Colligative Properties - MCAT Chemical and Physical Foundations of Biological Systems
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Which of the following aqueous solutions will have the highest boiling point?
Which of the following aqueous solutions will have the highest boiling point?
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In order to answer this problem, consider the equation for boiling point elevation: 
.
is a specific constant for the boiling substance, so it will not change between the solutions (they are all aqueous). Molality is designated as "m", and a high molality will result in a higher boiling point, however, the value we want to look at for this problem is 
, which is also known as the van't Hoff factor. The van't Hoff factor is the number of particles that a single solute will dissociate into when added to a solution. MgCl2 will dissociate into three particles: 1 Mg2+ cation and 2 Cl- anions. Since 2m of MgCl2 has the highest molality as well as the largest van't Hoff factor out of the options, it will result in the highest boiling point.
In order to answer this problem, consider the equation for boiling point elevation:
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The equation for boiling point elevation is written as 
.
The "
" value in the equation is referred to as the van't Hoff factor, and is the number of particles that the solute is expected to dissociate into once in solution. In ideal solutions, ions will separate entirely, and the van't Hoff factor will be the expected value; however, nonideal solutions can have ion pairing take place, where ions do not separate entirely. As a result, the observed van't Hoff factor will be slightly less than the expected van't Hoff factor.
If a solution has ion pairing taking place, which statement is true?
The equation for boiling point elevation is written as
The "
If a solution has ion pairing taking place, which statement is true?
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If there is ion pairing taking place in a solution, the van't Hoff factor will be slightly lower than predicted. As a result, the boiling point will not be as elevated as it would be if all of the ions were separated from each other. This conclusion can be draw from the given equation, 
. The number of particles in the solution does not affect the molality.
If there is ion pairing taking place in a solution, the van't Hoff factor will be slightly lower than predicted. As a result, the boiling point will not be as elevated as it would be if all of the ions were separated from each other. This conclusion can be draw from the given equation,
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Two moles of sodium chloride (NaCl) are added to 1kg of a mystery solvent. The addition of the NaCl caused an increase of 6K to the solvent's boiling point.
Based on this information, what is the boiling constant for the solvent?
Two moles of sodium chloride (NaCl) are added to 1kg of a mystery solvent. The addition of the NaCl caused an increase of 6K to the solvent's boiling point.
Based on this information, what is the boiling constant for the solvent?
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In order to solve this problem, we can use the boiling point elevation equation: 
.
We know the temperature change, we can compute molality from the given information, and we know the van't Hoff factor (expected to be 2 in this scenario due to NaCl becoming 2 ions in solution). We can calculate the boiling point constant for the solvent.
In order to solve this problem, we can use the boiling point elevation equation:
We know the temperature change, we can compute molality from the given information, and we know the van't Hoff factor (expected to be 2 in this scenario due to NaCl becoming 2 ions in solution). We can calculate the boiling point constant for the solvent.
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Suppose two containers each contain the same amount of solvent. 2m NaCl solution is added to the first container, and a mystery solution is added to the second container. Upon heating the flasks, it is determined that the second container has a higher boiling point than the first container. Assume the solutions are ideal.
Based on the above information, which of the following compounds could have been added to container 2?
Suppose two containers each contain the same amount of solvent. 2m NaCl solution is added to the first container, and a mystery solution is added to the second container. Upon heating the flasks, it is determined that the second container has a higher boiling point than the first container. Assume the solutions are ideal.
Based on the above information, which of the following compounds could have been added to container 2?
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Based on the equation 
, we see that there are two factors that differ between the containers and can affect the elevation of the boiling point: molality and the van't Hoff factor (
).
The sodium choride added to container 1 has a molality of 2, as well as a van't Hoff factor of 2. As a result, we are looking for a compound that has a larger combination of these two factors, which would cause a higher boiling point. 2m CaF2 has a molality of 2 and a van't Hoff factor of 3. Since this combination of factors in container 2 would be higher than the combination in container 1, we can conclude that this was the mystery compound added to the container with the higher boiling point.
