Question 1

In order to calculate the molality of a solution from its molarity, what other information would be needed?

Accepted Answer

To calculate molality, we need to know the amount of solute (in moles) per kg of solvent. We already have the molarity (moles of solute per liter of solution), but we need to know the density of the solution to convert the volume of solution to mass of solvent. The molar mass of the solute is also needed to convert the number of moles to mass. Therefore, we need the molar mass of solute and density of solution.

Question 2

The osmotic pressure of a solution of Mg(NO₃)₂ at a given temperature is ____ that of a solution of NaNO₃ of identical concentration at the same temperature.

Accepted Answer

The answer of The osmotic pressure of a solution of...

Question 3

Explain what is meant by
a. osmosis.
b. osmotic pressure.
c. reverse osmosis.

Accepted Answer

The answer of Explain what is meant by
a. osmosis.
b. osmotic...

Question 4

Osmotic pressure is the

Accepted Answer

Osmotic pressure is the pressure that must be applied to a solution in order to prevent osmosis from the pure solvent. It is the pressure required to stop the flow of solvent molecules into a solution through a semipermeable membrane. Therefore, option A is the correct choice.

Question 5

A coolant consisting of a 50/50 mixture by volume of ethylene glycol and water utilizes the

Accepted Answer

The mixture of ethylene glycol and water in a coolant utilizes both colligative properties (such as boiling point elevation and freezing point depression) and the boiling point elevation constant of water. Therefore, both choice A and C are correct, making E the best choice. The boiling point depression constant of water (choice D) is not relevant in this scenario as the coolant is designed to prevent overheating, not to lower the boiling point of water.

Question 6

Given that the value of k_f for water is 1.86^$\circ$C/m, what is the freezing point of an aqueous solution of NaCl prepared by mixing 427.0 g solute with 1.000 kg of water?

Accepted Answer

First, we need to calculate the molality of the solution: molality = moles of solute/kg of solvent To get moles of solute, we need to use the given mass and molar mass of NaCl: moles of NaCl = 427.0 g / 58.44 g/mol = 7.318 mol Now we can calculate the molality: molality = 7.318 mol / 1.000 kg = 7.318 m Next, we can use the equation: ΔTf = -kfm where ΔTf is the freezing point depression, kf is the freezing point depression constant (given as k_f for water), and m is the molality of the solution. Plugging in the values: ΔTf = -(1.86 °C/m) * (7.318 m) = -13.6 °C Finally, we can calculate the freezing point of the solution: freezing point = 0 °C - ΔTf = 0 °C - (-13.6 °C) = -13.6 °C = -13.6 F1F1F1S1F1F1F10C

Question 7

Drinkable water can be produced from seawater by the process of ____, using a membrane which is permeable to ____ but not to ____.

Accepted Answer

Reverse osmosis is the process in which seawater is forced through a membrane that allows water molecules to pass through, but not ions like sodium and chloride. This results in the production of drinkable water from seawater. Option A is incorrect because osmosis uses a semi-permeable membrane to allow water to pass through from an area of low solute concentration to an area of high solute concentration. Option C is incorrect because the membrane is permeable to water and not ions. Option D is also incorrect because osmosis does not use a membrane that is permeable to ions. Option E is almost correct, but the membrane is actually permeable to water and not ions.

Question 8

The freezing points of the following aqueous solutions, from highest to lowest, are:

Accepted Answer

The answer of The freezing points of the following aqueous...

Question 9

The driving force for osmosis is

Accepted Answer

The driving force for osmosis is entropy, as osmosis is a spontaneous process driven by the increase in entropy when a solvent moves from a region of low solute concentration to a region of high solute concentration through a semipermeable membrane.

Question 10

In living systems, a solution with a higher solute concentration than the surrounding cells is said to be ____. This causes water to flow ____ the cells by osmosis.

Accepted Answer

A solution with a higher solute concentration than the surrounding cells is hypertonic. This causes water to flow out of the cells by osmosis. This can cause the cells to shrink or even die if they lose too much water.

Question 11

What is the vapor pressure of a 45.0 % solution of glucose, C₆H₁₂O₆, at 90.0^$\circ$C, given that the vapor pressure of pure water at that temperature is 526 mm Hg?

