Chemistry Chapter 12 Bimodel Questions

Front 1

Acetic acid can be classified as a(n) ________.

Back 1

C) weak electrolyte

Front 2

The molarity of a solution of 5.00 g of KCl in 150. mL of solution is ________.

Back 2

C) 0.447 M

Front 3

How many grams of sodium chloride are required to make 2.00 L of a solution with a concentration of 0.100 M?

Back 3

D) 11.7 g

Front 4

When 25.0 g of NaCl is added to 175 g of water, the m/m % NaCl is ________.

Back 4

E) 12.5%

Front 5

How many grams of sulfuric acid, H2SO4, are needed to make 250. mL of a 1.22 M solution?

Back 5

A) 29.9 g

Front 6

What volume of a 2.00 M solution of sulfuric acid is needed to produce 0.0500 mol of sulfuric acid?

Back 6

B) 0.0250 L

Front 7

a solution that contains the highest amount of solute that dissolves at a given temperature

Back 7

L) saturated

Front 8

the major attraction between water molecules

Back 8

C) hydrogen bonding

Front 9

a solution in which more solute can be dissolved

Back 9

H) unsaturated

Front 10

a substance that does not form ions in solution

Back 10

J) nonelectrolyte

Front 11

a substance that does not form ions in solution

Back 11

J) nonelectrolyte

Front 12

a substance that ionizes completely in solution

Back 12

B) strong electrolyte

Front 13

one substance dissolved in another of significantly higher concentration

Back 13

G) solute

Front 14

the component of a solution present in greatest amount

Back 14

E) solvent

Front 15

the separation of a solute into ions when dissolved in water

Back 15

F) dissociation

Front 16

an equation for a reaction that only shows those species undergoing chemical change

Back 16

D) net ionic equation

Front 17

The molarity of a solution is the mass of solute divided by the solution volume.

Back 17

FALSE

Front 18

) The m/m % concentration of a solution is the mass of the solution divided by its volume multiplied by 100.

Back 18

FALSE

Front 19

The m/m % concentration of a solution is the mass of the solute divided by the solution mass multiplied by 100.

Back 19

TRUE

Front 20

The m/m % concentration of a solution is the mass of the solvent divided by its volume multiplied by 100.

Back 20

FALSE

Front 21

A solution with 58.5 g sodium chloride dissolved in 500.0 mL of water is 2.00 molar.

Back 21

TRUE

Front 22

Hydrochloric acid is a strong electrolyte.

Back 22

TRUE

Front 23

Carbon tetrachloride, CCl4, is soluble in water.

Back 23

FALSE

Front 24

Glucose is a nonelectrolyte

Back 24

TRUE

Front 25

For most solids, solubility decreases as the temperature of the solution increases

Back 25

FALSE

Front 26

The solubility of a gas in water decreases as the temperature increases

Back 26

TRUE

Front 27

The higher the pressure of a gas above a liquid in a closed container, the greater the solubility of the gas.

Back 27

TRUE

Front 28

A solution of a nonelectrolyte contains only ions

Back 28

FALSE

Front 29

An aqueous solution of NaCl has a higher freezing point than pure water

Back 29

FALSE

Front 30

19) If water is added to 100. mL of a 6.00 M CaCl2 solution until the volume is 200. mL, the new molarity is 3.00 M.

Back 30

TRUE

Front 31

The number of moles of a compound dissolved in one liter of a solution is called the ________.

Back 31

: molarity

Front 32

A substance that carries an electric current when dissolved in water is called a(n) ________.

Back 32

electrolyte

Front 33

A substance that produces only a small number of ions in solution is known as a ________ electrolyte.

Back 33

weak

Front 34

Sodium hydroxide has a molar mass of 40.0 g/mole. How many grams of sodium hydroxide are needed to make 500.0 mL of a 1.00 molar solution?

Back 34

20.0 g

Front 35

Sodium chloride has a molar mass of 58.4 g/mole. How many grams of sodium chloride are needed to make 500. mL of a 0.250 molar solution?

Back 35

7.30 g

Front 36

What mass of barium sulfate will be formed from 10.0 mL of 0.400 M H2SO4 ?

BaCl2 + H2SO4 → BaSO4 + 2HCl

Back 36

0.934 g

Front 37

student has available 1.00 L of a 5.00 M solution of sodium hydroxide. The student needs of sodium hydroxide for a reaction. How many mL of the concentrated solution should the student use?

Back 37

10.0 mL

Front 38

How many moles of lithium bromide are present in 25.0 mL of a 0.100 M solution?

Back 38

: 2.50 × 10-3 moles

Front 39

How many grams of lithium bromide are present in 25.0 mL of a 0.100 M solution?

Back 39

0.217 g

Front 40

If 4.55 g of NaCl is added to water to make 350. mL, what is the molarity of the solution?

Back 40

: 0.222 M

Front 41

) If water is added to 50.0 mL of 1.20 M KCl until the total volume is 150. mL, what is the molarity of the dilute solution?

Back 41

: 0.400 M