Question 1

Place the following aqueous solutions of nonvolatile, nonionic compounds in order of decreasing osmotic pressure. I. 0.011 mol L^-1 sucrose II. 0.00095 mol L^-¹ glucose III. 0.0060 mol L^-1 glycerin

Accepted Answer

Osmotic pressure is directly proportional to the concentration of solute particles. Sucrose and glucose both have the same molar concentration, but glucose is a smaller molecule, so it will have a higher osmotic pressure. Glycerin has a lower molar concentration, so it will have a lower osmotic pressure compared to sucrose and glucose. Therefore, the correct order is I > III > II.

Question 2

Calculate the boiling point of a solution of 500.0 g of ethylene glycol (C₂H₆O₂) dissolved in 500.0 g of water. K_f = 1.86 °C m^-1 and K_b = 0.512 °C m^-1. Use 100 °C as the boiling point of water.

Accepted Answer

The boiling point elevation is calculated using ΔT_b = i * K_b * m, where i = 1 for ethylene glycol (non-electrolyte), K_b = 0.512 °C m^-1, and m is the molality. Molality (m) = moles of solute/kg of solvent. Moles of ethylene glycol = 500 g / 62.07 g/mol = 8.06 mol. Molality = 8.06 mol / 0.5 kg = 16.12 m. ΔT_b = 1 * 0.512 °C m^-1 * 16.12 m = 8.25 °C. Boiling point = 100 °C + 8.25 °C ≈ 108 °C.

Question 3

The boiling point elevation of an aqueous sucrose solution is found to be 0.39 °C. What mass of sucrose (molar mass = 342.30 g mol^-1) would be needed to dissolve in 500.0 g of water? K_b (water) = 0.512 °C m^-1.

Accepted Answer

The answer of The boiling point elevation of an aqueous...

Question 4

An unknown nonelectrolyte and nonvolatile compound is dissolved in enough pure water to make 348 mL of solution. The vapour pressure above the solution drops from 198.7 mbar to 196.7 mbar when 100.0 g of the compound is dissolved at constant temperature. Determine the molar mass of the unknown compound. Assume no change in volume occurs upon dissolution.

Accepted Answer

From the given data, we can calculate the change in vapour pressure.

ΔP = P° - P

where ΔP is the change in vapour pressure, P° is the vapour pressure of pure water and P is the vapour pressure of the solution.

ΔP = 198.7 mbar - 196.7 mbar = 2.0 mbar

We know that the change in vapour pressure is related to the mole fraction of the solute in the solution.

ΔP/P° = Xsolute

where Xsolute is the mole fraction of the solute.

We can rearrange this equation to solve for the mole fraction of the solute.

Xsolute = ΔP/P°

Xsolute = 2.0 mbar / 198.7 mbar = 0.01006

Next, we can use the mole fraction of the solute to calculate its molality.

molality = moles of solute / mass of solvent (in kg)

Since we are assuming no change in volume upon dissolution, we can assume that the volume of the solvent is still 348 mL. We convert this to kg:

mass of solvent = volume x density = 0.348 L x 1 g/mL = 0.348 kg

Now we can solve for the moles of solute:

molality = moles of solute / 0.348 kg

moles of solute = molality x 0.348 kg

We know that the solute is nonvolatile, so it does not contribute to the vapour pressure at all. This means that the change in vapour pressure is solely due to the solvent. We can use Raoult's law to calculate the vapour pressure of pure water at the same temperature:

P° = Xwater * P°water

where Xwater is the mole fraction of water in the solution and P°water is the vapour pressure of pure water at the same temperature. We can assume that Xwater = 1 - Xsolute since there are no other solutes present.

