Question 1

What is the molarity and molality of a solution that is 10.00 % by mass potassium hydrogen carbonate (KHCO3, 100.11 g/mol)and has a density of 1.0650 g/mL?

Accepted Answer

Question 2

A solution is prepared by adding 40.3 g of Mg(NO3)2 to 127 g of water.Calculate the mole fraction and molality of magnesium nitrate in this solution.

Accepted Answer

mole fract

Question 3

The concentration of nitrogen in water at 25°C was determined to be 7.2 × 10-6 M.Calculate the partial pressure of nitrogen at the surface of the water in mmHg.The Henry's law constant for nitrogen gas at 25°C is 6.8 × 10-4 mol/L·atm?

Accepted Answer

Question 4

In how many grams of water should 25.31 g of potassium nitrate (KNO3)be dissolved to prepare a 0.1982 m solution?

Accepted Answer

A) 250.0 g 
B) 792.0 g 
C) 1,000.g 
D) 1,263 g 
E) 7,917 g 
A) 250.0 g 
B) 792.0 g 
C) 1,000.g 
D) 1,263 g 
E) 7,917 g

Question 5

Which of the following liquids would make a good solvent for iodine, I2?

Accepted Answer

A) HCl 
B) H2O 
C) CH3OH 
D) NH3 
E) CS2 
A) HCl 
B) H2O 
C) CH3OH 
D) NH3 
E) CS2

Question 6

Which of the following gases is expected to have a higher solubility in water than what is predicted using Henry's law?

Accepted Answer

A) N2 
B) CH4 
C) Ar 
D) NH3 
E) H2 
A) N2 
B) CH4 
C) Ar 
D) NH3 
E) H2

Question 7

The vapor pressure of a solution depends on the chemical nature of the solvent

Accepted Answer

A) True 
 B)False

Question 8

At 10°C one volume of water dissolves 3.10 volumes of chlorine gas at 1.00 atm pressure.What is the Henry's Law constant in mol/L·atm?

Accepted Answer

A) 0.043 
B) 0.13 
C) 3.1 
D) 3.8 
E) 36. 
A) 0.043 
B) 0.13 
C) 3.1 
D) 3.8 
E) 36.

Question 9

What is the percent by mass of a Na2SO4 solution in water with a mole fraction of Na2SO4, X = 0.350 ?

Accepted Answer

A) 2.76% 
B) 4.25% 
C) 19.1% 
D) 73.4 % 
E) 80.9% 
A) 2.76% 
B) 4.25% 
C) 19.1% 
D) 73.4 % 
E) 80.9%

Question 10

List the following solutions in order of decreasing melting point: 0.20m glycerol, 0.11m Sc(NO3)3, 0.15m K2CO3

Accepted Answer

glycerol <

Question 11

What is the molarity of a solution that is 5.50 % by mass oxalic acid (C2H2O4)and has a density of 1.0244 g/mL?

Accepted Answer

Question 12

How many grams of sucrose (C12H22O11, 342.3 g/mol)would be needed to make 2.5 L of a solution with an osmotic pressure of 14 atm at 25°C? (R = 0.0821 L.atm/K.mol)

Accepted Answer

A) 0.57 g 
B) 6.8 g 
C) 2.0 × 102 g 
D) 4.9 × 102 g 
E) 5.8 × 103 g 
A) 0.57 g 
B) 6.8 g 
C) 2.0 × 102 g 
D) 4.9 × 102 g 
E) 5.8 × 103 g

Question 13

The vapor pressure of water at 45.0 °C is 71.93 mmHg.Calculate the vapor pressure of a solution of 1.25m Al(ClO3)3 at this temperature (assume 100% dissociation)

Accepted Answer

A) 360.mmHg 
B) 89.9 mmHg 
C) 71.9 mmHg 
D) 70.4 mmHg 
E) 66.0 mmHg 
A) 360.mmHg 
B) 89.9 mmHg 
C) 71.9 mmHg 
D) 70.4 mmHg 
E) 66.0 mmHg

