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Chapter 13: Problem 2

Which of the following is moderately soluble both in water and in benzene \(\left[\mathrm{C}_{6} \mathrm{H}_{6}(1)\right]\), and why? (a) 1 -butanol, \(\mathrm{CH}_{3}\left(\mathrm{CH}_{2}\right)_{2} \mathrm{CH}_{2} \mathrm{OH} ;\) (b) naphthalene, \(\mathrm{C}_{10} \mathrm{H}_{8} ;\) (c) hexane, \(\mathrm{C}_{6} \mathrm{H}_{14} ;\) (d) \(\mathrm{NaCl}(\mathrm{s})\)

Short Answer

Expert verified
1-butanol is moderately soluble in both water and benzene due to the presence of both polar (hydroxyl group) and nonpolar (alkyl chain) characteristics.

Step by step solution

01

Understand the molecular structure

Evaluate each option and determine whether the substance is polar or nonpolar. Polar substances will have a significant difference in electronegativity between the atoms, while nonpolar substances will not. This step is important to determine which substances can dissolve in both solvents.
02

Evaluate Option (a)

1 -butanol, \(\mathrm{CH}_{3}\left(\mathrm{CH}_{2}\right)_{2}\mathrm{CH}_{2} \mathrm{OH}\), is a polar molecule due to the presence of the -OH (hydroxyl) group, which contains a polar O-H bond. Therefore, it is soluble in water. But, the longer alkyl chain also makes it somewhat soluble in nonpolar solvents like benzene.
03

Evaluate Option (b)

Naphthalene, \(\mathrm{C}_{10}\mathrm{H}_{8}\), is a nonpolar molecule due to symmetrical arrangement of electron charge distribution in it. So, it's not soluble in water but soluble in benzene.
04

Evaluate Option (c)

Hexane, \(\mathrm{C}_{6} \mathrm{H}_{14}\), is a nonpolar substance because of the symmetrical arrangement of its atoms. Therefore, hexane does not dissolve in water, but it is soluble in benzene.
05

Evaluate Option (d)

Sodium Chloride, \(\mathrm{NaCl}(\mathrm{s})\), is an ionic compound and it's quite polar. As a result, it is soluble in polar solvent like water but not in a nonpolar solvent like benzene.

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Most popular questions from this chapter

Which of the following ions has the greater charge density? (a) \(\mathrm{Na}^{+} ;\) (b) \(\mathrm{F}^{-} ;\) (c) \(\mathrm{K}^{+} ;\) (d) \(\mathrm{Cl}^{-}\).

An aqueous solution has \(109.2 \mathrm{g} \mathrm{KOH} / \mathrm{L}\) solution. The solution density is \(1.09 \mathrm{g} / \mathrm{mL} .\) Your task is to use \(100.0 \mathrm{mL}\) of this solution to prepare \(0.250 \mathrm{m}\) KOH. What mass of which component, \(\mathrm{KOH}\) or \(\mathrm{H}_{2} \mathrm{O}\), would you add to the \(100.0 \mathrm{mL}\) of solution?

A \(10.00 \%\) -by-mass solution of ethanol, \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}\) in water has a density of \(0.9831 \mathrm{g} / \mathrm{mL}\) at \(15^{\circ} \mathrm{C}\) and \(0.9804 \mathrm{g} / \mathrm{mL}\) at \(25^{\circ} \mathrm{C} .\) Calculate the molality of the ethanol-water solution at these two temperatures. Does the molality differ at the two temperatures (that is, at 15 and \(25^{\circ} \mathrm{C}\) )? Would you expect the molarities to differ? Explain.

The Environmental Protection Agency has a limit of 15 ppm for the amount of lead in drinking water. If a \(1.000 \mathrm{mL}\) sample of water at \(20^{\circ} \mathrm{C}\) contains \(15 \mathrm{ppm}\) of lead, how many lead ions are there in this sample of water? What is the mole fraction of lead ion in solution?

\(\mathrm{NH}_{3}(\mathrm{aq})\) conducts electric current only weakly. The same is true for acetic acid, \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(\mathrm{aq}) .\) When these solutions are mixed, however, the resulting solution conducts electric current very well. Propose an explanation.
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