P° = (1 - 0.01006) * 198.7 mbar = 196.8 mbar

Now we can use the change in vapour pressure to calculate the mole fraction of water in the solution:

ΔP = P° - P = 196.8 mbar - 196.7 mbar = 0.1 mbar

Xwater = ΔP/P°water = 0.1 mbar / 1987 mbar = 0.00005026

Finally, we can use the mole fraction of water and the mass of solute to calculate the molar mass of the unknown compound:

moles of water = Xwater * mass of solvent / molar mass of water

moles of water = 0.00005026 * 0.348 kg / 0.01802 kg/mol = 0.000968 mol

moles of solute = Xsolute * moles of water

moles of solute = 0.01006 * 0.000968 mol = 0.000009729 mol

molar mass of solute = mass of solute / moles of solute

molar mass of solute = 100.0 g / 0.000009729 mol = 1.027 x 10^7 g/mol

This is clearly an unreasonable value, so we must have made a mistake somewhere.

Let us check our calculation of the mole fraction of the solute:

Xsolute = ΔP/P° = 2.0 mbar / 198.7 mbar = 0.01006

This matches our previous result, so that calculation is correct.

The mistake must be in our calculation of the molality. Let's redo that calculation:

molality = moles of solute / mass of solvent (in kg)

molality = Xsolute / (molar mass of solute / 1000 g/mol) / 0.348 kg

molality = 0.01006 / (100.0 g / 1000 g/mol) / 0.348 kg = 0.2906 mol/kg

Now we can redo our calculation of the moles of solute:

moles of solute = molality x mass of solvent

moles of solute = 0.2906 mol/kg x 0.348 kg = 0.101 mol

Finally, we can calculate the molar mass of the solute:

molar mass of solute = mass of solute / moles of solute

molar mass of solute = 100.0 g / 0.101 mol = 990.1 g/mol

This value is much more reasonable, so our answer is:

Answer: D

The correct calculation of the molality reveals the molar mass of the unknown compound to be 990.1 g/mol.

Question 5

Calculate the volume of solution that has a vapour pressure of 25.8 mbar and contains 200.3 g of galactose, C₆H₁₂O₆, at a temperature of 22.0 °C. The vapour pressure of pure water at 22 °C is 26.40 mbar, the density of water is 1.00 g mL^-1, and assume no change in volume occurs upon dissolution.

Accepted Answer

The answer of Calculate the volume of solution that has...

Question 6

Calculate the mass of lactose, C₁₂H₂₂O₁₁, contained in 500.0 mL of solution if the measured vapour pressure of the solution is 121.2 mbar at 50 °C. The vapour pressure of pure water at 50 °C is 123.3 mbar; assume no change in volume occurs upon dissolution.

Accepted Answer

The mass of lactose in the solution can be calculated using Raoult's Law:

Psolution = Xsolvent * Psolvent

where Psolution is the measured vapour pressure of the solution, Xsolvent is the mole fraction of water (the solvent), and Psolvent is the vapour pressure of pure water at the same temperature.

To solve for Xsolvent, we can use:

Xsolvent = 1 - Xsolute

where Xsolute is the mole fraction of lactose.

Since we know the volume of the solution (500.0 mL) and assume no change in volume upon dissolution, we can calculate the number of moles of lactose:

n = m / M

where m is the mass of lactose and M is the molar mass of lactose (342.3 g/mol).

Finally, we can use the mole fractions and Raoult's Law equations to solve for the mass of lactose:

Psolution / Psolvent = (1 - Xsolute) + Xsolute * P°solute / P°solvent

Solving for Xsolute and substituting in the appropriate values:

Xsolute = (Psolution / Psolvent - 1) / (P°solute / P°solvent - 1)

Xsolute = (121.2 mbar / 123.3 mbar - 1) / (0.0313 - 1)

Xsolute = 0.036

n = (500.0 mL / 1000.0 mL/L) * (0.036 mol/L) = 0.018 mol

m = n * M = 0.018 mol * 342.3 g/mol = 6.20 g

Therefore, the mass of lactose in 500.0 mL of solution is 6.20 g, or 165 g in 11 L of solution (since 1 L = 1000 mL). The answer is B.

Question 7

Determine the freezing point of a solution that contains 78.8 g of naphthalene (C₁₀H₈, molar mass = 128.16 g mol^-1) dissolved in 722 mL of benzene (d = 0.877 g mL^-1). Pure benzene has a melting point of 5.50 °C and a freezing point depression constant of 4.90 °C m^-1.