Accepted Answer

To find the vapor pressure of the solution, we can use Raoult's Law, which states that the vapor pressure of a solution is equal to the mole fraction of the solvent times the vapor pressure of the pure solvent. Since glucose is a non-volatile solute, it will not contribute to the vapor pressure directly. The mole fraction of water (solvent) can be calculated by considering the percentage of the solution that is water, which is 100% - 45% = 55%. Assuming ideal behavior and that the percentage is a rough approximation of the mole fraction (which is a simplification because the question does not provide enough information to calculate exact mole fractions), the vapor pressure of the solution is approximately 55% of the vapor pressure of pure water. Therefore, 0.55 * 526 mm Hg = 289.3 mm Hg, which is closest to option A, 486 mm Hg, given the options provided. However, it seems there might be a misunderstanding in the calculation or the interpretation of the options. Based on the calculation, none of the options accurately match, indicating a potential error in the explanation or a misinterpretation of the question's requirements. The correct approach involves using Raoult's Law and the given data, but the precise answer seems to be mismatched with the provided options.

Question 12

A 0.1 M solution of Na₂SO₄ contains

Accepted Answer

A 0.1 M solution of Na₂SO₄ contains 0.1 M of SO₄^2-, 0.2 M of Na⁺, 14.2 g/L of sodium sulfate, and 0.3 mol/L of ions.

Question 13

Consider these three primary alcohols:
  The three alcohols have similar molecular structures. However, their solubilities in water decrease dramatically, in the order shown. Explain this.

Accepted Answer

The answer of Consider these three primary alcohols:
  The...

Question 14

The solubility in water of magnesium fluoride, MgF₂, is 7.3 mg/100 mL. Is a solution containing 33 mg MgF₂ in 475 mL water unsaturated, saturated, or supersaturated? Show a calculation to support your answer.

Accepted Answer

The answer of The solubility in water of magnesium fluoride,...

Question 15

Calculate the boiling point of a mixture where 95.0 g of formic acid, H₂CO₂, is dissolved in 250 g of acetic acid. Acetic acid has a K_b of 2.93^$\circ$C/m and boils at 118^$\circ$C. Assume that formic acid does not ionize when dissolved in acetic acid, and that formic acid is non-volatile.

Accepted Answer

The answer of Calculate the boiling point of a mixture...

Question 16

An aqueous solution of phosphoric acid, H₃PO₄, contains 285 g H₃PO₄ in 400 mL solution, and has a density of 1.35 g/mL. Calculate a. the weight % in this solution. b. The concentration in mol/L of this solution.

Accepted Answer

The answer of An aqueous solution of phosphoric acid, H₃PO₄,...

Question 17

An aqueous solution at 27^$\circ$C contains 3.60 g of a protein in a 200. mL sample. The osmotic pressure is 0.0203 atm. What is the molar mass of the protein?

Accepted Answer

The molar mass of the protein can be calculated using the formula for osmotic pressure: $\pi = \frac{n}{V}RT$, where $\pi$ is the osmotic pressure, $n$ is the number of moles of solute, $V$ is the volume of solution in liters, $R$ is the gas constant (0.0821 L·atm/(K·mol)), and $T$ is the temperature in Kelvin. First, convert the temperature to Kelvin (273.15 + 10 = 283.15 K) and the volume to liters (200 mL = 0.200 L). The number of moles $n$ can be found by rearranging the formula to $n = \pi V / RT$. Substituting the given values, $n = (0.0203 atm \times 0.200 L) / (0.0821 L·atm/(K·mol) \times 283.15 K)$. The molar mass (M) is then the mass of the protein divided by the number of moles calculated. Given the mass of the protein is 3.60 g, the calculation will yield a molar mass in the range of $10^4$ g/mol, matching option E.

Quiz 14: The Chemistry of Solutes and Solutions

In order to calculate the molality of a solution from its molarity, what other information would be needed?

The osmotic pressure of a solution of Mg(NO₃) ₂ at a given temperature is ____ that of a solution of NaNO₃ of identical concentration at the same temperature.

Explain what is meant by a. osmosis. b. osmotic pressure. c. reverse osmosis.

Osmotic pressure is the

A coolant consisting of a 50/50 mixture by volume of ethylene glycol and water utilizes the

Given that the value of k_f for water is 1.86^$\circ$C/m, what is the freezing point of an aqueous solution of NaCl prepared by mixing 427.0 g solute with 1.000 kg of water?

Drinkable water can be produced from seawater by the process of , using a membrane which is permeable to but not to .

The freezing points of the following aqueous solutions, from highest to lowest, are:

The driving force for osmosis is

In living systems, a solution with a higher solute concentration than the surrounding cells is said to be . This causes water to flow the cells by osmosis.

What is the vapor pressure of a 45.0 % solution of glucose, C₆H₁₂O₆, at 90.0^$\circ$C, given that the vapor pressure of pure water at that temperature is 526 mm Hg?

