Deck 11: Solutions

Question 1

Solutions have a higher boiling point than pure solvents.

Answer 1

True

Question 2

Solutions exist in all phases of matter.

Answer 2

True

Question 3

Solutions have a lower vapor pressure than the pure solvent.

Answer 3

True

Question 4

The freezing point of a 0.5 m solution of NaCl is water is less than 0°C.

Question 5

CH₃OH is not soluble in water

Question 6

Solutions have a higher freezing point than their pure solvents.

Question 7

A solution is made by mixing 2.00 mol of solute and 15.0 mol of solvent. The mole fraction of the solute is 0.133

Question 8

Molarity of a solution is the number of moles of solute divided by the milliliters of the solution.

Question 9

NaOH will be more soluble in CCl₄ than H₂O.

Question 10

The boiling point of a 5.00 m solution of C₆H₄Cl₂ in CCl₄ is 101.6°C. Assume that C₆H₄Cl₂ is not volatile and K_b = 4.95°C/m.

Question 11

The freezing point of a 1.9 m solution of NaCl in H₂O is -3.5°C if K_f = 1.86°C/m.

Question 12

Molality refers to the number of moles of solute per gram of solvent.

Question 13

Which of the following terms refer to the major component of a solution?

A) solute
B) solvent
C) precipitate
D) stream
E) pour out

Question 14

The van't Hoff factor for CaCO₃ is 2.

Question 15

The van't Hoff factor for CCl₄ is 5.

Question 16

For ionic solutions, the total ion concentration is the sum of the individual ion concentrations.

Question 17

In both dilution and concentration, the amount of solute stays the same.

Question 18

The molarity of a solution is 25 M if 5.0 moles of the solute is present in 5.0. liters of the solution.

Question 19

Osmotic pressure is the tendency of a solution to pass solution through a semipermeable membrane due to concentration differences.

Question 20

If 25.0 mL of a 1.0 M solution is diluted to 50.0 mL, the concentration becomes 0.50 M.

Question 21

What mass of CaCl₂ is needed to produce 15.0 liters of 1.60 M solution of CaCl₂? (Molar mass of CaCl₂ = 111 g)

A) 2.40 kg
B) 2.66 kg
C) 1,040 g
D) 24.0 g
E) 2.08 kg

Question 22

The process of adding solvent to a solution is called _____.

A) concentration
B) saturation
C) precipitation
D) ionization
E) dilution

Question 23

What is the molarity of a solution if 15 g NaCl is present in 0.50 L of the solution? (Molar mass of NaCl = 58.45 g/mol)

A) 0.26 M
B) 7.5 M
C) 15 M
D) 0.51M
E) 3.0 M

Question 24

What mass of solute is present in 2.050 L of 0.6630 M NaOH? (Molar mass of NaOH = 40.00 g/mol)

A) 82.00 g
B) 54.37 g
C) 66.30 g
D) 13.26 g
E) 10.25 g

Question 25

The concentration of Cl^- ion in a sample of H₂O is 21.0 ppth. What mass of Cl^- ion is present in 0.900 kg of H₂O?

A) 9.45 g
B) 9.45 mg
C) 18.9 mg
D) 21 g
E) 18.9 g

Question 26

What is the molarity of a solution made when 46.76 g of NaCl is dissolved to make 500.0 mL of solution? (Molar mass of NaCl = 58.45 g/mol)

A) 2.500 M
B) 0.002500 M
C) 1.600 M
D) 80.00 M
E) 0.001600 M

Question 27

A solution contains 65.0 g of solvent. How much solute is present in the solution if the mole fraction of the solute is 0.135? (Molar mass of solvent = 18 g/mol; molar mass of solute = 30 g/mol)

A) 0.563 g
B) 4.05 g
C) 3.61 g
D) 53.3 g
E) 16.9 g

Question 28

How many moles of a solute are present in 200.00 mL of a 1.50 M HCl solution?

A) 0.300 mol
B) 3.00 mol
C) 3.00 × 10² mol
D) 75.0 mol
E) 7.50 mol

Question 29

The number of moles of solute divided by the number of liters of solution is _____.