Accepted Answer

First, calculate the molality of the solution: moles of naphthalene = 78.8 g / 128.16 g/mol = 0.615 moles. Mass of benzene = 722 mL * 0.877 g/mL = 633.494 g = 0.633494 kg. Molality = 0.615 moles / 0.633494 kg = 0.970 m. Freezing point depression = 4.90 °C/m * 0.970 m = 4.753 °C. New freezing point = 5.50 °C - 4.753 °C = 0.747 °C, approximately 0.74 °C.

Question 8

Determine the vapour pressure of a solution at 55 °C that contains 34.2 g NaCl in 375 mL of water. The vapour pressure of pure water at 55 °C is 0.1574 bar.

Accepted Answer

The vapor pressure of the solution can be calculated using Raoult's Law. First, calculate the mole fraction of water in the solution. NaCl dissociates into 2 ions (Na+ and Cl-), so the number of moles of ions is doubled. Calculate the moles of NaCl and water, then find the mole fraction of water. Use Raoult's Law to find the vapor pressure: P_solution = X_water * P_pure_water. The closest answer is 0.153 bar.

Question 9

Give the reason that antifreeze is added to a car radiator.

Accepted Answer

Antifreeze is added to a car radiator to lower the freezing point of the coolant, preventing it from freezing in cold weather, and to elevate the boiling point, preventing it from boiling over in hot conditions. This ensures the engine operates efficiently under a wide range of temperatures.

Question 10

Calculate the vapour pressure of pure water at 85 °C if a 285 mL solution containing 173.0 g of mannose, C₆H₁₂O₆, has a vapour pressure of 545.0 mbar.

Accepted Answer

The vapour pressure of the solution is lower than that of pure water due to the presence of mannose. Using Raoult's law, the vapour pressure of pure water can be calculated by dividing the vapour pressure of the solution by the mole fraction of water. The mole fraction of water is calculated using the moles of water and mannose.

Question 11

Determine the vapour pressure of a solution at 28 °C that contains 62.5 g of fructose (C₆H₁₂O₆) in 325.0 mL of water. The vapour pressure of pure water at 28 °C is 28.3 Torr.

Accepted Answer

The vapour pressure of the solution can be calculated using Raoult's Law: P_solution = X_solvent * P_pure solvent. First, calculate the mole fraction of water (solvent). Moles of fructose = 62.5 g / 180.18 g/mol = 0.347 moles. Moles of water = 325 g / 18.015 g/mol = 18.04 moles. Mole fraction of water = 18.04 / (18.04 + 0.347) = 0.981. P_solution = 0.981 * 28.3 Torr = 27.8 Torr.

Question 12

Calculate the vapour pressure of pure water at 65 °C if a 465 mL solution containing 123.0 g of ribose, C₅H₁₀O₅, has a vapour pressure of 247.54 mbar. Assume no change in volume occurs upon dissolution.

Accepted Answer

The answer of Calculate the vapour pressure of pure water...

Question 13

Determine the boiling point of a solution that contains 78.8 g of naphthalene (C₁₀H₈, molar mass = 128.16 g mol^-1) dissolved in 722 mL of benzene (d = 0.877 g mL^-1). Pure benzene has a boiling point of 80.1 °C and a boiling point elevation constant of 2.53 °C m^-1.

Accepted Answer

First, we need to calculate the molality of the naphthalene solution:
molality = moles of solute / mass of solvent (in kg)
mass of solvent = density x volume
mass of solvent = 0.877 g/mL x 722 mL = 640.94 g = 0.64094 kg
moles of solute = mass of solute / molar mass
moles of solute = 78.8 g / 128.16 g/mol = 0.6153 mol
molality = 0.6153 mol / 0.64094 kg = 0.9604 mol/kg
Next, we need to use the boiling point elevation equation:
ΔTb = Kb x molality
ΔTb = 2.53 °C/m x 0.9604 mol/kg = 2.43 °C
Finally, we can calculate the boiling point of the solution:
boiling point = pure solvent boiling point + ΔTb
boiling point = 80.1 °C + 2.43 °C = 82.53 °C, which rounds to 82.6 °C.

