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Ch.13 - Solutions & Their Properties
All textbooksMcMurry 8th EditionCh.13 - Solutions & Their PropertiesProblem 46
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Chapter 13, Problem 46

Is the solubility of acetic acid, CH3COOH, greater in water or benzene, C6H6?

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Step 1: Identify the nature of acetic acid (CH3COOH). Acetic acid is a polar molecule due to the presence of the carboxyl group (-COOH), which can form hydrogen bonds with other polar molecules.
Step 2: Analyze the solvent water (H2O). Water is a highly polar solvent and is capable of forming hydrogen bonds due to its polar O-H bonds.
Step 3: Consider the solvent benzene (C6H6). Benzene is a nonpolar solvent, characterized by its symmetrical ring structure and lack of polar bonds.
Step 4: Apply the principle 'like dissolves like'. Polar solutes tend to dissolve well in polar solvents, while nonpolar solutes dissolve better in nonpolar solvents.
Step 5: Conclude based on the polarity. Since acetic acid is polar and water is polar, acetic acid is more soluble in water than in benzene, which is nonpolar.
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