15 M NaCl

Question 14

Henry's law states that the solubility of a gas in a liquid is directly proportional to its pressure above the liquid.This law holds correct for gases such as nitrogen and oxygen.However,Henry's law does not hold correct for hydrogen chloride gas.Why?

Accepted Answer

Henry's law is only correct fo

Question 15

If a 25.0-g sample of a nonelectrolyte is dissolved in 145.0 g of water,the resulting solution will freeze at -0.89°C.What is the molar mass of the nonelectrolyte? (Kfp for water is 1.858°C/m.)

Accepted Answer

A)  76 g/mol 
B)  0.36 g/mol 
C)  990 g/mol 
D)  290 g/mol 
E)  360 g/mol 
A)  76 g/mol 
B)  0.36 g/mol 
C)  990 g/mol 
D)  290 g/mol 
E)  360 g/mol

Question 16

If an egg's shell is carefully dissolved using an acid,the egg white and yolk will remain intact inside a membrane.If the egg is then placed in distilled water,it will slowly expand until it bursts.Why?

Accepted Answer

This is an example of osmotic pressure.T

Question 17

What mass of an aqueous 22.9% sodium chloride solution contains 99.5 g of water?

Accepted Answer

A)  129 g 
B)  29.6 g 
C)  0.500 g 
D)  22.8 g 
E)  99.5 g 
A)  129 g 
B)  29.6 g 
C)  0.500 g 
D)  22.8 g 
E)  99.5 g

Question 18

What is the mass percent of an aqueous sodium hydroxide solution in which the mole fraction of NaOH is 0.101?

Accepted Answer

A)  20.0% 
B)  12.1% 
C)  68.9% 
D)  12.4% 
E)  3.31% 
A)  20.0% 
B)  12.1% 
C)  68.9% 
D)  12.4% 
E)  3.31%

Question 19

For a dilute solution of NH4NO3,the van't Hoff factor (i)would be approximately ___.

Accepted Answer

A)  1 
B)  2 
C)  3 
D)  4 
E)  5 
A)  1 
B)  2 
C)  3 
D)  4 
E)  5

Question 20

A 15 meter by 12 meter pool of water has a depth of 2.2 meters.What mass of silver ion is present in the reservoir if the concentration of silver ion is 0.14 ppm? (1 m3 = 1000 L; assume the density of the solution is 1.00 g/mL)

Accepted Answer

A)  5.5 $\times$ 10-4 g 
B)  5.5 $\times$ 10-2 g 
C)  0.55 g 
D)  5.5 g 
E)  55 g 
A)  5.5 $\times$ 10-4 g 
B)  5.5 $\times$ 10-2 g 
C)  0.55 g 
D)  5.5 g 
E)  55 g

Exam 14: Solutions and Their Behavior

If the solubility of O2 at 0.360 bar and 25 ∘\circ∘ C is 15.0 g/100 g H2O,what is the solubility of O2 at a pressure of 1.72 bar and 25 ∘\circ∘ C?

What concentration unit is used in the calculation of osmotic pressure for a dilute solution?

Which action(s)will decrease the equilibrium concentration of an inert gas (such as N2)in water? 1)decreasing the temperature of the water 2)increasing the volume of water 3)decreasing the pressure of the gas above the liquid

At a particular temperature the solubility of O2 in water is 0.590 g/L at an oxygen pressure of 15.2 atm.What is the Henry's law constant for O2?

How many milliliters of 15.7 M H2SO4 are needed to prepare 600.0 mL of 0.10 M H2SO4?

The solubility of 1-hexanol in water is 0.60 g per 100 g of water at 25°C.What is the maximum amount of 1-hexanol that will dissolve in 5.3 g of water at 25°C?

Which of the following statements is INCORRECT?

What is the mole fraction of urea,CH4N2O,in an aqueous solution that is 54% urea by mass?

The lattice enthalpy of KF is -808 kJ/mol and the enthalpy of solution of KF is -17.7 kJ/mol.Calculate the enthalpy of hydration of KF(s).

