Question 1

The solubility of MnSO4 monohydrate in water at 20 °C is 70.0 g per 100.0 mL of water. A solution at 20 °C that is 4.22 M in MnSO4 monohydrate is best described as a(n) solution. The formula weight of MnSO4 monohydrate is 168.97 g/mol.

Accepted Answer

A)  solvated 
B)  supersaturated 
C)  hydrated 
D)  unsaturated 
E)  saturated

Question 2

The concentration of a benzene solution prepared by mixing 12.0 g C6H6 with 38.0 g CCl4 is
Molal.

Accepted Answer

A)  0.240 
B)  4.04 
C)  0.508 
D)  0.622 
E)  0.316

Question 3

Determine the freezing point (°C) of a 0.015 molal aqueous solution of MgSO4. Assume i = 2.0 for MgSO4. The molal freezing- point- depression constant of water is 1.86 °C/m.

Accepted Answer

A)  0.000 
B)  - 0.056 
C)  - 0.028 
D)  - 0.084 
E)  - 0.17

Question 4

The solubility of oxygen gas in water at 25 °C and 1.0 atm pressure of oxygen is 0.041 g/L. The solubility of oxygen in water at 3.0 atm and 25 °C is g/L.

Accepted Answer

A)  3.0 
B)  0.12 
C)  0.31 
D)  0.014 
E)  0.041

Question 5

The concentration of lead nitrate (Pb(NO3)2) in a 0.726 M solution is molal. The density of the solution is 1.202 g/mL.

Accepted Answer

A)  1.928 
B)  0.650 
C)  0.755 
D)  0.819 
E)  0.476

Question 6

A solution is prepared by adding 30.00 g of lactose (milk sugar) to 110.0 g of water at 55 °C. The partial pressure of water above the solution is torr. The vapor pressure of pure water at 55 °C is 118 torr. The MW of lactose is 342.3 g/mol.

Accepted Answer

A)  169.4 
B)  1.670 
C)  92.7 
D)  94.1 
E)  116.3

Question 7

Determine the fraction of ionization of HX if a solution prepared by dissolving 0.020 mol of HX in 115 g of water freezes at - 0.47 °C. The molal freezing- point- depression constant of water is
1)86 °C/m.

Accepted Answer

A)  1.45 
B)  0.45 
C)  0.044 
D)  0.348 
E)  0.30

Question 8

The solubility of Ar in water at 25 °C is 1.6 × 10- 3 M when the pressure of the Ar above the solution is 1.0 atm. The solubility of Ar at a pressure of 2.5 atm is M.

Accepted Answer

A)  4.0 × 10- 3  
B)  7.5 × 10- 2  
C)  1.6 × 10- 3  
D)  6.4 × 10- 4  
E)  1.6 × 103

Question 9

A solution contains 150.8 grams of NaCl in 678.3 grams of water. Calculate the vapor pressure of water (in torr) over the solution at 25.0 ^oC. (Note: the vapor pressure of pure water at 25.0 ^oC is 23.76 torr.)

Accepted Answer

The answer of A solution contains 150.8 grams of NaCl...

Question 10

Physical properties of a solution that depend on the quantity of the solute particles present, but not the kind or identity of the particles, are termed properties.

Accepted Answer

The answer of Physical properties of a solution that depend...

Question 11

A solution containing 10.0 g of an unknown liquid and 90.0 g water has a freezing point of - 3.33 °C. Given Kf = 1.86 °C/m for water, the molar mass of the unknown liquid is g/mol.

Accepted Answer

A)  69.0 
B)  161 
C)  333 
D)  619 
E)  62.1

Question 12

A solution is prepared by dissolving 23.7 g of CaCl2 in 375 g of water. The density of the resulting solution is 1.05 g/mL. The concentration of CaCl2 in this solution is molal.

Accepted Answer

A)  5.70 
B)  63.2 
C)  1.76 
D)  0.214 
E)  0.569

Question 13

A solution contains 150.8 grams of NaCl in 678.3 grams of water. Calculate the vapor pressure lowering (in torr) of the solution at 25.0 ^oC. (Note: the vapor pressure of pure water at 25.0 ^oC is 23.76 torr.)

Accepted Answer

The answer of A solution contains 150.8 grams of NaCl...

Question 14

Which produces the greatest number of ions when one mole dissolves in water?

Accepted Answer

A)  NH4NO3  
B)  NH4Cl 
C)  Na2SO4  
D)  NaCl 
E)  sucrose

Question 15

When two nonpolar organic liquids are mixed, a solution forms and the enthalpy of solution is quite small. Label the two organic liquids as A (solvent) and B (solute) The formation of solution is favored by .

Accepted Answer

A)  the highly negative enthalpy of the solution process 
B)  an increase in disorder, since A- A, B- B, and A- B interactions are similar 
C)  solvation of the solvent, A 
D)  hydration of the solute, B 
E)  the equal enthalpy of the solvent and solute

Question 16

The concentration of urea (MW = 60.0 g/mol) in a solution prepared by dissolving 16 g of urea in 39 g of H2O is molal.