A) concentration
B) molar volume
C) dilution
D) volume deliberation
E) molarity

Question 30

Identify the solvent in which C₂H₅OH will be most soluble.

A) CH₄
B) CCl₄
C) C₆H₆
D) H₂O
E) CO₂

Question 31

_____ refers to a property of solutions related to the fraction that the solute particles occupy in the solution, not their identity.

A) Dissolutive property
B) Static property
C) Dynamic property
D) Kinetic property
E) Colligative property

Question 32

How much NaCl is present in 15 L of a 1.5 M solution of NaCl? (Molar mass of NaCl = 58.5 g/mol)

A) 1.32 kg
B) 22.5 kg
C) 2.25 kg
D) 315 g
E) 565 g

Question 33

How many moles of HCl are present in 1.20 L of a 0.850 M solution?

A) 2.05 mol
B) 1.02 mol
C) 0.980 mol
D) 0.708 mol
E) 1.68 mol

Question 34

If there is 9.00 g of Ag present in 190 g of solution, what is the Ag concentration in parts per thousand?

A) 21.0 ppth
B) 1.70 ppth
C) 47 ppth
D) 47.4 ppth
E) 17.0 ppth

Question 35

A solution is made by dissolving 15.00 g of NaCl in 500.0 g of H₂O. What is the mole fraction of NaCl in the solution?

A) 0.0089
B) 0.2566
C) 0.0092
D) 0.1156
E) 0.2778

Question 36

A solution is made by mixing 25.0 g of NaOH in H₂O. What is the amount of H₂O in the solution? (Mole fraction of solute = 0.090; molar mass of NaOH = 40.0 g/mol; molar mass of H₂O = 18.0 g/mol)

A) 113.8 g
B) 56.25 g
C) 256.5 g
D) 6.32 g
E) 125.6 g

Question 37

Only a certain amount of solute can be dissolved in a given amount of solvent. This maximum amount is called the _____ of the solute.

A) solubility
B) reactivity
C) dilution
D) hydraulicity
E) acidity

Question 38

A concentrated solution refers to a solution that has _____.

A) very low density
B) very high viscosity
C) large amounts of solute
D) large amounts of solvent
E) very high density

Question 39

The molarity of a solution made by dissolving 2.00 moles of HCl in water is 2.65 M. What is the volume of the solution?

A) 2.65 L
B) 755 mL
C) 265 mL
D) 0.53 L
E) 53 mL

Question 40

The concentration of Br^- ion in a sample of H₂O is 10 ppm. What mass of Br^- ion is present in 300.0 mL of H₂O, which has a density of 1.02 g/mL?

A) 10 mg
B) 6.00 mg
C) 3.00 mg
D) 3.06 mg
E) 4.52 mg

Question 41

What is dilution and concentration?

Question 42

A solution is made by mixing 6.000 g of C₁₀H₈ in 90.00 g of C₆H₆. If the vapor pressure of pure C₆H₆ is 39.30 torr, what is the vapor pressure of the solution? (Molar masses: C₁₀H₈ = 128.0 g/mol; C₆H₆ = 78.00 g/mol)

A) 35.64 torr
B) 1.201 torr
C) 1.843 torr
D) 37.76 torr
E) 0.9609 torr

Question 43

You are given 15 liters of a solution of NaCl in water. You estimate that the given solution has a molarity of 0.50 M. How do you increase the molarity of this solution to 1.0 M?

Question 44

What is the freezing point of a 10.0 m solution of NaOH in water? (K_f for water = 1.86 °C/m)?

A) -18.6°C
B) -3.20°C
C) -11.6°C
D) -37.2°C
E) -9.25°C

Question 45

What is the ideal van't Hoff factor for LiNO₃?

A) 2
B) 3
C) 4
D) 5
E) 6

Question 46

What is the freezing point of a 1.8 m solution of CBr₄ in C₆H₆? (K_f for C₆H₆ = 4.90°C/m; Freezing point of C₆H₆ = 5.51°C)

A) -6.90 °C
B) 2.30 °C
C) -3.31 °C
D) 0.212 °C
E) 1.20 °C

Question 47

How do you determine the solute and solvent in a solution? Explain with an example.