What is the equilibrium partial pressure of water vapor above a mixture of 37.5 g H2O and 62.5 g HOCH2CH2OH at 55 ∘\circ∘ C.The partial pressure of pure water at 55.0 ∘\circ∘ C is 118.0 mm Hg.Assume ideal behavior for the solution.

Because ________ particles are relatively large (say,1000 nm in diameter)they scatter visible light,making the mixtures containing these particles appear cloudy.This scattering is known as the Tyndall effect.

Colloids are described by all of the following except: \textbf{ except: } except:

Which of the following solutions has the lowest osmotic pressure?

Henry's law states that the solubility of a gas in a liquid is directly proportional to its pressure above the liquid.This law holds correct for gases such as nitrogen and oxygen.However,Henry's law does not hold correct for hydrogen chloride gas.Why?

If a 25.0-g sample of a nonelectrolyte is dissolved in 145.0 g of water,the resulting solution will freeze at -0.89°C.What is the molar mass of the nonelectrolyte? (Kfp for water is 1.858°C/m.)

If an egg's shell is carefully dissolved using an acid,the egg white and yolk will remain intact inside a membrane.If the egg is then placed in distilled water,it will slowly expand until it bursts.Why?

What mass of an aqueous 22.9% sodium chloride solution contains 99.5 g of water?

What is the mass percent of an aqueous sodium hydroxide solution in which the mole fraction of NaOH is 0.101?

For a dilute solution of NH4NO3,the van't Hoff factor (i)would be approximately ___.

A 15 meter by 12 meter pool of water has a depth of 2.2 meters.What mass of silver ion is present in the reservoir if the concentration of silver ion is 0.14 ppm? (1 m3 = 1000 L; assume the density of the solution is 1.00 g/mL)

Basic Concepts of Chemistry

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Stoichiometry: Quantitative Information About Chemical Reactions

Principles of Chemical Reactivity: Energy and Chemical Reactions

The Structure of Atoms

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Bonding and Molecular Structure: Orbital Hybridization and Molecular Orbitals

Gases and Their Properties

Intermolecular Forces and Liquids

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Chemical Kinetics: the Rates of Chemical Reactions

Principles of Reactivity: Chemical Equilibria

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If the solubility of O₂ at 0.360 bar and 25^$\circ$C is 15.0 g/100 g H₂O,what is the solubility of O₂ at a pressure of 1.72 bar and 25^$\circ$C?

Which action(s)will decrease the equilibrium concentration of an inert gas (such as N₂)in water? 1)decreasing the temperature of the water 2)increasing the volume of water 3)decreasing the pressure of the gas above the liquid

At a particular temperature the solubility of O₂ in water is 0.590 g/L at an oxygen pressure of 15.2 atm.What is the Henry's law constant for O₂?

How many milliliters of 15.7 M H₂SO₄ are needed to prepare 600.0 mL of 0.10 M H₂SO₄?

What is the mole fraction of urea,CH₄N₂O,in an aqueous solution that is 54% urea by mass?

What is the equilibrium partial pressure of water vapor above a mixture of 37.5 g H₂O and 62.5 g HOCH₂CH₂OH at 55 ^$\circ$C.The partial pressure of pure water at 55.0 ^$\circ$C is 118.0 mm Hg.Assume ideal behavior for the solution.

Colloids are described by all of the following $\textbf{ except: }$

If a 25.0-g sample of a nonelectrolyte is dissolved in 145.0 g of water,the resulting solution will freeze at -0.89°C.What is the molar mass of the nonelectrolyte? (K_fp for water is 1.858°C/m.)

For a dilute solution of NH₄NO₃,the van't Hoff factor (i)would be approximately ___.

A 15 meter by 12 meter pool of water has a depth of 2.2 meters.What mass of silver ion is present in the reservoir if the concentration of silver ion is 0.14 ppm? (1 m³ = 1000 L; assume the density of the solution is 1.00 g/mL)