Note that C6H12O6 is the formula for glucose, and will not ionize in solution.
Based on the equation
The sodium choride added to container 1 has a molality of 2, as well as a van't Hoff factor of 2. As a result, we are looking for a compound that has a larger combination of these two factors, which would cause a higher boiling point. 2m CaF2 has a molality of 2 and a van't Hoff factor of 3. Since this combination of factors in container 2 would be higher than the combination in container 1, we can conclude that this was the mystery compound added to the container with the higher boiling point.
Note that C6H12O6 is the formula for glucose, and will not ionize in solution.
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Boiling point is the temperature a liquid needs to achieve in order to begin its transformation into a gaseous state. Campers and hikers who prepare food during their trips have to account for differences in atmospheric pressure as they ascend in elevation. During the ascent, the decrease in atmospheric pressure changes the temperature at which water boils.
Further complicating the matter is the observation that addition of a solute to a pure liquid also changes the boiling point. Raoult’s Law can be used to understand the changes in boiling point if a non-volatile solute is present, as expressed here.
In this law, 
is the mole fraction of the solvent, 
is the vapor pressure of the pure solvent, and 
is the vapor pressure of the solution. When this vapor pressure is equal to the local atmospheric pressure, the solution boils.
The change in boiling point with addition of a solute is a colligative property of a solution. Which of the following are also examples of colligative properties?
I. Vapor pressure reduction
II. Color emission with dissolution of a solute
III. Osmotic pressure
Boiling point is the temperature a liquid needs to achieve in order to begin its transformation into a gaseous state. Campers and hikers who prepare food during their trips have to account for differences in atmospheric pressure as they ascend in elevation. During the ascent, the decrease in atmospheric pressure changes the temperature at which water boils.
Further complicating the matter is the observation that addition of a solute to a pure liquid also changes the boiling point. Raoult’s Law can be used to understand the changes in boiling point if a non-volatile solute is present, as expressed here.
In this law,
The change in boiling point with addition of a solute is a colligative property of a solution. Which of the following are also examples of colligative properties?
I. Vapor pressure reduction
II. Color emission with dissolution of a solute
III. Osmotic pressure
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Colligative properties are defined as properties that depend entirely upon the ratio of the number of solute particles to the number of solvent particles. Only osmotic pressure and vapor pressure depression are examples of such phenomena. While color emission is a property of a solution, it depends on the chemical species involved, and not the number of particles.
Colligative properties are defined as properties that depend entirely upon the ratio of the number of solute particles to the number of solvent particles. Only osmotic pressure and vapor pressure depression are examples of such phenomena. While color emission is a property of a solution, it depends on the chemical species involved, and not the number of particles.
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Boiling point is the temperature a liquid needs to achieve in order to begin its transformation into a gaseous state. Campers and hikers who prepare food during their trips have to account for differences in atmospheric pressure as they ascend in elevation. During the ascent, the decrease in atmospheric pressure changes the temperature at which water boils.
Further complicating the matter is the observation that addition of a solute to a pure liquid also changes the boiling point. Raoult’s Law can be used to understand the changes in boiling point if a non-volatile solute is present, as expressed here.
In this law, 
is the mole fraction of the solvent, 
is the vapor pressure of the pure solvent, and 
is the vapor pressure of the solution. When this vapor pressure is equal to the local atmospheric pressure, the solution boils.
Two campers are preparing food at an altitude of 13,000 feet on a mountain in Colorado. Which of the following is true as they boil a pot of water?
Boiling point is the temperature a liquid needs to achieve in order to begin its transformation into a gaseous state. Campers and hikers who prepare food during their trips have to account for differences in atmospheric pressure as they ascend in elevation. During the ascent, the decrease in atmospheric pressure changes the temperature at which water boils.
Further complicating the matter is the observation that addition of a solute to a pure liquid also changes the boiling point. Raoult’s Law can be used to understand the changes in boiling point if a non-volatile solute is present, as expressed here.
