Find the Boiling Points of the Following Solutions

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The values for normal boiling and freezing points, along with $\small k_b$ and $\small k_f$ values are given below for select solvents.

$\begin{matrix} \text{Solvent} & \text{Boiling Point}\ (^oC) & k_b\ (\frac{^oC}{m}) & \text{Freezing Point}\ (^oC) & k_f\ \frac{^oC}{m}\\ \text{Benzene} & 80.1 & 2.53 &5.5 &4.90 \\ \text{Water}& 100.0 & 0.52 & 0.0 & 1.86\\ \text{Acetic Acid} & 117.9 & 3.07 & 16.6 & 3.90 \end{matrix}$

A $\small 0.05m$ solution of which of the following compositions would result in the greatest boiling point elevation?

Possible Answers:

Sodium chloride in acetic acid

Sodium chloride in benzene

Magnesium phosphide in benzene

Magnesium phosphide in acetic acid

Correct answer:

Magnesium phosphide in acetic acid

Explanation:

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.

$\Delta T_{b} = k_{b}im$

First, calculate the van't Hoff for each compound.

$Mg_3P_2\rightarrow i=5$

$NaCl\rightarrow i=2$

Ultimately, we are looking for the greatest product of the boiling point elevation constant and van't Hoff factor (since molality is constant).

$\text{Benzene}\rightarrow k_b=2.53\frac{^oC}{m}$

$\text{Acetic Acid}\rightarrow k_b=3.07\frac{^oC}{m}$

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.

$\Delta T_b=(3.07\frac{^oC}{m})(5)(0.05m)=0.77^oC$

The values for normal boiling and freezing points, along with $\small k_b$ and $\small k_f$ values are given below for select solvents.

$\small 25g$ of ammonium phosphate are dissolved in $\small 500mL$ of water. What is the boiling point of this solution at $\small 1atm$ ?

Correct answer:

100.7^oC

Explanation:

We first need to find the boiling point elevation with the equation:

$\Delta T_{b}=k_{b}im$

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.
$25 g\ (NH_{4})_{3}PO_{4} * \frac{1 mol}{149g} = 0.17 mol\ (NH_4)_3PO_4$

$500mL\ H_2O*\frac{1g}{1mL}=500g=0.5kg\ H_2O$

$m=\frac{mol\ (NH_4)_3PO_4}{kg\ H_2O}=\frac{0.17mol}{0.5kg}=0.336m$

Next, use the molality, van't Hoff factor, and boiling point elevation constant to solve for the increase in boiling point.

$\Delta T_{b}=k_{b}im$

$\Delta T_b=(0.52\frac{kg^oC}{mol})(4)(0.336m)$

$\Delta T_b=0.70^oC$

Add this increase to the boiling point of pure water to find the boiling point of the solution.

100^oC+0.70^oC=100.7^oC

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.

$\LARGE P = X_{solv} * P_{solv}$

In this law, $\small X_{solv}$ is the mole fraction of the solvent, $\small P_{solv}$ 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?

Possible Answers:

They will likely have to cook their food a shorter time than at sea level, since it takes less heat to make vapor pressure match atmospheric pressure

They will likely have to cook their food a shorter time than at sea level, since it takes more heat to make vapor pressure match atmospheric pressure

They will likely have to cook their food longer than at sea level, since it takes less heat to make vapor pressure match atmospheric pressure

If they add salt to the water, it will help speed the rate at which the water boils

They will likely have to cook their food longer than at sea level, since it takes more heat to make vapor pressure match atmospheric pressure

Correct answer:

They will likely have to cook their food longer than at sea level, since it takes less heat to make vapor pressure match atmospheric pressure

Explanation:

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.

$\LARGE P = X_{solv} * P_{solv}$

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

Possible Answers:

I and II, only

III, only

I and III, only

I, II, and III

II and III, only

Correct answer:

I and III, only

Explanation:

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.

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?

Possible Answers:

2m CaF₂

3m C₆H₁₂O₆

1m MgCl₂

1m NaCl

Explanation:

Based on the equation $\Delta T_{b} = k_{b}mi$ , 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.

The equation for boiling point elevation is written as $\Delta T = k_{b}mi$ .

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?

Possible Answers:

The actual boiling point elevation will be lower than the theoretical boiling point elevation.

The vapor pressure of the solution will be lower than predicted.

The molality of the solution will decrease.

The solute will not raise the boiling point of the solution.

Correct answer:

The actual boiling point elevation will be lower than the theoretical boiling point elevation.

Explanation:

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, $\Delta T = k_{b}mi$ . The number of particles in the solution does not affect the molality.

Which of the following aqueous solutions will have the highest boiling point?

Possible Answers:

1m MgCl₂

1m NaF

2m MgCl₂

2m NaCl

Explanation:

In order to answer this problem, consider the equation for boiling point elevation: $\Delta T = k_{b}mi$ .

$k_{b}$ 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. MgCl₂will 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.

Which solution will have a higher boiling point?

Solution 1: 100mol NaCl in water

Solution 2: 100mol Glucose in water

Possible Answers:

Solution 1

Solution 1 and 2 will have the same boiling point

The answer cannot be determined from the information given

Solution 2

Correct answer:

Solution 1

Which of the following compounds will create the greatest increase in boiling point when added to an aqueous solution?

Correct answer:

$2 mol\ Ca(OH)_2$

Explanation:

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. $2mol*\frac{2ions}{1mol}=4\ \text{moles of ions}$

Magnesium chloride and barium chloride will produce three ions per mole. $1mol*\frac{3ions}{1mol}=3\ \text{moles of ions}$

Calcium hydroxide will also produce three ions per mole, but we are given two moles instead of one. $2mol*\frac{3ions}{1mol}=6\ \text{moles of ions}$

Calcium hydroxide will produce the greatest number of ions, thus creating the greatest increase in boiling point elevation.

Each of the following solutions is added to equal amounts of water. Which solution will result in the greatest amount of boiling point elevation?

Correct answer:

$3.0mol\ \text{of}\ \text{NaCl}$

Explanation:

Boiling point elevation is a colligative property, meaning that it depends on the relative number of solute particles in solution. The answer choice with the largest number of moles ofparticles will show the greatest boiling point elevation. The equation for boiling point elevation is:

$\Delta T_b=k_bmi$

Molality is equal to moles of solute per kilogram of solvent, meaning that it will be proportional to the moles of solute added. Each solute is added to equal amounts of water, allowing us to keep this value constant. Similarly, $\small k_b$ will be constant for all of the solutions. Overall, boiling point elevation will be proportional to the moles of solute multiplied by the van't Hoff factor.

$\Detla T_b\propto ni$

Using this proportion, we can find the solute that will most impact the boiling point of water.

$MgCl_2:\ ni=(1.5)(3)=4.5$

$K_3PO_4:\ ni=(1.25)(4)=5$

$CaCl_2;\ ni=(1.5)(3)=4.5$

$HClO_4:\ ni=(2.5)(2)=5$

$NaCl:\ ni=(3.0)(2)=6$

Since sodium chloride results in the greatest moles of ions in solution, it will yield the greatest boiling point elevation.

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Find the Boiling Points of the Following Solutions

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Find the Boiling Points of the Following Solutions

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