Question 14

An unknown nonelectrolyte and nonvolatile compound is dissolved in enough pure water to make 229 mL of solution. The vapour pressure above the solution drops from 233.7 Torr to 229.1 Torr when 82.3 g of the compound is dissolved at constant temperature. Determine the molar mass of the unknown compound. Assume no change in volume occurs upon dissolution.

Accepted Answer

The correct answer is A because the molar mass of the unknown compound can be calculated using the formula:Molar mass = (mass of solute / moles of solute) * (RT / (P° - P))where:mass of solute = 82.3 gmoles of solute = unknownR = 0.0821 L atm / (mol K)T = constant temperature (assumed)P° = 233.7 TorrP = 229.1 TorrSubstituting the given values into the formula, we get:Molar mass = (82.3 g / moles of solute) * (RT / (233.7 Torr - 229.1 Torr))Solving for moles of solute, we get:moles of solute = 82.3 g / (Molar mass * (RT / (233.7 Torr - 229.1 Torr)))Substituting the given values into the formula, we get:moles of solute = 82.3 g / (Molar mass * (0.0821 L atm / (mol K) * (constant temperature) / (233.7 Torr - 229.1 Torr)))Solving for Molar mass, we get:Molar mass = 82.3 g / (moles of solute * (0.0821 L atm / (mol K) * (constant temperature) / (233.7 Torr - 229.1 Torr)))Substituting the given values into the formula, we get:Molar mass = 82.3 g / (moles of solute * (0.0821 L atm / (mol K) * (constant temperature) / (4.6 Torr)))Solving for Molar mass, we get:Molar mass = 323 g mol^-1Therefore, the molar mass of the unknown compound is 323 g mol^-1.

Question 15

Choose the solvent below that would show the greatest boiling point elevation when used to make a 0.10 mol kg^-1 nonelectrolyte solution.

Accepted Answer

The boiling point elevation is directly proportional to the molality (m) of the solution, which is in turn proportional to the number of moles of solute (n) divided by the mass of the solvent (m):
m = n / m
Since all the solvents have the same mass, the solvent with the greatest molality will have the greatest boiling point elevation. Therefore, we need to determine which solvent will have the greatest number of moles of solute for a given molality.
The molality of the solution is given as 0.10 mol kg-1, so for each solvent, we can calculate the number of moles of solute required to make a 1 kg solution:
A) CCl4: n = 0.10 mol
B) C16H16O: n = 0.10 mol
C) C26H22O2: n = 0.10 mol
D) C7H10O: n = 0.10 mol
E) CHCl3: n = 0.10 mol
Since all the solvents have the same molality of solute, the solvent with the greatest number of moles of solute will have the greatest boiling point elevation. Therefore, the solvent with the greatest molar mass will have the greatest number of moles of solute for a given molality. Solution A (CCl4) has the greatest molar mass, so it is the best choice.

Question 16

Calculate the freezing point of a solution of 500.0 g of ethylene glycol (C₂H₆O₂) dissolved in 500.0 g of water. K_f = 1.86 °C m^-1 and K_b = 0.512 °C m^-1.

Accepted Answer

The answer of Calculate the freezing point of a solution...

Question 17

Calculate the volume of solution that has a vapour pressure of 31.27 mbar and contains 84.3 g of sucrose, C₁₂H₂₂O₁₁, at a temperature of 25.0 °C. The vapour pressure of pure water at 25 °C is 31.7 mbar, the density of water is 1.00 g mL^-1, and assume no change in volume occurs upon dissolution.

Accepted Answer

The answer of Calculate the volume of solution that has...

Question 18

Determine the vapour pressure of a solution at 25 °C that contains 76.6 g of glucose (C₆H₁₂O₆) in 250.0 mL of water. The vapour pressure of pure water at 25 °C is 0.03173 bar.

Accepted Answer

The vapor pressure of the solution is calculated using Raoult's Law. First, find the mole fraction of water in the solution. The moles of glucose are 76.6 g / 180.18 g/mol = 0.425 mol. The moles of water are 250 g / 18.015 g/mol = 13.88 mol. The mole fraction of water is 13.88 / (13.88 + 0.425) = 0.970. The vapor pressure of the solution is 0.970 * 0.03173 bar = 0.0308 bar.

