Deck 11: Solutions and Their Colligative Properties

Question 1

Which of the following will have the largest lattice energy?

A) NaF
B) NaCl
C) NaBr
D) NaI
E) CsCl

Answer 1

NaF

Question 2

Indicate which aqueous solution has the fastest evaporation rate.

A) 0.1 M KCl
B) 0.2 M Na₂CO₃
C) 0.2 M NaCl
D) 0.1 M MgCl₂
E) 0.2 M MgCl₂

Answer 2

0.1 M KCl

Question 3

The vapor pressure of an aqueous solution is found to be 24.9 mm Hg at 25°C. What is the mole fraction of solute in this solution? The vapor pressure of water is 25.756 mm Hg at 25°C.

A) 0.967
B) 0.0332
C) 1.03
D) 0.0344
E) 0.976

Answer 3

0.0332

Question 4

Which of the following is needed to calculate the lattice energy of an ionic compound?

A) enthalpy of solution
B) enthalpy of combustion
C) specific heat
D) ionization energy
E) enthalpy of solvation

Question 5

Calculate the lattice energy of sodium fluoride from the following data: Ionization energy of Na: 496 kJ/mol
Electron affinity of F: -328 kJ/mol
Energy to vaporize Na: 108 kJ/mol
F₂ bond energy: 160 kJ/mol
Energy change for the reaction:
Na(s) + F₂(g)  NaF(s); H = -575 kJ

A) 931 kJ/mol
B) -931 kJ/mol
C) -1011 kJ/mol
D) 1011 kJ/mol
E) -851 kJ/mol

Question 6

Indicate which aqueous solution has the slowest evaporation rate.

A) 0.1 M KCl
B) 0.2 M Na₂CO₃
C) 0.2 M NaCl
D) 0.1 M MgCl₂
E) 0.1 M NaBr

Question 7

Which of the solutions shown here will have the highest vapor pressure? White circles indicate solvent molecules; black circles indicate molecules of a nonvolatile solute.

A)
B)
C)
D)

Question 8

Determine the energy change for the reaction Li(s) + Cl₂(g)  LiCl(s)
From the following data:
Lattice energy of LiCl = -861 kJ/mol
Energy to vaporize Li = 159 kJ/mol
Ionization energy of Li = 520 kJ/mol
Cl₂ bond energy: 240 kJ/mol
Electron affinity of Cl: -349 kJ/mol

A) -411 kJ/mol
B) -528 kJ/mol
C) 311 kJ/mol
D) -861 kJ/mol
E) -291 kJ/mol

Question 9

At 25°C, the vapor pressure of pure water is 25.756 mm Hg. What is the vapor pressure of water in a 0.500 m solution of sodium chloride?

A) 25.52 mm Hg
B) 0.2301 mm Hg
C) 0.4602 mm Hg
D) 25.35 mm Hg
E) 12.88 mm Hg

Question 10

Which listing of ionic compounds is in order of increasing melting point?

A) NaF < MgF₂ < AlF₃
B) MgF₂ < NaF < AlF₃
C) AlF₃ < MgF₂ < NaF
D) AlF₃ < NaF < MgF₂
E) NaF < AlF₃ < MgF₂

Question 11

Which of the solutions shown here will have the lowest vapor pressure? White circles indicate solvent molecules; black circles indicate molecules of a nonvolatile solute.

A)
B)
C)
D)

Question 12

Which of the following is not typically needed to calculate the lattice energy of an ionic compound?

A) enthalpy of vaporization
B) bond enthalpy
C) enthalpy of solution
D) electron affinity
E) ionization energy

Question 13

Indicate which aqueous solution has the lowest vapor pressure.

A) 0.1 M KCl
B) 0.1 M Na₂CO₃
C) 0.2 M NaCl
D) 0.1 M MgCl₂
E) 0.2 M MgCl₂

Question 14

Indicate which aqueous solution has the highest vapor pressure.

A) 0.1 M KCl
B) 0.2 M Na₂CO₃
C) 0.2 M NaCl
D) 0.1 M MgCl₂
E) 0.2 M MgCl₂

Question 15

Which of the following compounds has the largest melting point?

A) NaF
B) KCl
C) RbCl
D) BeF₂
E) NaCl

Question 16

Which of the following requires the smallest energy to separate the ions?

