Question 1

Which property of water is primarily responsible for its high surface tension?

Accepted Answer

Its hydrogen bonding

Question 2

A solution is prepared by dissolving 145 g of NaCl in enough water to make 2.75 L of solution. What is the molarity of the solution? (Molar mass of NaCl = 58.44 g/mol)

Accepted Answer

$$\displaystyle 0.900\ \mathrm{M}$$

Question 3

Which of the following best describes why ice floats on liquid water?

Accepted Answer

Ice is less dense than liquid water because hydrogen bonds hold water molecules further apart in the solid state.

Question 4

How many grams of KCl are needed to prepare 0.750 L of a 1.50 M solution? (Molar mass of KCl = 74.55 g/mol)

Accepted Answer

$$\displaystyle 83.6\ \mathrm{g}$$

Question 5

Which of the following statements about electrolytes is correct?

Accepted Answer

All ionic compounds are electrolytes because they dissociate into ions in solution.

Question 6

What is the molarity of a solution produced when 85.6 g of HCl is dissolved in enough water to make 0.385 L of solution? (Molar mass of HCl = 36.46 g/mol)

Accepted Answer

$$\displaystyle 2.42\ \mathrm{M}$$

Question 7

Which of the following best describes a saturated solution?

Accepted Answer

A solution in which no more solute can dissolve at a given temperature.

Question 8

To produce 3.00 L of a 1.90 M NaOH solution, how many grams of NaOH must be dissolved? (Molar mass of NaOH = 40.00 g/mol)

Accepted Answer

$$\displaystyle 228\ \mathrm{g}$$

Question 9

Which of the following is an example of a homogeneous mixture?

Accepted Answer

Salt water

Question 10

Which of the following best explains why lakes do not evaporate quickly?

Accepted Answer

Water has low vapor pressure due to hydrogen bonding.

Question 11

What is the molarity of a solution produced when 8.77 g of KI is dissolved in enough water to make 4.75 L of solution? (Molar mass of KI = 166.00 g/mol)

Accepted Answer

$$\displaystyle 0.0114\ \mathrm{M}$$

Question 12

Which of the following best describes the Tyndall effect?

Accepted Answer

The scattering of light by particles in a colloid

Question 13

How many grams of FeCl$$_3$$ are needed to prepare 2.00 L of a 3.00 M solution? (Molar mass of FeCl$$_3 = 162.2 g/$$mol)

Accepted Answer

$$\displaystyle 324\ \mathrm{g}$$

Question 14

Which of the following is true about the dissolving process of ionic compounds in water?

Accepted Answer

Polar water molecules surround and separate the ions of the ionic compound.

Question 15

What is the molarity of a solution produced when 14.1 g of NH$$_3 is $$dissolved in enough water to make 0.100 L of solution? (Molar mass of NH$$_3 = 17.03 g/$$mol)

Accepted Answer

$$\displaystyle 8.28\ \mathrm{M}$$

Question 16

Which of the following best describes a colloid?

Accepted Answer

A homogeneous mixture with particles that do not settle out

Question 17

To prepare 10.5 L of a 2.50 M KOH solution, how many grams of KOH must be used? (Molar mass of KOH = 56.11 g/mol)

Accepted Answer

$$\displaystyle 1,470\ \mathrm{g}$$

Question 18

Which of the following is an example of a gas dissolved in a liquid?

Accepted Answer

Soda (carbon dioxide in water)

Question 19

Which of the following best explains why you must be careful using electricity near a swimming pool?

Accepted Answer

Chlorinated water is a solution that can conduct electric current.

Solutions and Their Properties: Structure, Types, and Calculations

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