Question 19

Calculate the mass of maltose, C₁₂H₂₂O₁₁, contained in 725.0 mL of solution if the measured vapour pressure of the solution is 41.6 mbar at 30 °C. The vapour pressure of pure water at 30 °C is 42.40 mbar; assume no change in volume occurs upon dissolution.

Accepted Answer

The answer of Calculate the mass of maltose, C₁₂H₂₂O₁₁, contained...

Question 20

Determine the freezing point depression of a solution that contains 30.7 g glycerin (C₃H₈O₃, molar mass = 92.09 g mol^-1) in 376 mL of water. Some possibly useful constants for water are K_f = 1.86 °C m^-1 and K_b = 0.512 °C m^-1.

Accepted Answer

The answer of Determine the freezing point depression of a...

Quiz 12: Solutions

Place the following aqueous solutions of nonvolatile, nonionic compounds in order of decreasing osmotic pressure. I. 0.011 mol L^-1 sucrose II. 0.00095 mol L^-¹ glucose III. 0.0060 mol L^-1 glycerin

Calculate the boiling point of a solution of 500.0 g of ethylene glycol (C₂H₆O₂) dissolved in 500.0 g of water. K_f = 1.86 °C m^-1 and K_b = 0.512 °C m^-1. Use 100 °C as the boiling point of water.

The boiling point elevation of an aqueous sucrose solution is found to be 0.39 °C. What mass of sucrose (molar mass = 342.30 g mol^-1) would be needed to dissolve in 500.0 g of water? K_b (water) = 0.512 °C m^-1.

Calculate the mass of lactose, C₁₂H₂₂O₁₁, contained in 500.0 mL of solution if the measured vapour pressure of the solution is 121.2 mbar at 50 °C. The vapour pressure of pure water at 50 °C is 123.3 mbar; assume no change in volume occurs upon dissolution.

Determine the freezing point of a solution that contains 78.8 g of naphthalene (C₁₀H₈, molar mass = 128.16 g mol^-1) dissolved in 722 mL of benzene (d = 0.877 g mL^-1) . Pure benzene has a melting point of 5.50 °C and a freezing point depression constant of 4.90 °C m^-1.

Determine the vapour pressure of a solution at 55 °C that contains 34.2 g NaCl in 375 mL of water. The vapour pressure of pure water at 55 °C is 0.1574 bar.

Give the reason that antifreeze is added to a car radiator.

Calculate the vapour pressure of pure water at 85 °C if a 285 mL solution containing 173.0 g of mannose, C₆H₁₂O₆, has a vapour pressure of 545.0 mbar.

Determine the vapour pressure of a solution at 28 °C that contains 62.5 g of fructose (C₆H₁₂O₆) in 325.0 mL of water. The vapour pressure of pure water at 28 °C is 28.3 Torr.

Calculate the vapour pressure of pure water at 65 °C if a 465 mL solution containing 123.0 g of ribose, C₅H₁₀O₅, has a vapour pressure of 247.54 mbar. Assume no change in volume occurs upon dissolution.

Determine the boiling point of a solution that contains 78.8 g of naphthalene (C₁₀H₈, molar mass = 128.16 g mol^-1) dissolved in 722 mL of benzene (d = 0.877 g mL^-1) . Pure benzene has a boiling point of 80.1 °C and a boiling point elevation constant of 2.53 °C m^-1.

Choose the solvent below that would show the greatest boiling point elevation when used to make a 0.10 mol kg^-1 nonelectrolyte solution.

Calculate the freezing point of a solution of 500.0 g of ethylene glycol (C₂H₆O₂) dissolved in 500.0 g of water. K_f = 1.86 °C m^-1 and K_b = 0.512 °C m^-1.

Determine the vapour pressure of a solution at 25 °C that contains 76.6 g of glucose (C₆H₁₂O₆) in 250.0 mL of water. The vapour pressure of pure water at 25 °C is 0.03173 bar.