A) CaF₂
B) KF
C) NaF
D) MgF₂
E) LiF

Question 17

Which of the following ranks the compounds from lowest to highest lattice energy?

A) NaF < MgF₂ < CaF₂ < KF
B) KF < NaF < CaF₂ < MgF₂
C) MgF₂ < CaF₂ < NaF < KF
D) CaF₂ < KF < NaF < MgF₂
E) MgF₂ < CaF₂ < KF < NaF

Question 18

Coulomb's law states that the interaction energy between ions depends __________

A) only on the ionic charges.
B) only on the distance between the ions.
C) directly on both the ionic charges and the distance between the ions.
D) on the temperature.
E) directly on the ionic charges and inversely on the distance between the ions.

Question 19

What is the vapor pressure of an aqueous solution that has a solute mol fraction of  = 0.100? The vapor pressure of water is 25.756 mm Hg at 25°C.

A) 23.2 mm Hg
B) 2.58 mm Hg
C) 25.8 mm Hg
D) 0.900 mm Hg
E) 22.3 mm Hg

Question 20

Which of the following will require the greatest energy input to separate the ions?

A) MgI₂
B) MgF₂
C) MgCl₂
D) MgBr₂
E) NaCl

Question 21

Click, Clack, and Jim have identical icy driveways. Click buys 10 lb of NaCl, Clack buys 10 lb of CaCl₂, and Jim buys 10 lb of MgCl₂. They spread these salts on their driveways. Which driveway will deice more effectively? (Assume that ideal dissociation of the salts occurs, and that colligative properties are the only consideration.)

A) Click's driveway will deice best.
B) Clack's driveway will deice best.
C) Jim's driveway will deice best.
D) The three driveways will deice to the same extent.
E) Clack and Jim's driveways will deice better than Click's.

Question 22

Which statement regarding osmotic pressure is not correct? Osmotic pressure __________

A) increases with increasing temperature.
B) increases with increasing molar concentration of solute.
C) is greater for 0.1 M Na₂SO₄ than for 0.1 M NaCl.
D) depends on the value of the gas constant R.
E) is the same for solutions with the same mass percent of solute.

Question 23

Determine the molal concentration of a sugar solution in water that has a freezing point of -2.1°C. K_f = 1.86°C/m for water.

A) 1.13 m
B) -1.13 m
C) 3.91 m
D) -3.91 m
E) 0.113 m

Question 24

Which solution, if either, would create the higher osmotic pressure (compared to pure water): one prepared from 1.0 g of NaCl in 10 mL of water or 1.0 g of CsBr in 10 mL of water?

A) They would have the same osmotic pressures.
B) NaCl would give the higher pressure.
C) CsBr would give the higher pressure.
D) It is impossible to tell.
E) These compounds are salts and do not produce an osmotic pressure.

Question 25

Which solution will have the lowest osmotic pressure when measured against pure water?

A) 0.10 M sodium chloride
B) 0.10 M sodium sulfate
C) 0.10 M sodium sulfide
D) 0.10 M sodium phosphate
E) 0.10 M sodium carbonate

Question 26

What would be the freezing point of a 1 m solution of HCl in water (K_f = 1.86°C)?

A) 0.0°C
B) -1.86°C
C) -3.72°C
D) 1.86°C
E) -0.93°C

Question 27

A solution is made by dissolving 100 g of essentially nonvolatile ethylene glycol (C₂H₆O₂) in 500 g of water. What is the resulting freezing point of the solution (K_f = 1.86°C/m)?

A) -5.99°C
B) -1.86°C
C) -0.372°C
D) -1.61°C
E) -3.23°C

Question 28

Which of the following would be most effective in melting ice on a sidewalk?

A) 1 kg NaCl
B) 1 kg KCl
C) 1 kg MgCl₂
D) 1 kg CuCl
E) 1 kg CaCl₂

Question 29

You like boiled eggs for breakfast, but they take too long to cook, and you are always late to your early morning class. Lucky you! You have learned that adding table salt, NaCl (58.4 g/mol, 2.16 g/cm³), to water (K_b = 0.52^oC/m) increases the temperature at which it boils. You figure that you can cook eggs faster at a higher temperature in boiling salty water! What increase in the boiling point do you expect if you add 1 tablespoon (1 tbsp = 14.8 cm³) of salt to one 8-oz cup of water (237 mL)?

