Deck 12: Solutions

Question 1

A solution is made by mixing 50 grams of CHCl₃ (liquid) with 10 grams of CH₂Cl₂ (liquid). Which of the two is considered the solute and why?

A) CHCl₃ is the solute because it is in the greater amount.
B) CHCl₃ is the solute because it is in the lesser amount.
C) CH₂Cl₂ is the solute because it is in the greater amount.
D) CH₂Cl₂ is the solute because it is in the lesser amount.
E) Neither is the solute because they are both liquids at ambient conditions and therefore are solvents.

Answer 1

CH₂Cl₂ is the solute because it is in the lesser amount.

Question 2

How many milliliters of water must be added to 75.0 mL of 0.150 M AgNO₃ in order to prepare a 0.100 M solution?
(Assume volumes are additive.)

A) 25.0 mL of H₂O
B) 38.0 mL of H₂O
C) 50.0 mL of H₂O
D) 113 mL of H₂O
E) 188 mL of H₂O

Answer 2

38.0 mL of H₂O

Question 3

What mass of KCl is required to prepare 500 mL of a 2.50 M aqueous solution of KCl?
MM(KCl) = 74.55 g/mol.

A) 0.0168 g KCl
B) 0.0671 g KCl
C) 14.9 g KCl
D) 93.2 g KCl
E) 373 g KCl

Answer 3

93.2 g KCl

Question 4

Three hundred milliliters (300 mL) of 2.50 M sugar solution is diluted tO₆00 mL by the addition of pure water. Which of these statements about the solution is correct?

A) The moles of water remain the same.
B) The moles of sugar decrease.
C) The concentration of sugar increases tO₅ .0 M.
D) The moles of sugar remain constant.
E) All of these statements are incorrect.

Question 5

Calculate the molarity of a solution prepared by dissolving 43.2 grams of pentane (C₅H₁₂, molar mass = 72.15 g/mol) in enough carbon tetrachloride (CCl₄, molar mass = 153.8 g/mol) to take 400 mL of solution.

A) 10.8 M
B) 0.600 M
C) 6.01 M
D) 4.17 M
E) 1.50 M

Question 6

The molarity and molality of a solution:

A) may never be equal.
B) are equal for all solutions.
C) both express the quantity of solute in moles.
D) are equal for all solutions having water as the solvent.
E) are equal for all concentrated solutions.

Question 7

What is the definition for mass percent solute ?

A) (grams of solute / grams of solvent)×100%
B) (grams of solvent / grams of solute)×100%
C) (moles of solute / moles of solvent)×100%
D) (grams of solute / grams of solution)×100%
E) (moles of solution / moles of solute)×100%

Question 8

How many grams of silver nitrate (AgNO₃) are present in 255 mL of 2.50 M silver nitrate solution?
MM(AgNO₃) = 169.87 g/mol

A) 5.77×10 ^{- 2} g AgNO₃
B) 17.3 g AgNO₃
C) 108 g AgNO₃
D) 266 g AgNO₃
E) 1.67×10³ g AgNO₃

Question 9

A solution is made by mixing 25 grams of ethanol witH₅ grams of isopropanol. Which of the two is considered the solvent and why?

A) Ethanol is the solvent because it is in the greater amount.
B) Ethanol is the solvent because it is in the lesser amount.
C) Isopropanol is the solvent because it is in the greater amount.
D) Isopropanol is the solvent because it is in the lesser amount.
E) Both are solvents because they are both liquids at ambient conditions.

Question 10

How many grams of H₂SO₄ are present in 75.0 mL of 12.0 M H₂SO₄?
MM (H₂SO₄) = 98.09 g/mol

A) 1.63 g H₂SO₄
B) 9.18 g H₂SO₄
C) 15.7 g H₂SO₄
D) 88.3 g H₂SO₄
E) 613 g H₂SO₄

Question 11

How many grams of urea [CO(NH₂)₂] would be required to prepare 200 mL of a 5.0×10 ^{- 3} molar solution?

