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Chapter 13: Problem 58

How does increasing the concentration of a nonvolatile solute in water affect the following properties: (a) vapor pressure, (b) freezing point, (c) boiling point; (d) osmotic pressure?

Short Answer

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Increasing the concentration of a nonvolatile solute in water affects the properties as follows: (a) Vapor pressure decreases because fewer water molecules can escape into the vapor phase; (b) Freezing point decreases due to solute particles disrupting ice formation; (c) Boiling point increases because more energy is required for water molecules to escape; (d) Osmotic pressure increases as solvent molecules flow toward higher solute concentration to achieve equilibrium.

Step by step solution

01

(a) Vapor Pressure

A nonvolatile solute does not have a considerable vapor pressure at any given temperature. When it is dissolved in water, the solute particles take up some of the water's surface area, which is initially occupied by water molecules. As a result, the number of water molecules that can escape into the vapor phase decreases, lowering the overall vapor pressure of the solution compared to that of pure water. As the concentration of the nonvolatile solute increases, the vapor pressure decreases even further.
02

(b) Freezing Point

Adding a nonvolatile solute to water lowers the freezing point of the solution, a phenomenon known as freezing point depression. The solute particles disrupt the formation of the ordered structure of ice, making it harder for water to freeze. Consequently, a greater amount of energy has to be removed from the solution for freezing to occur. As the concentration of the solute increases, the freezing point of the solution decreases further.
03

(c) Boiling Point

The boiling point of a solution containing a nonvolatile solute in water is higher than that of pure water, which is called boiling point elevation. This is because the solute particles interfere with the escape of water molecules into the vapor phase, requiring more energy (in the form of increased temperature) for the same amount of water molecules to escape. As the concentration of the solute increases, the boiling point of the solution increases.
04

(d) Osmotic Pressure

Osmotic pressure is the pressure required to prevent the flow of solvent molecules across a semipermeable membrane (which allows the solvent but not the solute to pass through) from an area of lower solute concentration to an area of higher solute concentration. When the concentration of a nonvolatile solute in water increases, the osmotic pressure also increases. This is because the solvent molecules are more likely to flow towards the area of higher solute concentration to achieve equilibrium.

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Most popular questions from this chapter

At \(35^{\circ} \mathrm{C}\) the vapor pressure of acetone, \(\left(\mathrm{CH}_{3}\right)_{2} \mathrm{CO}\), is 360 torr, and that of chloroform, \(\mathrm{CHCl}_{3}\), is 300 torr. Acetone and chloroform can form weak hydrogen bonds between one another as follows: A solution composed of an equal number of moles of acetone and chloroform has a vapor pressure of 250 torr at \(35^{\circ} \mathrm{C}\). (a) What would be the vapor pressure of the solution if it exhibited ideal behavior? (b) Use the existence of hydrogen bonds between acetone and chloroform molecules to explain the deviation from ideal behavior. (c) Based on the behavior of the solution, predict whether the mixing of acetone and chloroform is an exothermic \(\left(\Delta H_{\mathrm{soln}}<0\right)\) or endothermic \(\left(\Delta H_{\text {soln }}>0\right)\) process.

A "canned heat" product used to warm chafing dishes consists of a homogeneous mixture of ethanol \(\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\right)\) and paraffin that has an average formula of \(\mathrm{C}_{24} \mathrm{H}_{5}\). What mass of \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\) should be added to \(620 \mathrm{~kg}\) of the paraffin in formulating the mixture if the vapor pressure of ethanol at \(35^{\circ} \mathrm{C}\) over the mixture is to be 8 torr? The vapor pressure of pure ethanol at \(35^{\circ} \mathrm{C}\) is 100 torr.

Calculate the number of moles of solute present in each of the following aqueous solutions: (a) \(600 \mathrm{~mL}\) of \(0.250 \mathrm{M} \mathrm{SrBr}_{2}\), (b) \(86.4 \mathrm{~g}\) of \(0.180 \mathrm{~m} \mathrm{KCl}\), (c) \(124.0 \mathrm{~g}\) of a solution that is \(6.45 \%\) glucose \(\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\right)\) by mass.

Commercial concentrated aqueous ammonia is \(28 \% \mathrm{NH}_{3}\) by mass and has a density of \(0.90 \mathrm{~g} / \mathrm{mL}\). What is the molarity of this solution?

At \(20{ }^{\circ} \mathrm{C}\) the vapor pressure of benzene \(\left(\mathrm{C}_{6} \mathrm{H}_{6}\right)\) is 75 torr, and that of toluene \(\left(\mathrm{C}_{7} \mathrm{H}_{8}\right)\) is 22 torr. Assume that benzene and toluene form an ideal solution. (a) What is the composition in mole fractions of a solution that has a vapor pressure of 35 torr at \(20^{\circ} \mathrm{C} ?\) (b) What is the mole fraction of benzene in the vapor above the solution described in part (a)?
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