In this law,
Two campers are preparing food at an altitude of 13,000 feet on a mountain in Colorado. Which of the following is true as they boil a pot of water?
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The local atmospheric pressure at 13,000 feet is less than the pressure at sea level; therefore, it takes less heat to make the vapor pressure meet the local atmospheric pressure. Heat added to the system easily exits again as the water is converted to steam, leaving less heat in the water to cook the food. Food cooks more slowly as a result.
The local atmospheric pressure at 13,000 feet is less than the pressure at sea level; therefore, it takes less heat to make the vapor pressure meet the local atmospheric pressure. Heat added to the system easily exits again as the water is converted to steam, leaving less heat in the water to cook the food. Food cooks more slowly as a result.
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Which solution will have a higher boiling point?
Solution 1: 
in 
water
Solution 2: 
in 
water
Which solution will have a higher boiling point?
Solution 1:
Solution 2:
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Adding solute to water will result in boiling point elevation due to the presence of more molecules. Change in temperature is given by the relation 
, where 
is a constant for the solvent, 
is the solution molality, and 
is the van't Hoff factor. In this example, the molalities are equal.
Since 
dissociates into 
and 
, 
, representing the two ions derived from each molecule. For glucose 
, as the molecule does not dissociate. Solution 1 will have a higher elevation in temperature due to the greater number of ions in solution.
Adding solute to water will result in boiling point elevation due to the presence of more molecules. Change in temperature is given by the relation
Since
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Which of the following compounds will create the greatest increase in boiling point when added to an aqueous solution?
Which of the following compounds will create the greatest increase in boiling point when added to an aqueous solution?
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Colligative properties are dependent only on the number of particles in a solution, and not their identity. Some examples of colligative properties are vapor pressure, boiling point, freezing point, and osmotic pressure.
There is a direct relationship between the boiling point elevation and the number of particles present in a solution. The more particles that are present in solution, the higher the boiling point elevation.
We are looking for the compound that will create the greatest number of ions when dissolved in solution.
Sodium chloride and magnesium sulfate will produce two ions per mole. 
Magnesium chloride and barium chloride will produce three ions per mole. 
Calcium hydroxide will also produce three ions per mole, but we are given two moles instead of one. 
Calcium hydroxide will produce the greatest number of ions, thus creating the greatest increase in boiling point elevation.
Colligative properties are dependent only on the number of particles in a solution, and not their identity. Some examples of colligative properties are vapor pressure, boiling point, freezing point, and osmotic pressure.
There is a direct relationship between the boiling point elevation and the number of particles present in a solution. The more particles that are present in solution, the higher the boiling point elevation.
We are looking for the compound that will create the greatest number of ions when dissolved in solution.
Sodium chloride and magnesium sulfate will produce two ions per mole.
Magnesium chloride and barium chloride will produce three ions per mole.
Calcium hydroxide will also produce three ions per mole, but we are given two moles instead of one.
Calcium hydroxide will produce the greatest number of ions, thus creating the greatest increase in boiling point elevation.
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The values for normal boiling and freezing points, along with 
and 
values are given below for select solvents.
of ammonium phosphate are dissolved in 
of water. What is the boiling point of this solution at 
?
The values for normal boiling and freezing points, along with
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We first need to find the boiling point elevation with the equation:
Ammonium phosphate has an van't Hoff value of four; each molecule dissociates into four ions in solution. To calculate the molality, we need to find moles of solute per kilogram of solution.
Next, use the molality, van't Hoff factor, and boiling point elevation constant to solve for the increase in boiling point.
Add this increase to the boiling point of pure water to find the boiling point of the solution.
We first need to find the boiling point elevation with the equation:
Ammonium phosphate has an van't Hoff value of four; each molecule dissociates into four ions in solution. To calculate the molality, we need to find moles of solute per kilogram of solution.
Next, use the molality, van't Hoff factor, and boiling point elevation constant to solve for the increase in boiling point.
Add this increase to the boiling point of pure water to find the boiling point of the solution.