A) 1.0×10 ^{- 3} g
B) 6.0×10 ^{- 2} g
C) 1.5 g
D) 5.0×10 ^{- 3} g
E) 1.7×10 ^{- 5} g

Question 12

Potassium fluoride is used for frosting glass. What is the molarity of a solution prepared by dissolving 78.6 g of KF in enough water to produce 225 mL of solution?
MM(KF) = 58.10 g/mol

A) 0.304 M
B) 0.349 M
C) 1.35 M
D) 3.29 M
E) 6.01 M

Question 13

Which of the following concentration terms below represents moles of solute per kilogram of solvent?

A) Molarity
B) Molality
C) Molar mass
D) Mole fraction
E) Mole percent

Question 14

Calculate the molarity of glucose (C₆H₁₂O₆) in a solution in which 10.0 g of glucose is dissolved in water and diluted to a final volume of 200 mL.

A) 0.278 M
B) 0.0556 M
C) 0.0050 M
D) 90.0 M
E) 50.0 M

Question 15

How many grams of AgNO₃ are present in 50.0 mL of a 12.0 M AgNO₃ solution?
MM(AgNO₃) = 169.88 g/mol

A) 3.53 g of AgNO₃
B) 40.8 g of AgNO₃
C) 102 g of AgNO₃
D) 283 g of AgNO₃
E) 708 g of AgNO₃

Question 16

What is the definition for molarity ?

A) Grams of solute per moles of solute
B) Moles of solute per grams of solution
C) Moles of solute per Liter of solvent
D) Grams of solute per Liter of solution
E) Moles of solute per Liter of solution

Question 17

What is the definition for molality ?

A) kilograms of solute/mole of solvent
B) Avogadro's number of atoms, molecules or formula units
C) moles of solute/Liter of solution
D) moles of solute/Kg of solvent
E) moles of solute/Kg of solution

Question 18

How many grams of solute are present in 164.1 mL of 0.207 M calcium acetate, Ca(C₂H₃O₂)₂?
MM[Ca(C₂H₃O₂)₂] = 158.17 g/mol

A) 0.200 g Ca(C₂H₃O₂)₂
B) 0.215 g Ca(C₂H₃O₂)₂
C) 4.66 g Ca(C₂H₃O₂)₂
D) 5.01 g Ca(C₂H₃O₂)₂
E) 5.37 g Ca(C₂H₃O₂)₂

Question 19

How many grams of KBr are required to prepare 1.50 L of 0.257 M aqueous solution?
MM(KBr) = 119.00 g/mol

A) 3.24×10 ^{- 3} g KBr
B) 20.4 g KBr
C) 45.9 g KBr
D) 309 g KBr
E) 695 g KBr

Question 20

What volume in milliliters of a 0.200 M NaCl solution is required to provide 1.00 grams of NaCl?
MM(NaCl) = 58.44 g/mol

A) 3.42 mL
B) 11.7 mL
C) 85.6 mL
D) 292 mL
E) 5000 mL

Question 21

A solution is prepared by mixing 22 g ethylene glycol [C₂H₄(OH)₂] with 108 g of water. What is the mass percent of ethylene glycol in the solution?

A) 20%
B) 17%
C) 22%
D) 83%
E) none of these

Question 22

What is the mole fraction of glycerol for a mixture prepared by mixing 300 grams of glycerol (non-volatile solute) and 505 grams of H₂O?
Molar Mass(glycerol) = 92.09 g/mol and Molar Mass(H₂O) = 18.02 g/mol

A) c _glycerol = 0.104
B) c _glycerol = 0.116
C) c _glycerol = 0.896
D) c _glycerol = 1.12
E) c _glycerol = 8.59

Question 23

How many grams of NaCl are required to prepare 250 mL of 3.60% (m/v) aqueous solution of NaCl?

A) 0.694 g NaCl
B) 1.44 g NaCl
C) 9.00 g NaCl
D) 69.4 g NaCl
E) 900 g NaCl

Question 24

The mass percent of acetone in a solution prepared by mixing 58.1 g acetone (C₃H₆O) and 72.1 g of H₂O is:

A) 44.6%
B) 80.6%
C) 55.4%
D) 13.9%
E) none of these

Question 25

How many grams of Na₂SO₄ are required to make 43.5 mL of a 13.7% (m/v) aqueous solution?

A) 0.168 g Na₂SO₄
B) 5.96 g Na₂SO₄
C) 13.7 g Na₂SO₄
D) 31.5 g Na₂SO₄
E) 318 g Na₂SO₄

Question 26

How many grams of Na₂CO₃ are required to prepare 25.0 mL of a 2.00% (m/v) Na₂CO₃ solution?