A) 1.0°C
B) 2.4°C
C) 28°C
D) 1.5°C
E) 3.7°C

Question 30

Isopropyl alcohol has a boiling point of 82.3°C. Solutions of isopropyl alcohol in water have normal boiling points less than 100°C. Is this observation consistent with the following equation? Explain. T_b = iK_bm

A) No, boiling point elevation only pertains to ionic solutes.
B) No, boiling point elevation only pertains to nonvolatile solutes.
C) Yes, boiling point depression occurs for all solutions.
D) Yes, the boiling point depression constant for isopropyl alcohol is large.
E) No, isopropyl alcohol can hydrogen bond with water.

Question 31

You like boiled eggs for breakfast, but they take too long to cook, and you are always late to your early morning class. Lucky you! You have learned that adding table salt, NaCl (58.4 g/mol, 2.16 g/cm³), to water (K_b = 0.52^oC/m) increases the temperature at which it boils. You figure that you can cook eggs faster at a higher temperature in boiling salty water! What increase in the boiling point do you expect if you add 4 tablespoons (1 tbsp = 14.8 cm³) of salt to 16 oz of water (474 mL)?

A) 14°C
B) 4.8°C
C) 28°C
D) 3.0°C
E) 8.4°C

Question 32

A newspaper article suggested using a fertilizer such as ammonium sulfate or ammonium nitrate to lower the melting point of ice on sidewalks because many of the deicing salts can damage lawns and sidewalks. Which of the following compounds would give the largest freezing point depression when 100 g of the compound are dissolved in 1 kg of solvent?

A) NH₄NO₃ (80.1 g/mol)
B) (NH₄)₂SO₄ (132.1 g/mol)
C) MgSO₄ (120.4 g/mol)
D) CaCl₂ (111.0 g/mol)
E) MgCl₂ (95.2 g/mol)

Question 33

Which of the following would not be effective in melting ice on a sidewalk?

A) NaCl
B) KCl
C) MgCl₂
D) CuCl
E) CaCl₂

Question 34

The normal temperature range of the liquid phase of pure water is 0°C to 100°C. Which of the following solutions will have the largest temperature range for the liquid state?

A) 1 M aqueous ethanol solution
B) 1 M aqueous potassium bromide solution
C) 1 M aqueous acetic acid solution
D) 1 M aqueous magnesium bromide solution
E) 1 M aqueous magnesium sulfate

Question 35

Which statement is not correct? Determination of molar mass of an unknown sample by an osmotic pressure measurement requires that __________

A) the solute dissolved in the solution is pure.
B) the solute is a nonelectrolyte.
C) the molecules of the solute do not pass through the semipermeable membrane.
D) the mass of the solute dissolved in the solution is known in advance.
E) the molar concentration of the solute in the solution is known in advance.

Question 36

In the process of dialysis, a special semipermeable membrane allows both small molecules and water to pass through, but not large protein molecules. These membranes are used to separate these small molecules and ions from much larger proteins. If a mixture of proteins and small molecules were separated from pure water by a dialysis membrane as shown in the figure, which way would the molecules flow?

A) Both water and small molecules would pass through into the pure water.
B) Only the proteins would pass through into the pure water.
C) Water would enter the solution while small molecules would pass through into the pure water.
D) Only small molecules would pass through the membrane, water and proteins would not.
E) Only water would pass through the membrane into the solution.

Question 37

Calculate the minimum pressure that must be applied to achieve reverse osmosis of 0.504 M NaCl at 22C.

A) 0.906 atm
B) 92.2 atm
C) 0.909 atm
D) 12.2 atm
E) 24.4 atm

Question 38

What is the molality of a solution produced by dissolving 14.40 g of LiCl (42.39 g/mol) in water to make 0.104 L of solution with a density of 1.102 g/mL?

A) 0.340 m
B) 3.39 m
C) 3.27 m
D) 3.74 m
E) 2.96 m

Question 39

The concentration unit of molality is symbolized as

A) M
B) m
C) "M"
D) mol
E) mo

Question 40

You are working as an intern in a biochemistry lab. Your advisor just isolated an enzyme and asks you to determine its molar mass using osmosis. You dissolve 1.0 g of the enzyme in water to make 250 mL of solution. You measure the osmotic pressure, and find it to be 3.5 torr at 298 K. You report that the molar mass is __________ g/mol.

