Deck 13: Solutions

Question 1

In a solution, solutes ________.

A) must be liquids
B) can be liquids or gases
C) cannot be solids
D) can be solids, liquids or gases

Answer 1

can be solids, liquids or gases

Question 2

A solution is always characterized by each of the following except one. The exception is ________.

A) homogeneity
B) variable composition
C) absence of settling
D) liquid state

Answer 2

liquid state

Question 3

In a mixture of 66 mL water, 75 mL ethyl alcohol, and 59 mL of acetone, the solvent is ________.

A) ethyl alcohol
B) water
C) acetone
D) acetone and ethyl alcohol

Answer 3

ethyl alcohol

Question 4

A crystal of solid NaCl is placed into an aqueous NaCl solution. No precipitate forms in the bottom of the container. The final solution ________.

A) is super saturated
B) is unsaturated
C) is slightly saturated
D) might be saturated, or it might be unsaturated

Question 5

A solution in which the rate of crystallization is equal to the rate of dissolution is ________.

A) unsaturated
B) saturated
C) supersaturated
D) dilute

Question 6

Which type of solution is described by the term miscible?

A) liquid/liquid
B) liquid/solid
C) liquid/gas
D) solid/solid

Question 7

Water and methanol are two liquids which dissolve in each other. When the two are mixed they form one layer. The liquids are ________.

A) miscible
B) immiscible
C) unsaturated
D) partially miscible

Question 8

Which of the following interparticle attractions play a part in the formation of a solution?

A) solute-solute
B) solvent-solvent
C) solvent-solute
D) Answers A, B, and C all play a part.

Question 9

The rule "likes dissolve likes" is not adequate for predicting solubilities when the solute is ________.

A) a nonpolar gas
B) an ionic compound
C) a nonpolar liquid
D) a polar gas

Question 10

Which type of compound is likely to dissolve in water?

A) one with hydrogen bonds
B) a salt
C) a highly polar compound
D) All are correct.

Question 11

Salts incorporating all but one of the following ions are usually soluble in water. Which ion is the exception?

A) SO₄^2-
B) C₂H₃O₂^-
C) PO₄^3-
D) K⁺

Question 12

In which of the following pairs of ionic compounds are both chemical species soluble in water?

A) K₂CO₃ and FeCO₃
B) CuS and NaNO₃
C) Be(NO₃)₂ and Be₃(PO₄)₂
D) NH₄F and Sr(OH)₂

Question 13

Which response includes all of the following compounds that are soluble in water, and no others?

A) I, III, and VI
B) II, IV, V, and VII
C) III, IV, V, and VIII
D) I, II, V, and VIII

Question 14

Which of the following percentage concentration units is most frequently used by chemists?

A) % (m/m)
B) % (m/v)
C) % (v/v)
D) % (v/m)

Question 15

If the concentration of a KCl solution is 16% (m/v), then the amount of KCl in 26.0 mL of solution is ________.

A) 61.5 grams
B) 32.6 grams
C) 4.16 grams
D) 9.84 grams

Question 16

What is the concentration in mass-volume percent for 13.9 g CaF₂ in 255 mL of solution?

A) 2.34%
B) 0.160%
C) 0.920%
D) 5.45%

Question 17

What volume of a 8.50% (m/v) solution contains 50.0 grams of glucose?

A) 588 mL
B) 356 mL
C) 279 mL
D) 480 mL

Question 18

What mass of water is needed to prepare 148 grams of 12.0% (m/m) KHCO₃ solution?

A) 17.8 g
B) 9.65 g
C) 130 g
D) 125 g

Question 19

If you had 75.0 mL of a 5.00%(m/v) NaOH solution, how much NaOH does it contain?

A) 5.00 g
B) 3.75 g
C) 6.67 g
D) 15.0 g

Question 20

It is determined that 9.86 x 10^-3 g of a contaminant is present in 4865 g of a particular solution. What is the concentration of the contaminant in ppm (m/m)?

A) 5.73
B) 2.03
C) 3.20
D) 1.00

Question 21

If a solution contains 6.8 ppm (m/v) of a solute, how many grams of that solute would be present in a 25 mL sample of the solution?

A) 170 g
B) 1.7 x 10^-5 g
C) 1.7 x 10^-4 g
D) 0.0017 g

Question 22

In which of the following pairs of concentrations are the two concentrations equivalent to each other?

A) 7 ppm (v/v) and 7000 ppb (v/v)
B) 7 ppb (v/v) and 7000 ppm (v/v)
C) 7% (v/v) and 7000 ppm (v/v)
D) 7% (v/v) and 7000 ppb (v/v)

Question 23

The concentration of Cu²⁺ ions in a river water sample is found to be 3.26 micrograms of Cu²⁺ ions per 0.250 kg of river water. Express the concentration of Cu²⁺ ions in ppb (m/m).

A) 13.0 ppb
B) 26.2 ppb
C) 4.66 ppb
D) 39.7 ppb

Question 24

An aqueous solution contains 38.6 g NaCl per 755 mL of solution. This solution is ________.

