Q: Which equation correctly expresses mass percent of a solute in a solution?

$$\text{mass percent} = \frac{\text{mass solute}}{\text{mass solute} + \text{mass solvent}} \times 100$$

Question 1

Which of the following statements best describes a solution?

Accepted Answer

A solution is a homogeneous mixture of two or more substances.

Question 2

In a solution of saltwater, which component is considered the solvent?

Accepted Answer

Water, because it is present in greater amount.

Question 3

Which statement correctly explains why sodium chloride (NaCl) dissolves in water?

Accepted Answer

The solvent-solute attractions (ion-dipole interactions) overcome the solute-solute and solvent-solvent attractions.

Question 4

Which of the following best describes the solubility of gases in liquids as temperature increases?

Accepted Answer

Solubility of gases in liquids decreases with increasing temperature.

Question 5

A solution is prepared by dissolving 36 g of NaCl in 100 g of water at 25°C. What type of solution is this?

Accepted Answer

Saturated solution

Question 6

Which of the following is a correct statement about electrolyte solutions?

Accepted Answer

Electrolyte solutions contain dissolved ions and conduct electricity.

Question 7

Which equation correctly expresses mass percent of a solute in a solution?

Accepted Answer

$$	ext{mass percent} = \frac{	ext{mass solute}}{	ext{mass solute} + 	ext{mass solvent}} 	imes 100$$

Question 8

A solution is made by dissolving 15.5 g of NaCl into enough water to make 1.50 L of solution. What is the molarity of NaCl? (Molar mass of NaCl = 58.44 g/mol)

Accepted Answer

$$0.177\ 	ext{M}$$

Question 9

Which of the following statements about molarity is correct?

Accepted Answer

Molarity is defined as moles of solute per liter of solution.

Question 10

A 1.0 M solution of CaCl$$_2$$ contains how many moles of Cl$$^-$$ ions per liter?

Accepted Answer

$$2.0\ 	ext{mol}$$

Question 11

Which equation is used to calculate the volume of stock solution needed to prepare a diluted solution?

Accepted Answer

$$M_1V_1 = M_2V_2$$

Question 12

If you have 0.100 L of 1.5 M NaOH and want to prepare a 1.0 M NaOH solution, what will be the final volume after dilution?

Accepted Answer

$$0.150\ 	ext{L}$$

Question 13

Which property is a colligative property?

Accepted Answer

Boiling point elevation

Question 14

What is the freezing point of a solution containing 1.1 molal ethylene glycol in water? ($$K_f$$ for water = $$1.86\ ^\circ	ext{C}\cdot	ext{kg solvent}/	ext{mol solute})$$

Accepted Answer

$$-2.05\ ^\circ	ext{C}$$

Question 15

Which equation is used to calculate freezing point depression?

Accepted Answer

$$\Delta T_f = m 	imes K_f$$

Question 16

A solution is made by dissolving 17.2 g of ethylene glycol ($$C_2H_6O_2) in 0.0500 kg of $$water. What is the molality of the solution? (Molar mass of ethylene glycol = 62.07 g/mol)

Accepted Answer

$$5.54\ 	ext{m}$$

Question 17

Which of the following best describes osmosis?

Accepted Answer

The flow of solvent from a less concentrated solution to a more concentrated solution through a semipermeable membrane.

Question 18

Why must intravenous (IV) solutions be isoosmotic with bodily fluids?

Accepted Answer

To prevent water from being pumped into or out of cells, maintaining cell integrity.

Solutions: Properties, Types, and Concentrations (Chapter 13 Study Notes)

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