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Chapter 13: Problem 30

Would you expect alanine (an amino acid) to be more soluble in water or in hexane? Explain.

Short Answer

Expert verified
Alanine is expected to be more soluble in water due to its polar nature, which is caused by the presence of polar amino (-NH2) and carboxyl (-COOH) groups in its structure. The polar nature of alanine makes it more compatible with the polar solvent water, adhering to the "like dissolves like" rule. Hexane, a nonpolar solvent, is less likely to dissolve alanine effectively.

Step by step solution

01

Analyze the structure of alanine

First, let us analyze the structure of alanine. Alanine is an 伪-amino acid with the chemical formula CH3CH(NH2)COOH. It has an amino group (-NH2) and a carboxyl group (-COOH) on the same carbon atom. Due to the presence of these polar groups, alanine exhibits some polar characteristics.
02

Analyze the structure of the solvents (water and hexane)

Now we have to analyze the structure of the solvents water and hexane: 1. Water (H2O) is a polar molecule due to the electronegativity difference between oxygen and hydrogen atoms. The presence of polar OH bonds gives water a high polarity and its well-known ability to dissolve various substances. 2. Hexane (C6H14) is a nonpolar molecule with single bonds between carbon and hydrogen atoms. No significant electronegativity difference exists between these atoms, resulting in a nonpolar molecule. Nonpolar molecules typically dissolve nonpolar substances.
03

Comparing the solubility of alanine in water and hexane

Now that we have analyzed the structures of alanine, water, and hexane, we can compare alanine's solubility in these solvents. - Alanine contains both polar groups (-NH2, -COOH), which makes it partially polar. - Water is a polar solvent, and hexane is a nonpolar solvent. Recalling the rule "like dissolves like", we would expect alanine to be more soluble in a polar solvent, like water, than in a nonpolar solvent, like hexane. Therefore, we can conclude that alanine should be more soluble in water than in hexane.

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Most popular questions from this chapter

Carbon disulfide \(\left(\mathrm{CS}_{2}\right)\) boils at \(46.30^{\circ} \mathrm{C}\) and has a density of \(1.261 \mathrm{~g} / \mathrm{mL}\). (a) When \(0.250 \mathrm{~mol}\) of a nondissociating solute is dissolved in \(400.0 \mathrm{~mL}\) of \(\mathrm{CS}_{2}\), the solution boils at \(47.46^{\circ} \mathrm{C}\). What is the molal boiling-point-elevation constant for \(\mathrm{CS}_{2}\) ? (b) When \(5.39 \mathrm{~g}\) of a nondissociating unknown is dissolved in \(50.0 \mathrm{~mL}\) of \(\mathrm{CS}_{2}\), the solution boils at \(47.08^{\circ} \mathrm{C}\). What is the molecular weight of the unknown?

A saturated solution of sucrose \(\left(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\right)\) is made by dissolving excess table sugar in a flask of water. There are \(50 \mathrm{~g}\) of undissolved sucrose crystals at the bottom of the flask in contact with the saturated solution. The flask is stoppered and set aside. A year later a single large crystal of mass \(50 \mathrm{~g}\) is at the bottom of the flask. Explain how this experiment provides evidence for a dynamic equilibrium between the saturated solution and the undissolved solute.

Calculate the number of moles of solute present in each of the following solutions: (a) \(255 \mathrm{~mL}\) of \(1.50 \mathrm{MHNO}_{3}(a q)\), (b) \(50.0 \mathrm{mg}\) of an aqueous solution that is \(1.50 \mathrm{~m} \mathrm{NaCl}\), (c) \(75.0 \mathrm{~g}\) of an aqueous solution that is \(1.50 \%\) sucrose \(\left(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\right)\) by mass.

Calculate the molality of each of the following solutions: (a) \(8.66 \mathrm{~g}\) of benzene \(\left(\mathrm{C}_{6} \mathrm{H}_{6}\right)\) dissolved in \(23.6 \mathrm{~g}\) of carbon tetrachloride \(\left(\mathrm{CCl}_{4}\right)\), (b) \(4.80 \mathrm{~g}\) of \(\mathrm{NaCl}\) dissolved in \(0.350 \mathrm{~L}\) of water.

When ammonium chloride dissolves in water, the solution becomes colder. (a) Is the solution process exothermic or endothermic? (b) Why does the solution form?
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