A) 0.0800 g Na₂CO₃
B) 0.500 g Na₂CO₃
C) 2.00 g Na₂CO₃
D) 12.5 g Na₂CO₃
E) 50.0 g Na₂CO₃

Question 27

How many grams of glucose (C₆H₁₂O₆) are required to prepare 50.0 mL of 6.30% (m/v) glucose-water solution?

A) 0.0175 g C₆H₁₂O₆
B) 0.126 g C₆H₁₂O₆
C) 3.15 g C₆H₁₂O₆
D) 6.30 g C₆H₁₂O₆
E) 7.94 g C₆H₁₂O₆

Question 28

What is the mole fraction of water for a mixture prepared by mixing 50.0 grams of glycerol (non-volatile solute) and 500 grams of H₂O?
Molar Mass(glycerol) = 92.09 g/mol and Molar Mass(H₂O) = 18.02 g/mol

A) c _water = 0.0192
B) c _water = 0.0361
C) c _water = 0.0909
D) c _water = 0.909
E) c _water = 0.981

Question 29

A solution is prepared by mixing 22 g ethylene glycol [C₂H₄(OH)₂, molar mass = 62 g/mol] with 108 g of water. What is the mole fraction of ethylene glycol in the solution?

A) 0.056
B) 0.17
C) 0.35
D) 6.3
E) none of these

Question 30

What is the mass percentage, %(m/m), of an aqueous solution prepared by dissolving 24.5 g of NaCl in 86.5 g of water?

A) 0.283%
B) 3.53%
C) 22.1%
D) 28.3%
E) 77.9%

Question 31

Calculate the mole fraction of water in a solution made by mixing 1.0 g of water and 2.0 g of ethyl alcohol (C₂H₅OH).

A) 75%
B) 67%
C) 33%
D) 56%
E) none of these

Question 32

A commercial bleaching solution contains 3.62% sodium hypochlorite, NaOCl. What is the mass of NaOCl present in a bottle that contains 4.50×10³ g of bleaching solution?

A) 8.04×10 ^{- 4} g NaOCl
B) 0.0804 g NaOCl
C) 163 g NaOCl
D) 1.24×10³ g NaOCl
E) 1.63×10⁴ g NaOCl

Question 33

What is the mole fraction of glucose in a solution prepared by dissolving 9.01 grams of glucose, C₆H₁₂O₆, in 17.1 grams of water?
Molar Mass(C₆H₁₂O₆) = 180.16 g/mol and Molar Mass(H₂O) = 18.02 g/mol

A) c _glucose = 0.0503
B) c _glucose = 0.345
C) c _glucose = 0.527
D) c _glucose = 0.909
E) c _glucose = 0.950

Question 34

The mole fraction of acetone in a solution prepared by mixing 58.1 g acetone (C₃H₆O) and 72.1 g of H₂O is:

A) 0.200
B) 0.250
C) 0.446
D) 0.806
E) 1.00

Question 35

How many grams of glucose (C₆H₁₂O₆) must be dissolved in 54 g of water to give a solution in which the mole fraction of glucose is 0.50?

A) 180 g
B) 54 g
C) 27 g
D) 5.4×10² g
E) 0.50 g

Question 36

A solution is prepared by mixing 4.00 grams of benzene (molar mass = 78.1 g/mol), 4.00 grams of CCl₄ (molar mass = 153.8 g/mol), and 4.00 grams of C S₂ (molar mass = 76.1 g/mol). The mole fraction of benzene in this solution is:

A) 0.051
B) 0.200
C) 0.333
D) 0.395
E) 0.605

Question 37

What is the mole fraction of lactose in a mixture prepared by adding 15.0 g of lactose (C₁₂H₂₂O₁₁) to 100.0 g of water?

A) c _lactose = 7.83×10 ^{- 3}
B) c _lactose = 7.89×10 ^{- 3}
C) c _lactose = 0.130
D) c _lactose = 0.150
E) c _lactose = 0.992

Question 38

Calculate the mole fraction of water in a solution made by mixing 1.0 g of water and 2.0 g of ethyl alcohol (C₂H₅OH).