Question 48

The osmotic pressure of blood is 4.83 atm at 47.0°C. If blood were considered a solution of NaCl, what is the molal concentration of NaCl in blood? Assume an ideal van't Hoff factor.

A) 0.345 m
B) 0.690 m
C) 0.920 m
D) 0.460 m
E) 0.230 m

Question 49

What is molarity? Explain with an example.

Question 50

Determine the freezing point of a 2.33 m solution of PCl₅ in H₂O. (K_f = 1.86°C/m)

A) -8.66°C
B) 8.66°C
C) -2.10°C
D) -4.33°C
E) 1.20°C

Question 51

The osmotic pressure of a 0.0750 M KCl solution at 25.0°C is 3.28 atm. What is the true van't Hoff factor of this ionic compound?

A) 3.28
B) 0.0750
C) 0.250
D) 3.48
E) 1.79

Question 52

Explain the concentration units parts per thousand (ppth), parts per million (ppm), and parts per billion (ppb).

Question 53

The mole fraction of the solute in a solution is 0.1590. If the vapor pressure of the solvent in its pure state is 56.30 torr, what is the vapor pressure of the solution?

A) 56.45 torr
B) 47.35 torr
C) 17.90 torr
D) 49.95 torr
E) 39.55 torr

Question 54

What is the osmotic pressure of a 2.726 M solution of C₆H₁₂O₆ at 47.00°C?

A) 98.63 atm
B) 71.57 atm
C) 840.32 atm
D) 10.13 atm
E) 4.656 atm

Question 55

What is the boiling point of a 5.60 m solution of C₆H₄Cl₂ in CCl₄? Assume that C₆H₄Cl₂ is not volatile. (K_b = 4.95°C/m for CCl₄; T_BP = 76.8°C)

A) 105°C
B) 101°C
C) 89.8°C
D) 91.2°C
E) 123°C

Question 56

How many liters of a 0.5 M solution of CaCl₂ will contain 10 moles of CaCl₂? Explain your calculations.

Question 57

The boiling point of a solution of NaOH in H₂O is 100.84°C. What is the molality of the solution? Assume that NaOH is not volatile. (K_b = 0.51200°C/m for H₂O₄; T_BP = 100.00°C).

A) 1.112 m
B) 1.857 m
C) 1.641m
D) 0.9568 m
E) 0.8205 m

Question 58

Explain the concept of molality.

Question 59

Explain the concept of concentration in solutions.

Question 60

What is the van't Hoff factor for Fe(NO₃)₃?

A) 11
B) 5
C) 2
D) 3
E) 4

Question 61

_____ =

Question 62

What are colligative properties?

Question 63

The ideal van't Hoff Factor for FeCl₃ is _____.

Question 64

_____ is described by P_soln = χ_solvP*_solv.

Question 65

A 10.0 L of a 0.055 M solution are diluted to 15.8 L. The final concentration is _____ M.

Question 66

_____ is defined as the number of moles of solute per kilogram of solvent.

Question 67

_____ is the boiling point of a 6.200 m solution of NaCl in H₂O. Assume that NaCl is not volatile (K_b for water = 0.5120 °C/m).

Question 68

Explain Raoult's law.

Question 69

Explain the concept of mole fraction with an example.

Question 70

Explain freezing point depression.

Question 71

What mass of solute is present in 1 L of 1.60 M solution of NaCl? Explain the calculations.

Question 72

_____ g solute is present in 15 L of 0.20 M NaOH. (Molar mass of NaOH = 40.0 g/mol)

Question 73

The minor component of a solution is called the _____.

Question 74

A solution that has a lot of solute is called a(n) _____ solution.

Question 75

The molarity is 3.50 M when _____ mol of NaCl is found in 0.500 L of solution.

Question 76

What is the reason why you should not drink seawater if you're stranded in a lifeboat on an ocean?

Question 77

_____ liters of 0.005 M NaOH are needed to obtain 1.00 mol of NaOH.

Question 78

Explain the concept of boiling point elevation.

Question 79

_____ is a property of solutions related to the fraction that the solute particles occupy in the solution, not their identity.

Question 80

_____ is the addition of solvent, which decreases the concentration of the solute in the solution.