Accepted Answer

A)  0.68 
B)  0.11 
C)  6.9 
D)  96 
E)  6.3

Question 17

A solution is prepared by dissolving 2.60 g of a strong electrolyte (formula weight = 101 g/mol) in enough water to make 1.00 L of solution. The osmotic pressure of the solution is 1.25 atm at 25.0 °C. What is the van't Hoff factor (i) for the unknown solute?

Accepted Answer

A)  0 
B)  0.99 
C)  1.98 
D)  2.98 
E)  0.630

Question 18

As the concentration of a solute in a solution increases, the freezing point of the solution
And the vapor pressure of the solution .

Accepted Answer

A)  decreases, increases 
B)  decreases, is unaffected 
C)  increases, increases 
D)  decreases, decreases 
E)  increases, decreases

Question 19

The value of the boiling- point- elevation constant (Kb) depends on the identity of the solvent.

Accepted Answer

A) True 
 B)False

Question 20

Which one of the following is most soluble in water?

Accepted Answer

A)  CH3CH2OH 
B)  CH3CH2CH2CH2OH 
C)  CH3OH 
D)  CH3CH2CH2OH 
E)  CH3CH2CH2CH2CH2OH

Exam 13: Properties of Solutions

The solubility of MnSO₄monohydrate in water at 20 °C is 70.0 g per 100.0 mL of water. A solution at 20 °C that is 4.22 M in MnSO₄monohydrate is best described as a(n) solution. The formula weight of MnSO₄monohydrate is 168.97 g/mol.

The concentration of a benzene solution prepared by mixing 12.0 g C₆H₆with 38.0 g CCl₄is Molal.

Determine the freezing point (°C) of a 0.015 molal aqueous solution of MgSO₄. Assume i = 2.0 for MgSO₄. The molal freezing- point- depression constant of water is 1.86 °C/m.

The solubility of oxygen gas in water at 25 °C and 1.0 atm pressure of oxygen is 0.041 g/L. The solubility of oxygen in water at 3.0 atm and 25 °C is g/L.

The concentration of lead nitrate (Pb(NO₃) ₂) in a 0.726 M solution is molal. The density of the solution is 1.202 g/mL.

A solution is prepared by adding 30.00 g of lactose (milk sugar) to 110.0 g of water at 55 °C. The partial pressure of water above the solution is torr. The vapor pressure of pure water at 55 °C is 118 torr. The MW of lactose is 342.3 g/mol.

Determine the fraction of ionization of HX if a solution prepared by dissolving 0.020 mol of HX in 115 g of water freezes at - 0.47 °C. The molal freezing- point- depression constant of water is 1) 86 °C/m.

The solubility of Ar in water at 25 °C is 1.6 × 10^-³M when the pressure of the Ar above the solution is 1.0 atm. The solubility of Ar at a pressure of 2.5 atm is M.

A solution contains 150.8 grams of NaCl in 678.3 grams of water. Calculate the vapor pressure of water (in torr) over the solution at 25.0 ^oC. (Note: the vapor pressure of pure water at 25.0 ^oC is 23.76 torr.)

Physical properties of a solution that depend on the quantity of the solute particles present, but not the kind or identity of the particles, are termed properties.

A solution containing 10.0 g of an unknown liquid and 90.0 g water has a freezing point of - 3.33 °C. Given K_f= 1.86 °C/m for water, the molar mass of the unknown liquid is g/mol.

A solution is prepared by dissolving 23.7 g of CaCl₂in 375 g of water. The density of the resulting solution is 1.05 g/mL. The concentration of CaCl₂in this solution is molal.

A solution contains 150.8 grams of NaCl in 678.3 grams of water. Calculate the vapor pressure lowering (in torr) of the solution at 25.0 ^oC. (Note: the vapor pressure of pure water at 25.0 ^oC is 23.76 torr.)

Which produces the greatest number of ions when one mole dissolves in water?

When two nonpolar organic liquids are mixed, a solution forms and the enthalpy of solution is quite small. Label the two organic liquids as A (solvent) and B (solute) The formation of solution is favored by .

The concentration of urea (MW = 60.0 g/mol) in a solution prepared by dissolving 16 g of urea in 39 g of H₂O is molal.

A solution is prepared by dissolving 2.60 g of a strong electrolyte (formula weight = 101 g/mol) in enough water to make 1.00 L of solution. The osmotic pressure of the solution is 1.25 atm at 25.0 °C. What is the van't Hoff factor (i) for the unknown solute?

As the concentration of a solute in a solution increases, the freezing point of the solution And the vapor pressure of the solution .

The value of the boiling- point- elevation constant (K_b) depends on the identity of the solvent.

Which one of the following is most soluble in water?

Exam 13: Properties of Solutions

The solubility of MnSO4 monohydrate in water at 20 °C is 70.0 g per 100.0 mL of water. A solution at 20 °C that is 4.22 M in MnSO4 monohydrate is best described as a(n) solution. The formula weight of MnSO4 monohydrate is 168.97 g/mol.

The concentration of a benzene solution prepared by mixing 12.0 g C6H6 with 38.0 g CCl4 is Molal.