A) 0.33
B) 0.25
C) 0.56
D) 0.78
E) 0.056

Question 39

What is the mass percent , %(m/m), of an aqueous solution prepared by dissolving 12.5 g of KNO₃ in 125 g of water?

A) 0.0909%
B) 0.100%
C) 9.09%
D) 10.0%
E) 90.9%

Question 40

A solution is made by dissolving 0.750 moles of isopropanol (C₃H₇OH) in 0.250 moles of water. What is the mass percentage of isopropanol in this mixture?
MM(C₃H₇OH) = 60.10 g/mol and Molar Mass(H₂O) = 18.02 g/mol

A) 5.51% (m/m)
B) 9.1% (m/m)
C) 75.0% (m/m)
D) 76.9% (m/m)
E) 90.9% (m/m)

Question 41

How many grams of NH₃ are present in 2.50 L of 3.00 M NH₃ solution?
MM(NH₃) = 17.03 g/mol

A) 0.0705 g NH₃
B) 7.50 g NH₃
C) 14.2 g NH₃
D) 20.4 g NH₃
E) 128 g NH₃

Question 42

A solution of ethanol (C₂H₅OH) in water is 15.0% ethanol by weight. The molality of this solution is:

A) 15.0 m
B) 3.83 m
C) 3.25 m
D) 1.77 m
E) none of these

Question 43

What is the molality of a solution prepared by mixing 22 g of ethylene glycol (molar mass = 62 g/mol) with 108 g of water?

A) 0.17 m
B) 0.20 m
C) 3.3 m
D) 12. m
E) none of these

Question 44

How many moles of sucrose, C₁₂H₂₂O₁₁, is present in 80.0 grams of an aqueous solution that is 3.50% sucrose by mass?
MM(C₁₂H₂₂O₁₁) = 342.30 g/mol

A) 8.18×10 ^{- 3} moles
B) 0.150 moles
C) 2.80 moles
D) 122 moles
E) 958 moles

Question 45

What is the molality of a solution prepared by dissolving 76.5 grams of glycine (NH₂CH₂COOH) in 1.280 kg of water?
MM(glycine) = 75.07 g/mol

A) 0.752 m
B) 0.796 m
C) 1.02 m
D) 1.26 m
E) 59.8 m

Question 46

The density of a solution that is 18.0% by mass lead nitrate [Pb(NO₃)₂] is 1.18 g/cm³. Calculate the molarity of the lead nitrate solution.

A) 4.9×10 ^{- 7} M
B) 0.64 M
C) 12.0 M
D) 19.8 M
E) 15.3 M

Question 47

What is the molality of a solution prepared by dissolving 10.5 grams of benzene, C₆H₆, in 18.5 grams of carbon tetrachloride, CCl₄?

A) 0.568 m
B) 1.76 m
C) 4.64 m
D) 7.27 m
E) 11.5 m

Question 48

How many grams of sulfur, S₈ must be dissolved in 100. grams of naphthalene, C₁₀H₈, to make a 0.180 m solution?
Molar Mass(S₈) = 256.48 g/mol

A) 0.0180 g S₈
B) 4.62 g S₈
C) 18.0 g S₈
D) 142 g S₈
E) 4330 g S₈

Question 49

What is the molality of a solution prepared by mixing 11 g of C₂H₅OH (molar mass = 46 g/mol) witH₂ 04 g of water?

A) 1.9 m
B) 1.2 m
C) 3.3 m
D) 0.12 m
E) none of these

Question 50

How many moles of solute are present in 50.0 grams of solution that is 2.50% by mass glucose (C₆H₁₂O₆)?
MM(C₆H₁₂O₆) = 180.16 g/mol

A) 6.94×10 ^{- 3} moles
B) 0.800 moles
C) 1.25 moles
D) 11.1 moles
E) 225 moles

Question 51

A solution contains 1.00 mole of NaCl in 500 g of water. What is the molal concentration of NaCl?