Question 14

Calculate the boiling point of a 4.5 m solution of Na2SO4 in water (assume 100% dissociation, Kb (H2O)= 0.52 °C/m)

Accepted Answer

A) 93.0 °C 
B) 97.7 °C 
C) 102.3°C 
D) 104.7°C 
E) 107.0°C 
A) 93.0 °C 
B) 97.7 °C 
C) 102.3°C 
D) 104.7°C 
E) 107.0°C

Question 15

Plasma is the fluid portion of blood.The concentration of acetylsalicylic acid (aspirin, C9H8O4, molar mass = 180.g/mol)in your plasma is found to be 2.99 × 10-4 M after you take two tablets of aspirin.If the volume of your plasma is 5.85 L, how many grams of aspirin are in your blood? (Assume that the density of plasma is 1.00 g/mL.)

Accepted Answer

Question 16

Calculate the molality of a 20.0% by mass ammonium sulfate (NH4)2SO4 solution.The density of the solution is 1.117 g/mL.

Accepted Answer

A) 0.150 m 
B) 1.51 m 
C) 1.70 m 
D) 1.89 m 
E) 2.10 m 
A) 0.150 m 
B) 1.51 m 
C) 1.70 m 
D) 1.89 m 
E) 2.10 m

Question 17

Which of the following aqueous solutions has the highest boiling point (assume 100% dissociation for all soluble ionic compounds)?

Accepted Answer

A) 0.10m Al(NO3)3 
B) 0.11m Na2SO4 
C) 0.15m K2CO3 
D) 0.18m NaCl 
E) 0.35m C6H12O6 
A) 0.10m Al(NO3)3 
B) 0.11m Na2SO4 
C) 0.15m K2CO3 
D) 0.18m NaCl 
E) 0.35m C6H12O6

Question 18

What is the osmotic pressure of a solution that contains 13.7 g of propyl alcohol (C3H7OH)dissolved in enough water to make 500.mL of solution at 27°C?

Accepted Answer

A) 0.0100 atm 
B) 0.0140 atm 
C) 0.0370 atm 
D) 0.456 atm 
E) 11.2 atm 
A) 0.0100 atm 
B) 0.0140 atm 
C) 0.0370 atm 
D) 0.456 atm 
E) 11.2 atm

Question 19

Calculate the molality of a solution containing 14.3 g of NaCl in 42.2 g of water.

Accepted Answer

A) 2.45 × 10-4 m 
B) 5.80 × 10-4 m 
C) 2.45 × 10-1 m 
D) 103 m 
E) 5.80 m 
A) 2.45 × 10-4 m 
B) 5.80 × 10-4 m 
C) 2.45 × 10-1 m 
D) 103 m 
E) 5.80 m

Question 20

What is the molality of a 0.142 M Na3PO4(aq)solution that has a density of 1.015 g/mL?

Accepted Answer

Exam 12: Physical Properties of Solutions

What is the molarity and molality of a solution that is 10.00 % by mass potassium hydrogen carbonate (KHCO3, 100.11 g/mol)and has a density of 1.0650 g/mL?

A solution is prepared by adding 40.3 g of Mg(NO3)2 to 127 g of water.Calculate the mole fraction and molality of magnesium nitrate in this solution.

The concentration of nitrogen in water at 25°C was determined to be 7.2 × 10-6 M.Calculate the partial pressure of nitrogen at the surface of the water in mmHg.The Henry's law constant for nitrogen gas at 25°C is 6.8 × 10-4 mol/L·atm?

In how many grams of water should 25.31 g of potassium nitrate (KNO3)be dissolved to prepare a 0.1982 m solution?

Which of the following liquids would make a good solvent for iodine, I2?

Which of the following gases is expected to have a higher solubility in water than what is predicted using Henry's law?