A) between 0 and 1000
B) between 1000 and 5000
C) between 5000 and 10,000
D) between 10,000 and 20,000
E) between 20,000 and 50,000

Question 41

A saline solution is administered intravenously to patients who cannot take fluid orally and are in danger of dehydration. The osmotic pressure of this solution must match that of blood to prevent hemolysis or crenation of blood cells. What mass of sodium chloride (58.44 g/mol) is needed to produce 100.0 mL of saline solution with an osmotic pressure of 7.83 atm at a body temperature of 37°C?

A) 0.899 g
B) 8.99 g
C) 18.0 g
D) 1.80 g
E) 0.450 g

Question 42

Gasoline is primarily a mixture of hydrocarbons and is sold with an octane rating that is based on a comparison with the combustion properties of isooctane. Gasoline usually contains an isomer of isooctane called tetramethylbutane (C₈H₁₈), which has an enthalpy of vaporization of 43.3 kJ/mol and a boiling point of 106.5°C. Determine the vapor pressure of tetramethylbutane on a very hot summer day when the temperature is 38°C.

A) 80.0 torr
B) 36.7 torr
C) 67.8 torr
D) 47.9 torr
E) 89.3 torr

Question 43

A solution contains 6.50 mol water, 0.300 mol sucrose, and 0.200 mol glucose. The solutes are nonvolatile. What is the vapor pressure of the solution at 35°C given that the vapor pressure of water is 42.2 torr?

A) 35.0 torr
B) 36.0 torr
C) 37.0 torr
D) 39.2 torr
E) 39.0 torr

Question 44

Calculate the molality of a solution containing 0.355 mol sodium hydrogen carbonate (baking soda) and 245 g of water.

A) 1.45 m
B) 1.12  10^-2 m
C) 2.11 m
D) 1.12  10^-3 m
E) 0.0211 m

Question 45

Portable lanterns and stoves used for camping often use a mixture of hydrocarbons for fuel. One such hydrocarbon is an alkane called n-pentane. These lanterns and stoves are often difficult to light on a cold day because the fuel has a low vapor pressure at low temperatures. Determine the vapor pressure of n-pentane on a night when the temperature is 0.0^oC. The enthalpy of vaporization of n-pentane is 27.6 kJ/mol, and its boiling point is 36.0°C.

A) 228 torr
B) 367 torr
C) 184 torr
D) 479 torr
E) 209 torr

Question 46

A solution is prepared by adding 0.300 mol glucose, which is not volatile, to 4.50 mol water. What is the vapor pressure of this solution at 25°C given that the vapor pressure of pure water is 23.8 torr?

A) 9.38 torr
B) 22.3 torr
C) 23.4 torr
D) 1.49 torr
E) 22.5 torr

Question 47

Which statement below regarding vapor pressure is not correct?

A) Vapor pressure is an intensive property.
B) The substance with the stronger intermolecular forces has the lower vapor pressure.
C) Vapor pressure increases with increasing temperature.
D) Pure water has a higher vapor pressure at a given temperature than seawater.
E) A nonvolatile solute increases the vapor pressure of the solvent.

Question 48

What physical property is used to separate the hydrocarbon components in petroleum (crude oil)?

A) melting point
B) density
C) boiling point
D) molar mass
E) viscosity

Question 49

Gasoline is primarily a mixture of hydrocarbons and is sold with an octane rating that is based on a comparison with the properties of isooctane (C₈H₁₈), which has an enthalpy of vaporization of 35.8 kJ/mol and a boiling point of 98.2°C. Determine the vapor pressure of isooctane on a very hot summer day when the temperature is 38°C.

A) 80.0 torr
B) 36.7 torr
C) 67.8 torr
D) 47.9 torr
E) 89.3 torr

Question 50

Which one of the ionic compounds below would you expect to have the largest (most negative) lattice energy?

A) MgO
B) CaO
C) SrO
D) BaO
E) BeO

Question 51

Which one of the ionic compounds below would you expect to have the smallest (least negative) lattice energy?

