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Chapter 12: Problem 44

Use a phase diagram to show the difference in freezing points and boiling points between an aqueous urea solution and pure water.

Short Answer

Expert verified
The phase diagram of an aqueaous urea solution will have a lower freezing point and a higher boiling point compared to the phase diagram of pure water due to the colligative properties of the solution, specifically freezing point depression and boiling point elevation.

Step by step solution

01

Understanding Phase Diagrams

A phase diagram provides graphical details about the stability of phases of a substance at different temperatures and pressures. The transition between phases (such as freezing or boiling) occur at specific temperatures and pressures, which can be observed on this diagram.
02

Phase Diagram of Pure Water

Plot the phase diagram for pure water. The x-axis represents temperature and y-axis pressure. You'll note three curves that represent phase transitions: solid-liquid, liquid-gas, and solid-gas. The point at which all these curves meet is known as the triple point. For water, the freezing point at 1 atmosphere of pressure is 0 degrees Celsius, and the boiling point is 100 degrees Celsius.
03

Phase Diagram of Aqueous Urea Solution

Now plot the phase diagram for an aqueous urea solution. Solutions have different phase behavior compared to pure substances. Due to the presence of urea, the freezing point will be lower than that of pure water (freezing point depression), while the boiling point is higher (boiling point elevation). These effects are due to the colligative properties of solutions.
04

Compare the Phase Diagrams

By comparing the two diagrams, it's clear that the phase transitions occur at different temperatures for pure water and the aqueaous urea solution due the properties of the urea solution. The key takeaway is that the solute (urea) effectively lowers the freezing point and raises the boiling point.

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Most popular questions from this chapter

Basing your answer on intermolecular force considerations, explain what "like dissolves like" means.

Describe how you would use freezing-point depression and osmotic pressure measurements to determine the molar mass of a compound. Why are boiling-point elevation and vapor-pressure lowering normally not used for this purpose?

A \(50-g\) sample of impure \(\mathrm{KClO}_{3}\) (solubility \(=7.1 \mathrm{~g}\) per \(100 \mathrm{~g} \mathrm{H}_{2} \mathrm{O}\) at \(20^{\circ} \mathrm{C}\) ) is contaminated with 10 percent of KCl (solubility \(=25.5 \mathrm{~g}\) per \(100 \mathrm{~g}\) of \(\mathrm{H}_{2} \mathrm{O}\) at \(20^{\circ} \mathrm{C}\) ). Calculate the minimum quantity of \(20^{\circ} \mathrm{C}\) water needed to dissolve all the \(\mathrm{KCl}\) from the sample. How much \(\mathrm{KClO}_{3}\) will be left after this treatment? (Assume that the solubilities are unaffected by the presence of the other compound.)

The vapor pressure of ethanol \(\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\right)\) at \(20^{\circ} \mathrm{C}\) is \(44 \mathrm{mmHg},\) and the vapor pressure of methanol \(\left(\mathrm{CH}_{3} \mathrm{OH}\right)\) at the same temperature is \(94 \mathrm{mmHg} . \mathrm{A}\) mixture of \(30.0 \mathrm{~g}\) of methanol and \(45.0 \mathrm{~g}\) of ethanol is prepared (and can be assumed to behave as an ideal solution). (a) Calculate the vapor pressure of methanol and ethanol above this solution at \(20^{\circ} \mathrm{C}\). (b) Calculate the mole fraction of methanol and ethanol in the vapor above this solution at \(20^{\circ} \mathrm{C}\). (c) Suggest a method for separating the two components of the solution.

A student is observing two beakers of water. One beaker is heated to \(30^{\circ} \mathrm{C}\), and the other is heated to \(100^{\circ} \mathrm{C}\). In each case, bubbles form in the water. Are these bubbles of the same origin? Explain.
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