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Chapter 13: Problem 1

Which of the following do you expect to be most water soluble, and why? \(\mathrm{C}_{10} \mathrm{H}_{8}(\mathrm{s}), \mathrm{NH}_{2} \mathrm{OH}(\mathrm{s})\) \(\mathrm{C}_{6} \mathrm{H}_{6}(\mathrm{l}), \mathrm{CaCO}_{3}(\mathrm{s})\).

Short Answer

Expert verified
NH2OH is the most water soluble compound as it can form hydrogen bonds with water due to its polarity.

Step by step solution

01

Identification of Compound Type

First identify whether each compound is polar or non-polar. C10H8 and C6H6 are nonpolar hydrocarbons. NH2OH is a polar covalent compound due to the presence of hydrogen bonds. Lastly, CaCO3 is an ionic compound.
02

Determination of Solubility

Using the 'like dissolves like' concept, hydrocarbons(e.g C10H8 and C6H6) with nonpolar characteristics will not be easily dissolved in water. CaCO3, though ionic, is generally insoluble in water as the strong ionic bonds between the calcium and carbonate ions are too difficult for water molecules to break. The polar compound, NH2OH, would be expected to dissolve most readily in water as it can form hydrogen bonds with water.

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Most popular questions from this chapter

Calculate the vapor pressure at \(20^{\circ} \mathrm{C}\) of a saturated solution of the nonvolatile solute, urea, \(\mathrm{CO}\left(\mathrm{NH}_{2}\right)_{2},\) in methanol, \(\mathrm{CH}_{3} \mathrm{OH} .\) The solubility is \(17 \mathrm{g}\) urea/100 \(\mathrm{mL}\) methanol. The density of methanol is \(0.792 \mathrm{g} / \mathrm{mL}\), and its vapor pressure at \(20^{\circ} \mathrm{C}\) is \(95.7 \mathrm{mmHg}\).

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