A) 1.09 M
B) 2.41 M
C) 0.49 M
D) 0.874 M

Question 25

A 0.360 M solution of KNO₃ (formula mass = 101.09) which contains 125 grams of solute would have a volume of ________.

A) 3430 mL
B) 3600 mL
C) 7500 mL
D) 1250 mL

Question 26

A solution is made by dissolving 2.68 mole of KF in enough water to give a final volume of 1030 mL. What is the molarity of the solution?

A) 0.125 M
B) 0.800 M
C) 2.60 M
D) 1.52 M

Question 27

Molarity could be used as a conversion factor between ________.

A) grams of solute and moles of solvent
B) moles of solute and volume of solution
C) grams of solute and volume of solution
D) moles of solute and kilograms of solute

Question 28

How many grams of H₃PO₄ are needed to make 175 mL of a 0.175 M H₃PO₄ solution?

A) 0.786 g
B) 0.312 g
C) 5.02 g
D) 3.00 g

Question 29

What is the molarity of KCl in sea water if sea water is 12.5% (m/m) and the density of sea water is 1.06 g/mL?

A) 2.69 M
B) 0.854 M
C) 1.78 M
D) 17.1 M

Question 30

What mass of KOH is needed to produce 22.0 mL of 0.576 M solution?

A) 0.423 g
B) 1.39 g
C) 0.711 g
D) 2.64 g

Question 31

If 29.4 g of LiOH is dissolved in enough water to make 985 mL of solution, what is the molarity of the LiOH solution?

A) 0.986 M
B) 0.478 M
C) 1.25 M
D) 2.19 M

Question 32

What mass of CaCl₂ is required to prepare 3.20 L of 0.850 M CaCl₂ solution?

A) 302 g
B) 139 g
C) 101 g
D) 78.9 g

Question 33

How many grams of FeSO₄ are present in a 20.0 mL sample of a 0.500 M solution?

A) 65.8 g
B) 6.08 g
C) 1.52 g
D) 0.760 g

Question 34

The density of a NaNO₃ solution is 1.24 g/mL. What is the molarity of a 25.0% (m/m) NaNO₃ solution?

A) 3.65 M
B) 0.960 M
C) 8.23 M
D) 15.1 M

Question 35

What is the molarity of a solution made by dissolving 25.0 g of NaCl in enough water to make 625 mL of solution?

A) 0.308 M
B) 0.526 M
C) 0.479 M
D) 0.684 M

Question 36

Which of the following gives the correct defining expression for molality?

A) moles of solute/liter of solution
B) moles of solute/kilogram of solvent
C) moles of solute/liter of solute
D) moles of solute/liter of solvent

Question 37

When a 20.0 mL sample of a CuSO₄ solution was dried, 0.967 g of copper (II) sulfate was left behind. What was the molarity of the original solution?

A) 0.433 M
B) 0.303 M
C) 0.0484 M
D) 0.0207 M

Question 38

The molality concentration unit is defined in terms of a fixed ________.

A) mass of solution
B) volume of solution
C) mass of solvent
D) volume of solvent

Question 39

What is the molality of a solution made by dissolving 16.84 g of NaF in 325 g of H₂O?

A) 0.265 m
B) 0.0308 m
C) 1.23 m
D) 0.492 m

Question 40

What is the molality of KBr in a solution made by dissolving 2.21 g of KBr in 897 g of water?

A) 2.46 m
B) 0.0167 m
C) 0.0207 m
D) 2.07 x 10^-5 m

Question 41

Calculate the number of grams of HNO₃ which must be added to 31.5 g of H₂O to prepare a 0.95 m solution.

A) 1.26 g
B) 2.31 g
C) 1.89 g
D) 10.3 g

Question 42

Calculate the molality of a solution prepared by dissolving 12.1 g of CH₃OH in 475 g of water.

A) 1.37 m
B) 0.795 m
C) 2.40 m
D) 0.458 m

Question 43

A student wishes to prepare 65.0 mL of 0.875 M HCl from 12.0 M HCl. What volume of the 12.0 M HCl should he/she start with?

A) 4.74 mL
B) 9.28 mL
C) 4.65 mL
D) 18.2 mL

Question 44

If 250 mL of 4.00 M CaBr₂ is diluted to 1.60 L, the resulting solution contains ________.

A) 0.400 mole of CaBr₂
B) 1.00 mole of CaBr₂
C) 2.40 moles of CaBr₂
D) 0.0500 moles of CaBr₂

Question 45

If 850 mL of 1.36 M NH₄Cl is diluted to 4.50 L, the concentration of the resulting solution is ________.

A) 0.257 M
B) 4.00 M
C) 0.200 M
D) 0.0356 M

Question 46

To prepare 25 mL of 0.25 M MgCl₂ solution from a 0.75 M MgCl₂ stock solution, you should mix ________.