A) 10.5 m
B) 2.00 m
C) 1.00 m
D) 0.0347 m
E) none of these

Question 52

What is the molality of an aqueous 3.0% hydrogen peroxide solution?
(H₂O₂, molar mass = 34.0 g/mol)

A) 0.016 m
B) 0.030 m
C) 0.88 m
D) 0.91 m
E) none of these

Question 53

What mass of CsCl must be added to 0.55 liters of water to produce a 0.430 m solution?
Molar Mass(CsCl) = 168.35 g/mol and Density(H₂O) = 1.00 g/mL

A) 0.237 g CsCl
B) 0.782 g CsCl
C) 39.8 g CsCl
D) 132 g CsCl
E) 215 g CsCl

Question 54

How many grams of LiNO₃ must be added to 235 grams of water to prepare a 40.0% (m/m) solution of LiNO₃?

A) 0.170 g LiNO₃
B) 94.0 g LiNO₃
C) 157 g LiNO₃
D) 353 g LiNO₃
E) 588 g LiNO₃

Question 55

How many grams of water must be added tO₅ 0.0 g of glucose in order to prepare a 5.00% (m/m) glucose solution?

A) 2.5 g of H₂O
B) 2.63 g of H₂O
C) 250 g of H₂O
D) 950 g of H₂O
E) 1000 g of H₂O

Question 56

How many grams of water must be added to 20.0 g of NaOH in order to prepare a 6.75% (m/m) solution?

A) 1.35 g H₂O
B) 1.45 g H₂O
C) 93.25 g H₂O
D) 276 g H₂O
E) 296 g H₂O

Question 57

How many grams of glucose (C₆H₁₂O₆) must be dissolved in 750 g of ethanol (C₂H₅OH) to prepare a 0.545 m solution?
MM(C₆H₁₂O₆) = 180.15 g/mol

A) 2.27×10 ^{- 3} g glucose
B) 73.6 g glucose
C) 131 g glucose
D) 248 g glucose
E) 441 g glucose

Question 58

What is the molality of a solution that contains 9.00 g of ethylene glycol (C₂H₆O₂) in 100 g of water?

A) 1.45 m
B) 1.61 m
C) 9.00 m
D) cannot be calculated
E) none of these

Question 59

How many grams of NaCl must be dissolved in 500 g of H₂O to prepare a 0.750 m solution?
Molar Mass(NaCl) = 58.44 g/mol

A) 6.42×10 ^{- 3} g NaCl
B) 0.156 g NaCl
C) 21.9 g NaCl
D) 39.0 g NaCl
E) 87.7 g NaCl

Question 60

How many grams of glucose must be added to 275 g of water in order to prepare a 31.0% aqueous glucose solution?

A) 7.78 g glucose
B) 85.3 g glucose
C) 124 g glucose
D) 612 g glucose
E) 887 g glucose

Question 61

A research worker has only 300 g of a valuable solvent and wishes to use all of it to make up a 10.0 mass percent solution of solute A. How many grams of A should be weighed out?

A) 30.0 g
B) 22.2 g
C) 33.3 g
D) 10.0 g
E) cannot calculate without knowing molar masses

Question 62

An aqueous solution of hydrochloric acid contains 36.0% (m/m). What is the molality of this same solution?
MM(HCl) = 36.46 g/mol and MM(H₂O) = 18.015 g/mol

A) 0.217 m
B) 0.563 m
C) 9.87 m
D) 15.4 m
E) 98.7 m

Question 63

Concentrated red fuming Nitric acid, HNO₃, is 90.0% (m/m). What is this solution's Molar concentration if its density is 1.490 g/mL?
MM(HNO₃) = 63.01 g/mol

A) 1.43 M
B) 2.36 M
C) 9.59 M
D) 14.3 M
E) 21.3 M

Question 64

An aqueous solution of concentrated glacial acetic acid, HC₂H₃O₂, has a mole fraction of 0.993. What is this solution's Molar concentration if its density is 1.049 g/mL?
Molar Mass(HC₂H₃O₂) = 60.05 g/mol and Molar Mass(H₂O) = 18.02 g/mol

A) 1.05 M
B) 6.31 M
C) 15.8 M
D) 16.6 M
E) 17.4 M

Question 65

What is the mole fraction of NH₃ for a 5.00% (m/m) aqueous solution of NH₃?

A) c _NH3 = 0.0527
B) c _NH3 = 0.190
C) c _NH3 = 0.294
D) c _NH3 = 0.810
E) c _NH3 = 0.947

Question 66

Calculate the mole fraction of ethylene glycol (C₂H₆O₂) in a solution that is 85% by mass ethylene glycol in water.