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The values for normal boiling and freezing points, along with 
and 
values are given below for select solvents.
A 
solution of which of the following compositions would result in the greatest boiling point elevation?
The values for normal boiling and freezing points, along with
A
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Boiling point elevation depends on three variables: the boiling point elevation constant of the solvent, the van't Hoff factor of the solute, and the molality of the solution. In this question, molality is held constant.
First, calculate the van't Hoff for each compound.
Ultimately, we are looking for the greatest product of the boiling point elevation constant and van't Hoff factor (since molality is constant).
Magnesium phosphide has the greater van't Hoff factor and acetic acid has the greater boiling point elevation constant. A solution of magnesium phosphide in acetic acid will thus have the greatest boiling point elevation.
Boiling point elevation depends on three variables: the boiling point elevation constant of the solvent, the van't Hoff factor of the solute, and the molality of the solution. In this question, molality is held constant.
First, calculate the van't Hoff for each compound.
Ultimately, we are looking for the greatest product of the boiling point elevation constant and van't Hoff factor (since molality is constant).
Magnesium phosphide has the greater van't Hoff factor and acetic acid has the greater boiling point elevation constant. A solution of magnesium phosphide in acetic acid will thus have the greatest boiling point elevation.
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Colligative properties are properties of compounds that are altered by the amount of substance present. There are four main colligative properties: boiling point, freezing point, vapor pressure, and osmotic pressure. The change in each of these properties can be calculated using the amount of molecules/ions present in solution and the concentration or partial pressure of the compound. The boiling point is defined as the temperature at which the vapor pressure equals the atmospheric pressure. The freezing point is the temperature at which a liquid is converted to a solid. Vapor pressure is the pressure produced by the vapor above a solution. Osmotic pressure is the pressure required to prevent flow of water into a solution (across a membrane).
Which of the following is true regarding the boiling point of a sodium chloride solution and calcium chloride solution?
Colligative properties are properties of compounds that are altered by the amount of substance present. There are four main colligative properties: boiling point, freezing point, vapor pressure, and osmotic pressure. The change in each of these properties can be calculated using the amount of molecules/ions present in solution and the concentration or partial pressure of the compound. The boiling point is defined as the temperature at which the vapor pressure equals the atmospheric pressure. The freezing point is the temperature at which a liquid is converted to a solid. Vapor pressure is the pressure produced by the vapor above a solution. Osmotic pressure is the pressure required to prevent flow of water into a solution (across a membrane).
Which of the following is true regarding the boiling point of a sodium chloride solution and calcium chloride solution?
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Recall that the boiling point of a solution depends on the number of ions in the solution and the concentration of the solution. Increase in both of these factors will elevate the boiling point to higher temperatures. The equation describing this is given below.
where 
is change in boiling point, 
is the boiling point elevation constant, 
is the number of ions, and 
is the molality. Sodium chloride, or 
, will produce two ions in solution whereas calcium chloride, or 
, will produce three ions. If the concentrations were the same, the calcium chloride solution would have a higher boiling point; however, since we are not given the concentration we cannot determine the relative boiling points of the solution.
Recall that the boiling point of a solution depends on the number of ions in the solution and the concentration of the solution. Increase in both of these factors will elevate the boiling point to higher temperatures. The equation describing this is given below.
where
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Colligative properties are properties of compounds that are altered by the amount of substance present. There are four main colligative properties: boiling point, freezing point, vapor pressure, and osmotic pressure. The change in each of these properties can be calculated using the amount of molecules/ions present in solution and the concentration or partial pressure of the compound. The boiling point is defined as the temperature at which the vapor pressure equals the atmospheric pressure. The freezing point is the temperature at which a liquid is converted to a solid. Vapor pressure is the pressure produced by the vapor above a solution. Osmotic pressure is the pressure required to prevent flow of water into a solution (across a membrane).
How does the boiling point of a solution change after adding 
potassium bromide? The solution has a density of 
and 
.