A) 12 mL of stock solution mixed with enough water to make 25 mL
B) 17 mL of stock solution mixed with enough water to make 25 mL
C) 8.3 mL of stock solution mixed with enough water to make 25 mL
D) 9.6 mL of stock solution mixed with enough water to make 25 mL

Question 47

What volume of 8.25 M HCl must be diluted to prepare 2.40 L of 0.500 M HCl?

A) 39.6 L
B) 438 mL
C) 145 mL
D) 0.256 L

Question 48

If 50.0 mL of a 6.0 M HCl is diluted to 200. mL, what will be the new concentration of the solution?

A) 1.5 M
B) 24. M
C) 2.1 M
D) 3.0 M

Question 49

What volume, in liters, of a 0.150 M Ba(OH)₂ solution is needed to react completely with 0.200 L of a 0.300 M HNO₃ solution according to the equation:
Ba(OH)₂ + 2HNO₃ $\rightarrow$ Ba(NO₃)₂ + 2H₂O

A) 0.150 L Ba(OH)₂
B) 0.200 L Ba(OH)₂
C) 0.600 L Ba(OH)₂
D) 0.250 L Ba(OH)₂

Question 50

How many grams of KCl (molar mass = 74.55 g) will be produced from the reaction of 50.0 mL of 0.300 M KOH with excess HCl?
KOH (aq) + HCl (aq) $\rightarrow$ KCl (aq) + HCl (l)

A) 1.12 g
B) 4.65 g
C) 6.98 g
D) 9.31 g

Question 51

Calculate the grams of magnesium needed to completely react with 100.0 mL of 0.557 M HClO₄ solution, given the following reaction:
Mg (s) + 2 HClO₄ (aq) $\rightarrow$ Mg(ClO₄)₂ (aq) + H₂ (g)

A) 1350 g
B) 675 g
C) 0.677 g
D) 2.70 g

Question 52

Calculate the volume, in mL, of a 1.22 M Na₂S solution needed to react with 2.75 g of AlBr₃ in the following equation:
3 Na₂S (aq) + 2 AlBr₃ (aq) $\rightarrow$ Al₂S₃ (s) + 6 NaBr (aq)

A) 0.0254 mL
B) 8.45 mL
C) 12.7 mL
D) 0.0127 mL

Question 53

How many grams of solid KCl are needed to prepare 250. mL of a 0.125 M solution?

A) 9.32 g
B) 31.3 g
C) 15.6 g
D) 2.33 g

Question 54

What volume, in mL, of 0.300 M Cu(OH)₂ is needed to react with 500. mL of 0.100 M H₃PO₄?
3 Cu(OH)₂ (aq) + 2H₃PO₄ (aq) $\rightarrow$ Cu ₃(PO₄)₂ (s) + 6 H₂O (l)

A) 250 mL
B) 167 mL
C) 83.3 mL
D) 60.0 mL

Question 55

15.00 mL of 0.425 M H₂SO₄ is required to completely neutralize 23.9 mL of KOH. What is the molarity of the KOH?
2 KOH(aq) + H₂SO₄(aq) $\rightarrow$ K₂SO₄(aq) + 2 H₂O (l)

A) 1.75 M
B) 0.988 M
C) 0.614 M
D) 0.533 M

Question 56

16.24 mL of 0.325 M Ba(OH)₂ solution is required to completely neutralize 26.58 mL of HNO₃ solution. What is the molarity of the nitric acid solution?
Ba(OH)₂ (aq) + 2 HNO₃ (aq) $\rightarrow$ Ba(NO₃)₂ (aq) + 2 H₂O (l)

A) 0.0993 M
B) 0.432 M
C) 0.397 M
D) 0.741 M

Question 57

Predict the solubility of each solute-solvent combination by writing the word soluble or insoluble in the blank space.

-NO₂ (a polar gas) in H₂O ____________________

A) soluble
B) insoluble

Question 58

Predict the solubility of each solute-solvent combination by writing the word soluble or insoluble in the blank space.

-KCl in CCl₄ (a liquid) ____________________

A) soluble
B) insoluble

Question 59

Predict the solubility of each solute-solvent combination by writing the word soluble or insoluble in the blank space.

-BaSO₄ in H₂O ____________________

A) soluble
B) insoluble

Question 60

Predict the solubility of each solute-solvent combination by writing the word soluble or insoluble in the blank space.

-LiF in H₂O ____________________

A) soluble
B) insoluble

Question 61

Predict the solubility of each solute-solvent combination by writing the word soluble or insoluble in the blank space.

-C₈H₁₈ (a nonpolar liquid) in CCl₄ ____________________

A) soluble
B) insoluble

Question 62

Saline I.V. solution is 0.92% (m/v) NaCl solution. A patient is to receive 0.50 L of saline solution. What mass of NaCl is the patient to receive?

Question 63

A concentration of the pollutant nitrogen dioxide in air of 3.0 ppm (m/v) may be lethal to humans. Will air that contains 1.9 x 10⁻³ g of NO₂ per liter be lethal to humans?

Question 64

What volume, in milliliters, of 0.655 M LiCl solution contains 19.6 g of LiCl?