A) 1.4
B) 0.85
C) 0.18
D) 0.38
E) 0.62

Question 67

Caffeine (C₈H₁₀N₄O₂) is a stimulant found in coffee and tea. What is the mass percent of caffeine, %(m/m), for a solution of caffeine dissolved in chloroform (CHCl₃) that has a concentration of 0.0890 m ?
Molar Mass(C₈H₁₀N₄O₂) = 194.19 g/mol

A) 1.05%
B) 1.70%
C) 8.9%
D) 16.2%
E) 68.6%

Question 68

A 2.90 m aqueous solution of acetic acid, C₂H₄O₂ (60.0 g/mol), has a density of 1.020 g/mL. Calculate the molarity of the solution.

A) 2.90 M
B) 2.42 M
C) 2.96 M
D) 2.84 M
E) 2.52 M

Question 69

Commercial concentrated ammonium hydroxide is 28.0% (m/m) NH₃ and has a density of 0.890 g/mL. What is the molarity of a concentrated solution of ammonium hydroxide?
MW(NH₃) = 17.03 g/mol

A) 5.4 M
B) 14.6 M
C) 16.4 M
D) 18.5 M
E) 22.8 M

Question 70

A 2.20 molar solution of acetic acid (molar mass = 60.05 g/mol) has a density of 1.0178 g/mL. What is the molality of the solution?

A) 2.16 m
B) 2.20 m
C) 2.23 m
D) 2.48 m
E) none of these

Question 71

What is the molality of a 5.00% aqueous solution of NH₃?
MM(NH₃) = 17.03 g/mol

A) 1.12 m
B) 2.94 m
C) 3.09 m
D) 35.9 m
E) 52.6 m

Question 72

Glacial acetic acid, HC₂H₃O₂, is 99.8% (m/m). What is this solution's Molar concentration if its density is 1.049 g/mL?
MM(HC₂H₃O₂) = 60.05 g/mol

A) 1.05 M
B) 6.31 M
C) 15.8 M
D) 16.6 M
E) 17.4 M

Question 73

A 1.14 molar solution of ammonium chloride (molar mass = 53.50 g/mol) has a density of 1.019 g/mL. What is the molality of the solution?

A) 1.12 m
B) 1.16 m
C) 1.19 m
D) 1.24 m
E) none of these

Question 74

A concentrated reagent is sold as a solution that is 60.0 mass % solute. If the molar mass of the solute is 120 g/mol and the density of this solution is 1.70 g/mL, what is the molarity of the solution?

A) 18.0 M
B) 23.6 M
C) 32.5 M
D) 5.35 M
E) 8.50 M

Question 75

The molality of an unknown aqueous solution was found to be 3.50 m . What is the mole fraction of water (molar mass = 18.0 g/mol) in this solution?

A) 0.059
B) 0.941
C) 0.778
D) 0.222
E) cannot be determined

Question 76

What is the Molarity of a 5.00% (m/m) aqueous NH₃ solution?
(Density of solution = 0.9651 g/mL)

A) 2.83 M
B) 2.94 M
C) 3.09 M
D) 3.20 M
E) 48.3 M

Question 77

A 3.60 m solution of KBr (molar mass = 119 g/mol) in water has a density of 1.26 g/mL. The molarity of this solution is:

A) 3.60 M
B) 2.86 M
C) 3.18 M
D) 4.09 M
E) 2.51 M

Question 78

A 3.38 molar solution of cesium chloride (molar mass = 168.4 g/mol) has a density of 1.423 g/mL. What is the molality of the solution?

A) 4.81 m
B) 3.96 m
C) 3.38 m
D) 2.38 m
E) none of these

Question 79

What is the molality of a 10.0% aqueous solution of NH₃?
MM(NH₃) = 17.03 g/mol

A) 1.11 m
B) 1.70 m
C) 1.89 m
D) 5.87 m
E) 6.52 m

Question 80

A solution of 3.0 g of citric acid (C₆H₈O₇) dissolved in 70.0 g of water was found to have a density of 1.13 g/mL. The molarity of the solution was:

A) 1.81 M
B) 0.16 M
C) 11 M
D) 88 M
E) 0.24 M