Colligative properties are properties of compounds that are altered by the amount of substance present. There are four main colligative properties: boiling point, freezing point, vapor pressure, and osmotic pressure. The change in each of these properties can be calculated using the amount of molecules/ions present in solution and the concentration or partial pressure of the compound. The boiling point is defined as the temperature at which the vapor pressure equals the atmospheric pressure. The freezing point is the temperature at which a liquid is converted to a solid. Vapor pressure is the pressure produced by the vapor above a solution. Osmotic pressure is the pressure required to prevent flow of water into a solution (across a membrane).
How does the boiling point of a solution change after adding
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Recall that adding solutes to a solution increases the boiling point. This phenomenon is called the boiling point elevation. Knowing this information, we can eliminate two choices immediately. The equation to calculate the boiling point elevation is as follows.
where 
is change in boiling point, 
is the boiling point elevation constant, 
is the number of ions, and 
is the molality. The question gives us the concentration in molarity; therefore, we need to convert the concentration to molality.
Molarity = 
Molality = 
We need to find the mass of solvent in kilograms. The molarity is 
; therefore, let’s assume we have 
of solute and 
of solution. The density of the solution is 
or 
. We can calculate the mass of the total solution using density.
mass of total solution = 
We need the mass of the solvent only. To find this, we need to first calculate the mass of solute. The MW of potassium bromide is 
(this can be calculated by obtaining values from the periodic table). We have 
of solute; therefore, the mass of solute is
This means that the mass of solvent is equal to:
mass of solvent = total mass of solution - mass of solute = 
= 
Molality of solution is
, or the number of ions, for 
is 2 (because 
will produce two ions in solution). Now we have all the information to calculate the boiling point elevation.
Therefore, boiling point increases by 
.
Recall that adding solutes to a solution increases the boiling point. This phenomenon is called the boiling point elevation. Knowing this information, we can eliminate two choices immediately. The equation to calculate the boiling point elevation is as follows.
where
Molarity =
Molality =
We need to find the mass of solvent in kilograms. The molarity is
mass of total solution =
We need the mass of the solvent only. To find this, we need to first calculate the mass of solute. The MW of potassium bromide is
This means that the mass of solvent is equal to:
mass of solvent = total mass of solution - mass of solute =
Molality of solution is
Therefore, boiling point increases by
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What is the freezing point of a 3m solution of K2SO4 in water? (kf = 1.9oC/mol)
What is the freezing point of a 3m solution of K2SO4 in water? (kf = 1.9oC/mol)
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Freezing point depression is given by the equation 
.
i is the Vant Hoff Factor that tells us how many particles (often ions) a solid produces when dissolved in solution. m is the molality of the solution. kf is the freezing point constant.
The question gives us m as 3mol, kf as 1.9, and i is found to be 3 (2K+ and SO42- ). Whe then plug the values into the equation.
Freezing point depression is given by the equation
i is the Vant Hoff Factor that tells us how many particles (often ions) a solid produces when dissolved in solution. m is the molality of the solution. kf is the freezing point constant.
The question gives us m as 3mol, kf as 1.9, and i is found to be 3 (2K+ and SO42- ). Whe then plug the values into the equation.
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The city of New York is developing a new salt substitute to distribute on the streets during icy weather. Which solution would be the most useful for this purpose?
The city of New York is developing a new salt substitute to distribute on the streets during icy weather. Which solution would be the most useful for this purpose?
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The key to understanding this problem is realizing that it is asking about freezing point depression, or colligative properties. The main factor that concerns freezing point depression is the number of particles in solution, rather than other features, such as size or weight. The more solute dissolved, the greater the freezing point depression will be, meaning that a colder temperature will be needed for a solution to freeze.
In our answer choices we are looking for the solute that is dissociate into the greatest number of ions, or has the highest van't Hoff factor. Magnesium chloride and calcium bromide both generate three moles of ions per mole of solute. The answer choice with magnesium chloride is more concentrated, however, making this the correct option.