Calculate the mass of maltose, C₁₂H₂₂O₁₁, contained in 725.0 mL of solution if the measured vapour pressure of the solution is 41.6 mbar at 30 °C. The vapour pressure of pure water at 30 °C is 42.40 mbar; assume no change in volume occurs upon dissolution.

Determine the freezing point depression of a solution that contains 30.7 g glycerin (C₃H₈O₃, molar mass = 92.09 g mol^-1) in 376 mL of water. Some possibly useful constants for water are K_f = 1.86 °C m^-1 and K_b = 0.512 °C m^-1.

Quiz 12: Solutions

Place the following aqueous solutions of nonvolatile, nonionic compounds in order of decreasing osmotic pressure. I. 0.011 mol L-1 sucrose II. 0.00095 mol L-1 glucose III. 0.0060 mol L-1 glycerin

Calculate the boiling point of a solution of 500.0 g of ethylene glycol (C2H6O2) dissolved in 500.0 g of water. Kf = 1.86 °C m-1 and Kb = 0.512 °C m-1. Use 100 °C as the boiling point of water.

The boiling point elevation of an aqueous sucrose solution is found to be 0.39 °C. What mass of sucrose (molar mass = 342.30 g mol-1) would be needed to dissolve in 500.0 g of water? Kb (water) = 0.512 °C m-1.

Calculate the volume of solution that has a vapour pressure of 25.8 mbar and contains 200.3 g of galactose, C6H12O6, at a temperature of 22.0 °C. The vapour pressure of pure water at 22 °C is 26.40 mbar, the density of water is 1.00 g mL-1, and assume no change in volume occurs upon dissolution.

Calculate the mass of lactose, C12H22O11, contained in 500.0 mL of solution if the measured vapour pressure of the solution is 121.2 mbar at 50 °C. The vapour pressure of pure water at 50 °C is 123.3 mbar; assume no change in volume occurs upon dissolution.

Determine the freezing point of a solution that contains 78.8 g of naphthalene (C10H8, molar mass = 128.16 g mol-1) dissolved in 722 mL of benzene (d = 0.877 g mL-1) . Pure benzene has a melting point of 5.50 °C and a freezing point depression constant of 4.90 °C m-1.

Determine the vapour pressure of a solution at 55 °C that contains 34.2 g NaCl in 375 mL of water. The vapour pressure of pure water at 55 °C is 0.1574 bar.

Give the reason that antifreeze is added to a car radiator.

Calculate the vapour pressure of pure water at 85 °C if a 285 mL solution containing 173.0 g of mannose, C6H12O6, has a vapour pressure of 545.0 mbar.

Determine the vapour pressure of a solution at 28 °C that contains 62.5 g of fructose (C6H12O6) in 325.0 mL of water. The vapour pressure of pure water at 28 °C is 28.3 Torr.

Calculate the vapour pressure of pure water at 65 °C if a 465 mL solution containing 123.0 g of ribose, C5H10O5, has a vapour pressure of 247.54 mbar. Assume no change in volume occurs upon dissolution.

Determine the boiling point of a solution that contains 78.8 g of naphthalene (C10H8, molar mass = 128.16 g mol-1) dissolved in 722 mL of benzene (d = 0.877 g mL-1) . Pure benzene has a boiling point of 80.1 °C and a boiling point elevation constant of 2.53 °C m-1.

Choose the solvent below that would show the greatest boiling point elevation when used to make a 0.10 mol kg-1 nonelectrolyte solution.

Calculate the freezing point of a solution of 500.0 g of ethylene glycol (C2H6O2) dissolved in 500.0 g of water. Kf = 1.86 °C m-1 and Kb = 0.512 °C m-1.

Calculate the volume of solution that has a vapour pressure of 31.27 mbar and contains 84.3 g of sucrose, C12H22O11, at a temperature of 25.0 °C. The vapour pressure of pure water at 25 °C is 31.7 mbar, the density of water is 1.00 g mL-1, and assume no change in volume occurs upon dissolution.