The vapor pressure of a solution depends on the chemical nature of the solvent

At 10°C one volume of water dissolves 3.10 volumes of chlorine gas at 1.00 atm pressure.What is the Henry's Law constant in mol/L·atm?

What is the percent by mass of a Na2SO4 solution in water with a mole fraction of Na2SO4, X = 0.350 ?

List the following solutions in order of decreasing melting point: 0.20m glycerol, 0.11m Sc(NO3)3, 0.15m K2CO3

What is the molarity of a solution that is 5.50 % by mass oxalic acid (C2H2O4)and has a density of 1.0244 g/mL?

How many grams of sucrose (C12H22O11, 342.3 g/mol)would be needed to make 2.5 L of a solution with an osmotic pressure of 14 atm at 25°C? (R = 0.0821 L.atm/K.mol)

The vapor pressure of water at 45.0 °C is 71.93 mmHg.Calculate the vapor pressure of a solution of 1.25m Al(ClO3)3 at this temperature (assume 100% dissociation)

Calculate the boiling point of a 4.5 m solution of Na2SO4 in water (assume 100% dissociation, Kb (H2O)= 0.52 °C/m)

Calculate the molality of a 20.0% by mass ammonium sulfate (NH4)2SO4 solution.The density of the solution is 1.117 g/mL.

Which of the following aqueous solutions has the highest boiling point (assume 100% dissociation for all soluble ionic compounds)?

What is the osmotic pressure of a solution that contains 13.7 g of propyl alcohol (C3H7OH)dissolved in enough water to make 500.mL of solution at 27°C?

Calculate the molality of a solution containing 14.3 g of NaCl in 42.2 g of water.

What is the molality of a 0.142 M Na3PO4(aq)solution that has a density of 1.015 g/mL?

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What is the molarity and molality of a solution that is 10.00 % by mass potassium hydrogen carbonate (KHCO₃, 100.11 g/mol)and has a density of 1.0650 g/mL?

A solution is prepared by adding 40.3 g of Mg(NO₃)₂ to 127 g of water.Calculate the mole fraction and molality of magnesium nitrate in this solution.

The concentration of nitrogen in water at 25°C was determined to be 7.2 × 10^-6 M.Calculate the partial pressure of nitrogen at the surface of the water in mmHg.The Henry's law constant for nitrogen gas at 25°C is 6.8 × 10^-4 mol/L·atm?

In how many grams of water should 25.31 g of potassium nitrate (KNO₃)be dissolved to prepare a 0.1982 m solution?

Which of the following liquids would make a good solvent for iodine, I₂?

What is the percent by mass of a Na₂SO₄ solution in water with a mole fraction of Na₂SO₄, X = 0.350 ?

List the following solutions in order of decreasing melting point: 0.20m glycerol, 0.11m Sc(NO₃)₃, 0.15m K₂CO₃

What is the molarity of a solution that is 5.50 % by mass oxalic acid (C₂H₂O₄)and has a density of 1.0244 g/mL?

How many grams of sucrose (C₁₂H₂₂O₁₁, 342.3 g/mol)would be needed to make 2.5 L of a solution with an osmotic pressure of 14 atm at 25°C? (R = 0.0821 L.atm/K.mol)

The vapor pressure of water at 45.0 °C is 71.93 mmHg.Calculate the vapor pressure of a solution of 1.25m Al(ClO₃)₃ at this temperature (assume 100% dissociation)

Calculate the boiling point of a 4.5 m solution of Na₂SO₄ in water (assume 100% dissociation, K_b (H₂O)= 0.52 °C/m)

Calculate the molality of a 20.0% by mass ammonium sulfate (NH₄)₂SO₄ solution.The density of the solution is 1.117 g/mL.

What is the osmotic pressure of a solution that contains 13.7 g of propyl alcohol (C₃H₇OH)dissolved in enough water to make 500.mL of solution at 27°C?

What is the molality of a 0.142 M Na₃PO₄(aq)solution that has a density of 1.015 g/mL?