The key to understanding this problem is realizing that it is asking about freezing point depression, or colligative properties. The main factor that concerns freezing point depression is the number of particles in solution, rather than other features, such as size or weight. The more solute dissolved, the greater the freezing point depression will be, meaning that a colder temperature will be needed for a solution to freeze.
In our answer choices we are looking for the solute that is dissociate into the greatest number of ions, or has the highest van't Hoff factor. Magnesium chloride and calcium bromide both generate three moles of ions per mole of solute. The answer choice with magnesium chloride is more concentrated, however, making this the correct option.
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Five solutions are made, each comprised of 1L of water and 1mol of C6H12O6, NaCl, H2SO4, Al(NO3)3, or CaCl2.
Which solution will show the smallest amount of freezing point depression?
Five solutions are made, each comprised of 1L of water and 1mol of C6H12O6, NaCl, H2SO4, Al(NO3)3, or CaCl2.
Which solution will show the smallest amount of freezing point depression?
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Freezing point depression is a colligative property, meaning that it depends on the amount of particles present in solution. The more ions that a solute dissociates into, the larger the magnitude of freezing point depression. Here, we're looking for the smallest amount of depression, so we want to find the solute that dissociates into the fewest particles. The answer is glucose, which is not ionic and does not dissociate at all in solution.
Freezing point depression is a colligative property, meaning that it depends on the amount of particles present in solution. The more ions that a solute dissociates into, the larger the magnitude of freezing point depression. Here, we're looking for the smallest amount of depression, so we want to find the solute that dissociates into the fewest particles. The answer is glucose, which is not ionic and does not dissociate at all in solution.
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Phase diagrams are used to depict changes in the properties of a solution at different temperatures and pressures. Below is a phase diagram of a polar solution.
If a polar molecule were added to the solution, how would the slope of segment AD change?
Phase diagrams are used to depict changes in the properties of a solution at different temperatures and pressures. Below is a phase diagram of a polar solution.
If a polar molecule were added to the solution, how would the slope of segment AD change?
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This question asks us to consider what would happen to the freezing point (also known as the melting point) of the solution if a polar molecule were added, for exampl adding NaCl to water. More directly, this question is a freezing point elevation/depression problem. After we determine what would happen to the freezing point of the solution, we can predict the change in the slope of the line.
The formula for freezing point depression is given below.
kf is the cryoscopic constant that says how easily a solution freezes with a given change in temperature, m is the molality of the solution, and i is the Vant Hoff factor. (The Vant Hoff factor is the number of ion particles per individual molecule that has been added; i.e. for NaCl this is 2 because it will separate into exactly two ionic particles when dissociated).
Given that kf and b will be constants for a given solution, we know that adding a molecule will decrease the freezing point because i has some positive value. Now that we know the freezing point is depressed (lowered), how will the slope of the line change?
At the same pressure, a lower temperature will be required for the solution with the added polar molecule to freeze, thus the slope will be less negative (segment AD will look more flat on the graph).
Why does the added molecule have to be polar to have an effect? First, notice that we are told that the phase diagram is of a polar solution. Next, let’s look at the i factor. i only has a value if the added molecules can be dissolved in the original solution. If, for example, we added a nonpolar molecule, it could not be dissolved by the solution and will not contribute to depressing the freezing point. “Like-dissolves-like” also applies here; the freezing point will only change if the solution and molecule added are both polar or both nonpolar.
This question asks us to consider what would happen to the freezing point (also known as the melting point) of the solution if a polar molecule were added, for exampl adding NaCl to water. More directly, this question is a freezing point elevation/depression problem. After we determine what would happen to the freezing point of the solution, we can predict the change in the slope of the line.
The formula for freezing point depression is given below.
kf is the cryoscopic constant that says how easily a solution freezes with a given change in temperature, m is the molality of the solution, and i is the Vant Hoff factor. (The Vant Hoff factor is the number of ion particles per individual molecule that has been added; i.e. for NaCl this is 2 because it will separate into exactly two ionic particles when dissociated).