Determine the freezing point (°C) of a 0.015 molal aqueous solution of MgSO4. Assume i = 2.0 for MgSO4. The molal freezing- point- depression constant of water is 1.86 °C/m.

The solubility of oxygen gas in water at 25 °C and 1.0 atm pressure of oxygen is 0.041 g/L. The solubility of oxygen in water at 3.0 atm and 25 °C is g/L.

The concentration of lead nitrate (Pb(NO3) 2) in a 0.726 M solution is molal. The density of the solution is 1.202 g/mL.

A solution is prepared by adding 30.00 g of lactose (milk sugar) to 110.0 g of water at 55 °C. The partial pressure of water above the solution is torr. The vapor pressure of pure water at 55 °C is 118 torr. The MW of lactose is 342.3 g/mol.

Determine the fraction of ionization of HX if a solution prepared by dissolving 0.020 mol of HX in 115 g of water freezes at - 0.47 °C. The molal freezing- point- depression constant of water is 1) 86 °C/m.

The solubility of Ar in water at 25 °C is 1.6 × 10- 3 M when the pressure of the Ar above the solution is 1.0 atm. The solubility of Ar at a pressure of 2.5 atm is M.

A solution contains 150.8 grams of NaCl in 678.3 grams of water. Calculate the vapor pressure of water (in torr) over the solution at 25.0 oC. (Note: the vapor pressure of pure water at 25.0 oC is 23.76 torr.)

Physical properties of a solution that depend on the quantity of the solute particles present, but not the kind or identity of the particles, are termed properties.

A solution containing 10.0 g of an unknown liquid and 90.0 g water has a freezing point of - 3.33 °C. Given Kf = 1.86 °C/m for water, the molar mass of the unknown liquid is g/mol.

A solution is prepared by dissolving 23.7 g of CaCl2 in 375 g of water. The density of the resulting solution is 1.05 g/mL. The concentration of CaCl2 in this solution is molal.

A solution contains 150.8 grams of NaCl in 678.3 grams of water. Calculate the vapor pressure lowering (in torr) of the solution at 25.0 oC. (Note: the vapor pressure of pure water at 25.0 oC is 23.76 torr.)

Which produces the greatest number of ions when one mole dissolves in water?

When two nonpolar organic liquids are mixed, a solution forms and the enthalpy of solution is quite small. Label the two organic liquids as A (solvent) and B (solute) The formation of solution is favored by .

The concentration of urea (MW = 60.0 g/mol) in a solution prepared by dissolving 16 g of urea in 39 g of H2O is molal.

A solution is prepared by dissolving 2.60 g of a strong electrolyte (formula weight = 101 g/mol) in enough water to make 1.00 L of solution. The osmotic pressure of the solution is 1.25 atm at 25.0 °C. What is the van't Hoff factor (i) for the unknown solute?

As the concentration of a solute in a solution increases, the freezing point of the solution And the vapor pressure of the solution .

The value of the boiling- point- elevation constant (Kb) depends on the identity of the solvent.

Which one of the following is most soluble in water?

The solubility of MnSO₄monohydrate in water at 20 °C is 70.0 g per 100.0 mL of water. A solution at 20 °C that is 4.22 M in MnSO₄monohydrate is best described as a(n) solution. The formula weight of MnSO₄monohydrate is 168.97 g/mol.

The concentration of a benzene solution prepared by mixing 12.0 g C₆H₆with 38.0 g CCl₄is Molal.

Determine the freezing point (°C) of a 0.015 molal aqueous solution of MgSO₄. Assume i = 2.0 for MgSO₄. The molal freezing- point- depression constant of water is 1.86 °C/m.

The concentration of lead nitrate (Pb(NO₃) ₂) in a 0.726 M solution is molal. The density of the solution is 1.202 g/mL.

The solubility of Ar in water at 25 °C is 1.6 × 10^-³M when the pressure of the Ar above the solution is 1.0 atm. The solubility of Ar at a pressure of 2.5 atm is M.

A solution contains 150.8 grams of NaCl in 678.3 grams of water. Calculate the vapor pressure of water (in torr) over the solution at 25.0 ^oC. (Note: the vapor pressure of pure water at 25.0 ^oC is 23.76 torr.)

A solution containing 10.0 g of an unknown liquid and 90.0 g water has a freezing point of - 3.33 °C. Given K_f= 1.86 °C/m for water, the molar mass of the unknown liquid is g/mol.

A solution is prepared by dissolving 23.7 g of CaCl₂in 375 g of water. The density of the resulting solution is 1.05 g/mL. The concentration of CaCl₂in this solution is molal.

A solution contains 150.8 grams of NaCl in 678.3 grams of water. Calculate the vapor pressure lowering (in torr) of the solution at 25.0 ^oC. (Note: the vapor pressure of pure water at 25.0 ^oC is 23.76 torr.)

The concentration of urea (MW = 60.0 g/mol) in a solution prepared by dissolving 16 g of urea in 39 g of H₂O is molal.

The value of the boiling- point- elevation constant (K_b) depends on the identity of the solvent.