Laura Pepe
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University Chemistry 102 Quiz on Chapter 13: Solutions, created by Laura Pepe on 10/02/2020.

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Chapter 13: Solutions

Chapter 13: Solutions

Question 1 of 25

1

The equation for molarity is

Select one of the following:

  • Moles of solute / Liter of solution

  • Moles of solute/ Moles of solution

  • Moles of solution/ Liters of solute

  • Liter of solution/ Moles of solute

Explanation

Question 2 of 25

1

Moles of a component over the total moles of the solution is known as?

Select one of the following:

  • Molality

  • Molarity

  • Mass percent

  • Mole Fraction

Explanation

Question 3 of 25

1

Mass of component/ total mass solution x 100 is mass percent.

Select one of the following:

  • True
  • False

Explanation

Question 4 of 25

1

CH3COOH is more soluble in which of these solutions?

Select one of the following:

  • H2O

  • CH3COOH

Explanation

Question 5 of 25

1

C6H6 is nonpolar and soluble in water.

Select one of the following:

  • True
  • False

Explanation

Question 6 of 25

1

What is the molarity of a solution made by dissolving 2.335 grams of H2SO4 in enough water to make 50 mL of solution?

Select one of the following:

  • .476 M

  • .764 M

  • 6.47 M

  • 7.46 M

Explanation

Question 7 of 25

1

How many mL of .200 m HCL solution are needed to obtain 0.0500 moles of HCL?

Select one of the following:

  • .250 mL

  • 250 mL

  • 4 mL

  • .400 mL

Explanation

Question 8 of 25

1

What is the mole fraction of methanol if 32.0 grams of methanol (CH3OH) is dissolved in 90 grams of water?

Select one of the following:

  • .166

  • .452

  • .998

  • 4.99

Explanation

Question 9 of 25

1

Which one of the following can be used as a solvent for hexane (C6H14)?

Select one of the following:

  • Methanol (CH3OH)

  • Benzene (C6H6)

  • Liquid ammonia

  • Water

Explanation

Question 10 of 25

1

What is the mass percent of a saline solution made by dissolving 1 mole of NaCl (mm = 58.45 g) in 1 liter of water total?

Select one of the following:

  • 5.84%

  • 5.52%

  • 5.00%

  • 11.34%

Explanation

Question 11 of 25

1

The NaCl concentration of seawater is 3.5% by mass. What is its molarity if the density of seawater is 1.025 g/mL?

Select one of the following:

  • 6.14 m

  • .614 m

  • .416 m

  • 1.46 m

Explanation

Question 12 of 25

1

Molality is the moles of solute/kg of solvent.

Select one of the following:

  • True
  • False

Explanation

Question 13 of 25

1

What is the molality of a solution made by dissolving 1.45 grams of sucrose C12H22O11 in 30 mL of water?

Select one of the following:

  • 14.1 M

  • .141 m

  • .141 M

  • 1.41 m

Explanation

Question 14 of 25

1

The density of a 45.0 mass % solution of ethanol (C2H5OH) in water is 0.873 g/mL. What is the molarity of the solution?

Select one of the following:

  • 8.53 M

  • 9.77 M

  • 15.5 M

  • 0.515 M

Explanation

Question 15 of 25

1

What is the mole fraction of HCl in a 4.50 m aqueous HCl solution?

Select one of the following:

  • 3.87

  • 0.222

  • 0.0750

  • 0.0811

Explanation

Question 16 of 25

1

What is the mass percent concentration of a saline solution prepared by dissolving 1.00 mol of Na2SO4 in 1.00 L of water?

Select one of the following:

  • 12.4%

  • 11.34%

  • 57%

  • 6%

Explanation

Question 17 of 25

1

Fill the blank space to complete the text.

The density at 20 ∘C of a 0.828 M solution of acetic acid in water is 1.0052 g/mL. The molar mass of acetic acid, CH3CO2H, is 60.05 g/mol. What is the molality of the solution?
Molality = m

Explanation

Question 18 of 25

1

Fill the blank space to complete the text.

The molality of a solution prepared by dissolving 22.5 g of H2SO4 in 1.80 L of water
m = m

Explanation

Question 19 of 25

1

Fill the blank spaces to complete the text.

The mole fraction of each component of a solution prepared by dissolving 2.05 g of nicotine, C10H14N2, in 88.0 g of CH2Cl2
XC10H14N2 , XCH2Cl2 = ,

Explanation

Question 20 of 25

1

The density of a 16.0 mass % solution of sulfuric acid in water is 1.1094 g/mL at 25.0 ∘C. What is the molarity of the solution?

Select one of the following:

  • 148.18 M

  • 2.12 M

  • 1.81M

  • 167.4 M

Explanation

Question 21 of 25

1

A 0.944 M solution of glucose, C6H12O6, in water, has a density of 1.0624 g/mL at 20∘C. What is the concentration of this solution in the following units?
What is the mole fraction?
What is the mass percent?
What is the molality?

Select one or more of the following:

  • Mole Fraction = 1.87×10−2

  • Mole Fraction = 1.10×10−4

  • Mass Percent = 37.0 mass %

  • Mass Percent = 16.0 mass %

  • Molality = 1.06 m

  • Molality = 3.04 m

Explanation

Question 22 of 25

1

Which of the following conditions will increase the solubility of a gas?

Select one of the following:

  • Low temperature and low pressure

  • Low temperature and high pressure

  • High temperature and low pressure

  • High temperature and high pressure

Explanation

Question 23 of 25

1

Henry's law constant is 3.2×10−2mol/(L⋅atm). Find the concentration of CO2 in: A can of soda under a CO2 pressure of 2.1 atm at 25 ∘C

Select one of the following:

  • 6.7×10−2 M

  • 7.7×10−2 M

  • 5.7×10−2 M

  • 8.7×10−2 M

Explanation

Question 24 of 25

1

Fill the blank space to complete the text.

Henry's law constant is 3.2×10−2mol/(L⋅atm). Find the concentration of CO2 in: A can of soda open to the atmosphere at 25 ∘C (CO2 is approximately 0.04% by volume in the atmosphere.)
Express your answer to two significant figures and include the appropriate units.
The answer is = M

Explanation

Question 25 of 25

1

Colligative properties are properties that changed when a solute is added. It depends on the number of solute particles not on what the solute is.

Select one of the following:

  • True
  • False

Explanation

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