Given that kf and b will be constants for a given solution, we know that adding a molecule will decrease the freezing point because i has some positive value. Now that we know the freezing point is depressed (lowered), how will the slope of the line change?
At the same pressure, a lower temperature will be required for the solution with the added polar molecule to freeze, thus the slope will be less negative (segment AD will look more flat on the graph).
Why does the added molecule have to be polar to have an effect? First, notice that we are told that the phase diagram is of a polar solution. Next, let’s look at the i factor. i only has a value if the added molecules can be dissolved in the original solution. If, for example, we added a nonpolar molecule, it could not be dissolved by the solution and will not contribute to depressing the freezing point. “Like-dissolves-like” also applies here; the freezing point will only change if the solution and molecule added are both polar or both nonpolar.
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What is the freezing point of a 
aqueous solution of 
?
What is the freezing point of a
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Freezing-point depression is a colligative property and is calculated with the formula:
The van't Hoff factor, 
, represents the number of particles a compound will dissociate into when dissolving in a solution. 
is the freezing-point depression constant, which is given in the question. 
is molality.
Using the equation, we can calculate the freezing point depression using the values from the question.
The standard freezing point of water is 
. With the freezing point depression, the solution will freeze at 
Freezing-point depression is a colligative property and is calculated with the formula:
The van't Hoff factor,
Using the equation, we can calculate the freezing point depression using the values from the question.
The standard freezing point of water is
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What is the freezing point of a 
aqueous solution of 
?
What is the freezing point of a
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Freezing-point depression is a colligative property and is calculated with the formula:
The van't Hoff factor, 
, represents the number of particles a compound will dissociate into when dissolving in a solution. 
is the freezing-point depression constant, which is given in the question. 
is molality.
Using the equation, we can calculate the freezing point depression using the values from the question.
The standard freezing point of water is 
. With the freezing point depression, the solution will freeze at 
.
Freezing-point depression is a colligative property and is calculated with the formula:
The van't Hoff factor,
Using the equation, we can calculate the freezing point depression using the values from the question.
The standard freezing point of water is
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The values for normal boiling and freezing points, along with 
and 
values are given below for select solvents.
What is the freezing point of a 
solution of glucose in benzene?
The values for normal boiling and freezing points, along with
What is the freezing point of a
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First, calculate the freezing point depression with the equation:
The van't Hoff factor for glucose is 1, since it does not dissociate in solution. The freezing point depression constant is given in the table.
Next, subtract this value from the freezing point of pure benzene to find the freezing point of the final solution.
First, calculate the freezing point depression with the equation:
The van't Hoff factor for glucose is 1, since it does not dissociate in solution. The freezing point depression constant is given in the table.
Next, subtract this value from the freezing point of pure benzene to find the freezing point of the final solution.
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The values for normal boiling and freezing points, along with 
and 
values are given below for select solvents.
Which of the following will result in the least freezing point depression when added to 
of water?
The values for normal boiling and freezing points, along with
Which of the following will result in the least freezing point depression when added to
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We are looking for the least amount of freezing point depression. Freezing point depression is calculated using the equation:
Each of these solutions has a different molality, which needs to be calculated. Molality is equal to moles of solute per kilogram solvent. To find this value, convert grams to moles (using molar mass) and divide by the mass of the solvent.
Next, find the van't Hoff factor for each compound.
Finally, use the initial equation to find the smallest freezing point depression (we are looking for the solution with the highest freezing point).
After calculating the change in freezing point for each solution, we find that the barium hydroxide solution has the smallest depression.
We are looking for the least amount of freezing point depression. Freezing point depression is calculated using the equation:
Each of these solutions has a different molality, which needs to be calculated. Molality is equal to moles of solute per kilogram solvent. To find this value, convert grams to moles (using molar mass) and divide by the mass of the solvent.
Next, find the van't Hoff factor for each compound.
Finally, use the initial equation to find the smallest freezing point depression (we are looking for the solution with the highest freezing point).
After calculating the change in freezing point for each solution, we find that the barium hydroxide solution has the smallest depression.
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