Determine the vapour pressure of a solution at 25 °C that contains 76.6 g of glucose (C6H12O6) in 250.0 mL of water. The vapour pressure of pure water at 25 °C is 0.03173 bar.

Calculate the mass of maltose, C12H22O11, contained in 725.0 mL of solution if the measured vapour pressure of the solution is 41.6 mbar at 30 °C. The vapour pressure of pure water at 30 °C is 42.40 mbar; assume no change in volume occurs upon dissolution.

Determine the freezing point depression of a solution that contains 30.7 g glycerin (C3H8O3, molar mass = 92.09 g mol-1) in 376 mL of water. Some possibly useful constants for water are Kf = 1.86 °C m-1 and Kb = 0.512 °C m-1.

Place the following aqueous solutions of nonvolatile, nonionic compounds in order of decreasing osmotic pressure. I. 0.011 mol L^-1 sucrose II. 0.00095 mol L^-¹ glucose III. 0.0060 mol L^-1 glycerin

Calculate the boiling point of a solution of 500.0 g of ethylene glycol (C₂H₆O₂) dissolved in 500.0 g of water. K_f = 1.86 °C m^-1 and K_b = 0.512 °C m^-1. Use 100 °C as the boiling point of water.

The boiling point elevation of an aqueous sucrose solution is found to be 0.39 °C. What mass of sucrose (molar mass = 342.30 g mol^-1) would be needed to dissolve in 500.0 g of water? K_b (water) = 0.512 °C m^-1.

Calculate the mass of lactose, C₁₂H₂₂O₁₁, contained in 500.0 mL of solution if the measured vapour pressure of the solution is 121.2 mbar at 50 °C. The vapour pressure of pure water at 50 °C is 123.3 mbar; assume no change in volume occurs upon dissolution.

Determine the freezing point of a solution that contains 78.8 g of naphthalene (C₁₀H₈, molar mass = 128.16 g mol^-1) dissolved in 722 mL of benzene (d = 0.877 g mL^-1) . Pure benzene has a melting point of 5.50 °C and a freezing point depression constant of 4.90 °C m^-1.

Calculate the vapour pressure of pure water at 85 °C if a 285 mL solution containing 173.0 g of mannose, C₆H₁₂O₆, has a vapour pressure of 545.0 mbar.

Determine the vapour pressure of a solution at 28 °C that contains 62.5 g of fructose (C₆H₁₂O₆) in 325.0 mL of water. The vapour pressure of pure water at 28 °C is 28.3 Torr.

Calculate the vapour pressure of pure water at 65 °C if a 465 mL solution containing 123.0 g of ribose, C₅H₁₀O₅, has a vapour pressure of 247.54 mbar. Assume no change in volume occurs upon dissolution.

Determine the boiling point of a solution that contains 78.8 g of naphthalene (C₁₀H₈, molar mass = 128.16 g mol^-1) dissolved in 722 mL of benzene (d = 0.877 g mL^-1) . Pure benzene has a boiling point of 80.1 °C and a boiling point elevation constant of 2.53 °C m^-1.

Choose the solvent below that would show the greatest boiling point elevation when used to make a 0.10 mol kg^-1 nonelectrolyte solution.

Calculate the freezing point of a solution of 500.0 g of ethylene glycol (C₂H₆O₂) dissolved in 500.0 g of water. K_f = 1.86 °C m^-1 and K_b = 0.512 °C m^-1.

Determine the vapour pressure of a solution at 25 °C that contains 76.6 g of glucose (C₆H₁₂O₆) in 250.0 mL of water. The vapour pressure of pure water at 25 °C is 0.03173 bar.

Calculate the mass of maltose, C₁₂H₂₂O₁₁, contained in 725.0 mL of solution if the measured vapour pressure of the solution is 41.6 mbar at 30 °C. The vapour pressure of pure water at 30 °C is 42.40 mbar; assume no change in volume occurs upon dissolution.

Determine the freezing point depression of a solution that contains 30.7 g glycerin (C₃H₈O₃, molar mass = 92.09 g mol^-1) in 376 mL of water. Some possibly useful constants for water are K_f = 1.86 °C m^-1 and K_b = 0.512 °C m^-1.