A) MgF₂
B) MgCl₂
C) MgBr₂
D) MgI₂
E) CaI₂

Question 52

Ethylene glycol is used in automobile radiators as an antifreeze. What will the freezing point of an antifreeze solution be if 2.5 L of ethylene glycol are mixed together with 2.5 L of water? The following information may be helpful to you. Ethylene glycol has a very low vapor pressure and is essentially nonvolatile. molar mass of ethylene glycol = 62.1 g/mol
Van't Hoff factor = 1
Density of ethylene glycol = 1.11 g/mL
Density of water = 1.00 g/mL
K_f for water = 1.86°C kg/mol

A) -39°C
B) -16°C
C) -1.6°C
D) -33°C
E) -24°C

Question 53

Which one of the ionic compounds below would you expect to have the largest (most negative) lattice energy?

A) MgF₂
B) MgCl₂
C) MgBr₂
D) MgI₂
E) CaI₂

Question 54

Which of the following aqueous solutions will have the lowest freezing point?

A) 0.1 m magnesium sulfate, MgSO₄
B) 0.1 m potassium chloride, KCl
C) 0.08 m magnesium chloride, MgCl₂
D) 0.04 m sodium sulfate, Na₂SO₄
E) 0.05 m sodium chloride, NaCl

Question 55

The aroma from almonds and cherries is due in part to a compound called benzaldehyde. A graph of the natural logarithm of the vapor pressure of benzaldehyde vs. 1/temperature produces a straight line with a slope of -5870.99 K. What is the enthalpy of vaporization of benzaldehyde?

A) +473 kJ/mol
B) -47.3 kJ/mol
C) +47.3 kJ/mol
D) -48.8 kJ/mol
E) +48.8 kJ/mol

Question 56

The smell of fresh-cut pine is due in part to a cyclic alkene called pinene. A graph of the natural logarithm of the vapor pressure of pinene vs. 1/temperature produces a straight line with a slope of -4936.37 K. What is the enthalpy of vaporization of pinene?

A) +397 kJ/mol
B) -39.7 kJ/mol
C) +39.7 kJ/mol
D) -41.0 kJ/mol
E) +41.0 kJ/mol

Question 57

Which statement regarding the fractional distillation of two substances is not correct?

A) The substance with the lower boiling point has a higher concentration in the vapor than in the liquid.
B) The boiling point of the mixture is not constant, changing as the distillation progresses.
C) The substance with the higher vapor pressure has a higher concentration in the vapor than in the liquid.
D) The mole ratio of the two substances in the vapor is not the same as it is in the liquid.
E) Raoult's law does not apply to mixtures of volatile components.

Question 58

A solution is prepared by adding 1.50 mol glucose, which is not volatile, to 3.50 mol water. What is the vapor pressure of this solution at 25°C given that the vapor pressure of pure water is 23.8 torr?

A) 7.00 torr
B) 16.7 torr
C) 10.2 torr
D) 7.14 torr
E) 34.0 torr

Question 59

Which one of the ionic compounds below would you expect to have the smallest (least negative) lattice energy?

A) MgO
B) CaO
C) SrO
D) BaO
E) BeO

Question 60

Calculate the molality of a solution containing 0.755 mol glucose and 1.75 kg of water.

A) 0.875 m
B) 0.583 m
C) 0.431 m
D) 580 m
E) 0.850 m

Question 61

A 376 mg sample of a nonelectrolyte compound isolated from throat lozenges was dissolved in water to produce 10.0 mL of a solution at 25°C. The osmotic pressure of this solution was measured and found to be 4.89 atm. What is the molar mass of this compound?

A) 489 g/mol
B) 941 g/mol
C) 48.9 g/mol
D) 199 g/mol
E) 188 g/mol

Question 62

Identify the following statement as true or false and choose the correct explanation. "For solutions with the same molarity at the same temperature, the pressure needed for reverse osmosis of a sodium chloride solution will always be less than the pressure needed for a calcium chloride solution."

A) True, because the molar mass of sodium chloride is smaller.
B) True, because the van't Hoff factor is smaller for sodium chloride.
C) False, because the van't Hoff factor is smaller for sodium chloride.
D) False, because the van't Hoff factor is larger for sodium chloride.
E) True, because the van't Hoff factor is larger for sodium chloride.

Question 63

Eugenol is one of the compounds responsible for the flavor of cloves. A 222-mg sample of eugenol was dissolved in 1.00 g of chloroform (K_b = 3.63°C/m), increasing the boiling point of chloroform by 3.68°C. What is the molar mass of eugenol?

A) 82.0 g/mol
B) 125 g/mol
C) 164 g/mol
D) 193 g/mol
E) 219 g/mol

Question 64

Identify the following statement as true or false and choose the correct explanation. "For solutions with the same reverse osmotic pressure at the same temperature, the molarity of a sodium chloride solution will always be less than the molarity of a calcium chloride solution."

