Chemistry Chapter 12

Front 1

The O-H bond in water is polar because

Back 1

B) oxygen is much more electronegative than hydrogen

Front 2

In a solution, the solvent

Back 2

C) can be a solid, liquid, or gas.

Front 3

Which of the following molecules can form hydrogen bonds?

Back 3

C) H2O

Front 4

A solution is prepared by dissolving 2 g of KCl in 100 g of H2O. In this solution, H2O is the ________.

Back 4

B) solvent

Front 5

Oil does not dissolve in water because

Back 5

oil is nonpolar.

Front 6

When KCl dissolves in water

Back 6

D) the K+ ions are attracted to the partially negative oxygen atoms of the water molecules

Front 7

Water is a polar solvent and hexane (C6H14) is a nonpolar solvent. Which of the following correctly describes the solubility of the solute?

Back 7

C) NaHCO3, soluble in water

Front 8

In water, a substance that ionizes completely in solution is called a ________.

Back 8

E) strong electrolyte

Front 9

When some of the sugar added to iced tea remains undissolved at the bottom of the glass, the solution is ________.

Back 9

D) saturated

Front 10

The solubility of KI is 50. g in 100. g of H2O at 20 °C. If 110. grams of KI are added to 200. grams of H2O,

Back 10

D) a saturated solution will form.

Front 11

An increase in the temperature of a solution usually

Back 11

C) increases the solubility of a solid solute in the solution.

Front 12

When the weak electrolyte HF is dissolved in water, the solution contains ________.

Back 12

D) mostly HF molecules and a few H+ and F- ions

Front 13

When the nonelectrolyte glucose is dissolved in water, the solution contains ________.

Back 13

A) all glucose molecules

Front 14

The mass/mass percent concentration refers to the number of grams of solute in ________.

Back 14

D) 100 g of solution

Front 15

What is the concentration, in m/m %, of a solution prepared from 50.0 g NaCl and 150.0 g of water?

Back 15

D) 25.0%

Front 16

Rubbing alcohol is 70.0% isopropyl alcohol by volume. How many mL of isopropyl alcohol are in a full 1 pint (473 mL) container?

Back 16

E) 331 mL

Front 17

What is the concentration, in m/m %, of a solution prepared from 500. g NaCl and 2.50 kg of water?

Back 17

C) 16.7%

Front 18

How many grams of glucose are needed to prepare 400. g of a 2.00% (m/m) glucose solution?

Back 18

C) 8.00 g

Front 19

What mass of a 15.0% (m/m) NaOH solution contains 125 g NaOH?

Back 19

E) 833 g

Front 20

What is the molarity of a solution that contains 2.35 g of NH3 in 0.0500 L of solution?

Back 20

B) 2.76 M

Front 21

The molarity (M) of a solution refers to

Back 21

A) moles of solute/L of solution

Front 22

What is the molarity of a solution containing 5.00 moles of KCl in 2.00 L of solution?

Back 22

A) 2.50 M

Front 23

What is the molarity of a solution which contains 58.4 g of sodium chloride dissolved in
500. mL of solution?

Back 23

D) 2.00 M

Front 24

How many moles of CaCl2 are in 250. mL of a 3.00 M of CaCl2 solution?

Back 24

D) 0.750 mol

Front 25

How many mL of 1.15 M KOH solution are needed to provide 0.665 mol of KOH?

Back 25

C) 578 mL

Front 26

During the process of diluting a solution to a lower concentration,

Back 26

A) the amount of solute does not change.

Front 27

According to Henry's law, the solubility of a gas in a liquid

Back 27

B) increases as the gas pressure above the liquid increases.

Front 28

When sucrose, C12H22O11, is dissolved in water, the sucrose is classified as the ________.

Back 28

A) solute

Front 29

Vinegar is a solution of acetic acid (melting point 16.5 °C) in water. At room temperature
(25 °C), vinegar is an example of a ________ solution

Back 29

A) liquid-liquid

Front 30

Which of the following statements is not true about water?

Back 30

E) The water molecule is linear.

Front 31

A solution containing a large concentration of dissolved ions can be classified as a(n) ________.

Back 31

C) electrolyte

Front 32

A solution of an electrolyte in water will

Back 32

A) carry an electric current

Front 33

At 26 °C, the solubility of sodium chloride is 36 g/100 mL of solution. How would you describe a solution of 10 g of sodium chloride in 100 mL of solution at room temperature?

Back 33

D) unsaturated

Front 34

The solubility of carbon dioxide in soda water

Back 34

D) is lower as the temperature increases.

Front 35

Ammonium chloride, NH4Cl, is ________ in water.

Back 35

B) soluble

Front 36

A solid that comes out of a solution as its solubility is exceeded is called a ________.

Back 36

D) precipitate

Front 37

In the reaction of silver nitrate and sodium chloride to produce solid silver chloride, sodium ions and nitrate ions are ________.

Back 37

A) spectator ions

Front 38

Calcium chloride reacts with sodium hydroxide to form solid calcium hydroxide, Ca(OH)2. The balanced net ionic equation is

Back 38

C) Ca+2(aq) + 2OH-(aq) → Ca(OH)2 (s).

Front 39

What is the concentration (m/m %) of a solution of 10.0 g of sodium chloride in 100. g of solution?

Back 39

E) 10.0%

Front 40

25.0 mL of alcohol is dissolved in water and the solution is diluted to a total final volume of 125 mL. What is the final concentration of ethanol?

Back 40

B) 20.0% (v/v)

Front 41

A solution of artificial tears is 0.090% (m/m) sodium chloride. How many grams of sodium chloride are contained in 1.00 g of this solution?

Back 41

A) 9.0 × 10-4 g

Front 42

Calculate the molarity of 60.05 g of acetic acid, HC2H3O2, dissolved in 0.250 L of solution.

Back 42

B) 4.00 M

Front 43

What is the molarity of the solution obtained when 0.100 mol of copper sulfate are dissolved in

Back 43

A) 0.500 M

Front 44

How many mL of 1.24 M H2SO4 reacts with 1.26 g of Al?

Back 44

B) 56.5 mL