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Chapter 13: Problem 9

Arrange these compounds in order of increasing solubility in water: \(\mathrm{O}_{2}, \mathrm{LiCl}, \mathrm{Br}_{2}, \mathrm{CH}_{3} \mathrm{OH}\) (methanol).

Short Answer

Expert verified
The compounds arranged in order of increasing solubility in water are: \(\mathrm{O}_{2} , \mathrm{Br}_{2} , \mathrm{CH}_{3} \mathrm{OH}, \mathrm{LiCl}\)

Step by step solution

01

Identify the polar and ionic compounds

Polar and ionic compounds are highly soluble in water. In our list, \(\mathrm{LiCl}\) is ionic and \(\mathrm{CH}_{3} \mathrm{OH}\) (methanol) is polar.
02

Identify the nonpolar compounds

Nonpolar compounds are less soluble in water. In our list, \(\mathrm{O}_{2}\) and \(\mathrm{Br}_{2}\) are nonpolar and hence less soluble.
03

Arrange the compounds in increasing order of solubility

As per the solubility rule, nonpolar compounds will be less soluble compared to polar and ionic compounds. Therefore, the least soluble compound is \(\mathrm{O}_{2}\), followed by \(\mathrm{Br}_{2}\). Methanol (\(\mathrm{CH}_{3} \mathrm{OH}\)) will be more soluble due to its polar nature and capability to form hydrogen bonds with water. The most soluble will be the ionic compound \(\mathrm{LiCl}\) which can dissociate completely in water.

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Most popular questions from this chapter

Liquids A (molar mass \(100 \mathrm{~g} / \mathrm{mol}\) ) and \(\mathrm{B}\) (molar mass \(110 \mathrm{~g} / \mathrm{mol}\) ) form an ideal solution. At \(55^{\circ} \mathrm{C}\), A has a vapor pressure of \(95 \mathrm{mmHg}\) and \(\mathrm{B}\) has a vapor pressure of \(42 \mathrm{mmHg}\). A solution is prepared by mixing equal masses of \(\mathrm{A}\) and \(\mathrm{B}\). (a) Calculate the mole fraction of each component in the solution. (b) Calculate the partial pressures of \(\mathrm{A}\) and \(\mathrm{B}\) over the solution at \(55^{\circ} \mathrm{C}\). (c) Suppose that some of the vapor described in (b) is condensed to a liquid. Calculate the mole fraction of each component in this liquid and the vapor pressure of each component above this liquid at \(55^{\circ} \mathrm{C}\).

How is the lowering in vapor pressure related to a rise in the boiling point of a solution?

What is the effect of pressure on the solubility of a liquid in liquid and of a solid in liquid?

Two liquids \(A\) and \(B\) have vapor pressures of 76 \(\mathrm{mmHg}\) and \(132 \mathrm{mmHg}\), respectively, at \(25^{\circ} \mathrm{C}\). What is the total vapor pressure of the ideal solution made up of (a) 1.00 mole of \(A\) and 1.00 mole of \(B\) and (b) 2.00 moles of \(\mathrm{A}\) and 5.00 moles of \(\mathrm{B} ?\)

Calculate the molarity and the molality of \(\mathrm{NH}_{3}\) for a solution of \(30.0 \mathrm{~g}\) of \(\mathrm{NH}_{3}\) in \(70.0 \mathrm{~g}\) of water. The density of the solution is \(0.982 \mathrm{~g} / \mathrm{mL}\).
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