A) True, because the molar mass of sodium chloride is smaller.
B) True, because the van't Hoff factor is smaller for sodium chloride.
C) False, because the van't Hoff factor is smaller for sodium chloride.
D) False, because the van't Hoff factor is larger for sodium chloride.
E) True, because the van't Hoff factor is larger for sodium chloride.

Question 65

What mass of a 0.66 m ammonium nitrate (80.04 g/mol) solution will contain 0.15 mol of solute?

A) 227 g
B) 239 g
C) 440 g
D) 493 g
E) 4453 g

Question 66

The arrow in the diagram below indicates the direction of solvent flow through a membrane in osmosis. Which solution, A or B, is more concentrated? Explain your reasoning.

Question 67

A 15.0 mg sample of a protein was dissolved in water to produce 5.00 mL of solution at 25.1°C. The osmotic pressure of this solution was measured and found to be 6.50 torr. What is the molar mass of this protein?

A) 427 g/mol
B) 941 g/mol
C) 8580 g/mol
D) 4270 g/mol
E) 561 g/mol

Question 68

How many moles of solute are there in a 0.155 m glucose solution prepared with 50.0 kg of water?

A) 15.5 mol
B) 15.0 mol
C) 0.155 mol
D) 31.0 mol
E) 7.75 mol

Question 69

Does the temperature of the vapors in a still head increase or decrease as a fractional distillation progresses? Explain.

Question 70

What is the molarity of a sucrose (C₁₂H₂₂O₁₁) solution that produces an osmotic pressure of 2.65 atm at 25°C?

A) 0.0349 M
B) 0.127 M
C) 0.0127 M
D) 0.108 M
E) 0.398 M

Question 71

A physiological saline solution is 0.92% NaCl by mass. What is the osmotic pressure of such a solution at a body temperature of 37°C?

A) 8.0 atm
B) 3.9 atm
C) 2.3 atm
D) 4.3 atm
E) 4.1 atm

Question 72

A 300-mg sample of caffeine was dissolved in 10.0 g of camphor (K_f = 39.7°C/m), decreasing the freezing point of camphor by 3.07°C. What is the molar mass of caffeine?

A) 47.0 g/mol
B) 194 g/mol
C) 388 g/mol
D) 94.0 g/mol
E) 97.0 g/mol

Question 73

Which has the higher vapor pressure at a given temperature, pure water or salty seawater? Explain.

Question 74

A mixture of salt and ice is used to chill the contents of old-fashioned, hand-operated ice cream makers. What is the melting point of a mixture of 1.00 lb of sodium chloride and 16.00 lb of ice if exactly half the ice melts? Assume ideal behavior and that all the sodium chloride dissolves in the melted ice water. K_f(water) = 1.86°C/m

A) -8°C
B) -11°C
C) -12°C
D) -21°C
E) -15°C

Question 75

A solution of 5.00 g of sodium chloride in 1.00 kg of water has a freezing point of -0.299°C. What is the actual van't Hoff factor for this salt at this concentration compared to the ideal one of 2? K_f(water) = 1.86°C/m

A) 1.88
B) 1.98
C) 1.93
D) 1.83
E) 1.94

Question 76

The term colligative refers to properties that __________

Question 77

The freezing point of a 0.0925 m solution of ammonium chloride was found to be -0.325°C. What is the actual van't Hoff factor for this salt at this concentration compared to the ideal one of 2? K_f(water) = 1.86°C/m

A) 1.89
B) 1.95
C) 1.90
D) 1.80
E) 1.97

Question 78

Magnesium chloride is often used to melt ice on sidewalks. Considering that the solubility of magnesium chloride (95.21 g/mol) in water is 54.3 g per 100.0 g of water, what is the lowest temperature that you would expect to be able to melt ice with magnesium chloride? Assume ideal behavior. K_f(water) = 1.86°C/m

A) -40°C
B) -32°C
C) -11°C
D) -25°C
E) -22°C

Question 79

Rank the following ionic compounds in order of increasing lattice energy (largest lattice energy is the most negative): MgF₂, MgCl₂, MgBr₂, and MgI₂.

Question 80

Define the terms enthalpy of solution, enthalpy of hydration, and lattice energy.