A 0.1 M solution of Na₂SO₄ contains

Consider these three primary alcohols: The three alcohols have similar molecular structures. However, their solubilities in water decrease dramatically, in the order shown. Explain this.

The solubility in water of magnesium fluoride, MgF₂, is 7.3 mg/100 mL. Is a solution containing 33 mg MgF₂ in 475 mL water unsaturated, saturated, or supersaturated? Show a calculation to support your answer.

Calculate the boiling point of a mixture where 95.0 g of formic acid, H₂CO₂, is dissolved in 250 g of acetic acid. Acetic acid has a K_b of 2.93^$\circ$C/m and boils at 118^$\circ$C. Assume that formic acid does not ionize when dissolved in acetic acid, and that formic acid is non-volatile.

An aqueous solution of phosphoric acid, H₃PO₄, contains 285 g H₃PO₄ in 400 mL solution, and has a density of 1.35 g/mL. Calculate a. the weight % in this solution. b. The concentration in mol/L of this solution.

An aqueous solution at 27^$\circ$C contains 3.60 g of a protein in a 200. mL sample. The osmotic pressure is 0.0203 atm. What is the molar mass of the protein?

Quiz 14: The Chemistry of Solutes and Solutions

In order to calculate the molality of a solution from its molarity, what other information would be needed?

The osmotic pressure of a solution of Mg(NO3) 2 at a given temperature is ____ that of a solution of NaNO3 of identical concentration at the same temperature.

Explain what is meant by a. osmosis. b. osmotic pressure. c. reverse osmosis.

Osmotic pressure is the

A coolant consisting of a 50/50 mixture by volume of ethylene glycol and water utilizes the

Given that the value of kf for water is 1.86 ∘\circ∘ C/m, what is the freezing point of an aqueous solution of NaCl prepared by mixing 427.0 g solute with 1.000 kg of water?

Drinkable water can be produced from seawater by the process of ____, using a membrane which is permeable to ____ but not to ____.

The freezing points of the following aqueous solutions, from highest to lowest, are:

The driving force for osmosis is

In living systems, a solution with a higher solute concentration than the surrounding cells is said to be ____. This causes water to flow ____ the cells by osmosis.

What is the vapor pressure of a 45.0 % solution of glucose, C6H12O6, at 90.0 ∘\circ∘ C, given that the vapor pressure of pure water at that temperature is 526 mm Hg?

A 0.1 M solution of Na2SO4 contains

Consider these three primary alcohols: The three alcohols have similar molecular structures. However, their solubilities in water decrease dramatically, in the order shown. Explain this.

The solubility in water of magnesium fluoride, MgF2, is 7.3 mg/100 mL. Is a solution containing 33 mg MgF2 in 475 mL water unsaturated, saturated, or supersaturated? Show a calculation to support your answer.

An aqueous solution of phosphoric acid, H3PO4, contains 285 g H3PO4 in 400 mL solution, and has a density of 1.35 g/mL. Calculate a. the weight % in this solution. b. The concentration in mol/L of this solution.

An aqueous solution at 27 ∘\circ∘ C contains 3.60 g of a protein in a 200. mL sample. The osmotic pressure is 0.0203 atm. What is the molar mass of the protein?

The osmotic pressure of a solution of Mg(NO₃) ₂ at a given temperature is ____ that of a solution of NaNO₃ of identical concentration at the same temperature.

Given that the value of k_f for water is 1.86^$\circ$C/m, what is the freezing point of an aqueous solution of NaCl prepared by mixing 427.0 g solute with 1.000 kg of water?

Drinkable water can be produced from seawater by the process of , using a membrane which is permeable to but not to .

In living systems, a solution with a higher solute concentration than the surrounding cells is said to be . This causes water to flow the cells by osmosis.

What is the vapor pressure of a 45.0 % solution of glucose, C₆H₁₂O₆, at 90.0^$\circ$C, given that the vapor pressure of pure water at that temperature is 526 mm Hg?

A 0.1 M solution of Na₂SO₄ contains

The solubility in water of magnesium fluoride, MgF₂, is 7.3 mg/100 mL. Is a solution containing 33 mg MgF₂ in 475 mL water unsaturated, saturated, or supersaturated? Show a calculation to support your answer.

An aqueous solution of phosphoric acid, H₃PO₄, contains 285 g H₃PO₄ in 400 mL solution, and has a density of 1.35 g/mL. Calculate a. the weight % in this solution. b. The concentration in mol/L of this solution.

An aqueous solution at 27^$\circ$C contains 3.60 g of a protein in a 200. mL sample. The osmotic pressure is 0.0203 atm. What is the molar mass of the protein?