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Chapter 13: Problem 34

Which of the following in each pair is likely to be more soluble in water: (a) cyclohexane \(\left(\mathrm{C}_{6} \mathrm{H}_{12}\right)\) or glucose \(\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\right)\), (b) propionic acid \(\left(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{COOH}\right)\) or sodium propionate $\left(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{COONa}\right),(\mathbf{c}) \mathrm{HCl}$ or ethyl chloride \(\left(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{Cl}\right) ?\) Explain in each case.

Short Answer

Expert verified
(a) Glucose, (b) Sodium propionate, (c) HCl

Step by step solution

01

Determine the polarity of each compound

First, let's assess the polarity of each compound in the pairs. Polar molecules have regions of partial positive and negative charge due to the uneven distribution of electron density in the molecule, while nonpolar molecules have an even distribution of electron density. (a) cyclohexane (C6H12) - nonpolar; glucose (C6H12O6) - polar (has hydroxyl groups) (b) propionic acid (CH3CH2COOH) - polar (has carboxylic acid group); sodium propionate (CH3CH2COONa) - ionic (has an ionic bond between sodium and carboxylate group) (c) HCl - polar (due to the difference in electronegativity between hydrogen and chlorine); ethyl chloride (CH3CH2Cl) - polar but less polar than HCl (large alkyl group with chlorine)
02

Analyze the interactions between each compound and water molecules

Now, let's analyze the possible interactions between each compound and water, a polar solvent: (a) cyclohexane - weak van der Waals forces with water; glucose - hydrogen bonding with water (b) propionic acid - hydrogen bonding with water; sodium propionate - ion-dipole interactions with water (c) HCl - strong ion-dipole interactions with water due to dissociation into ions; ethyl chloride - weaker dipole-dipole interactions with water
03

Determine which compound is more soluble in water for each pair

Based on polarity and interactions with water, we can determine which compound is more soluble in water: (a) Glucose is more soluble in water than cyclohexane, because it is polar and can form hydrogen bonds with water molecules. (b) Sodium propionate is more soluble in water than propionic acid, because it is ionic and can form strong ion-dipole interactions with water molecules. (c) HCl is more soluble in water than ethyl chloride, because it can form strong ion-dipole interactions with water molecules when completely dissociated, while ethyl chloride can only form weaker dipole-dipole interactions.

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Most popular questions from this chapter

Two nonpolar organic liquids, benzene $\left(\mathrm{C}_{6} \mathrm{H}_{6}\right)\( and toluene \)\left(\mathrm{C}_{7} \mathrm{H}_{8}\right),\( are mixed. (a) Do you expect \)\Delta H_{\text {soln }}$ to be a large positive number, a large negative number, or close to zero? Explain. (b) Benzene and toluene are miscible with each other in all proportions. In making a solution of them, is the entropy of the system increased, decreased, or close to zero, compared to the separate pure liquids?

Aerosols are important components of the atmosphere. Does the presence of aerosols in the atmosphere increase or decrease the amount of sunlight that arrives at the Earth's surface, compared to an "aerosol-free" atmosphere? Explain your reasoning.

What is the osmotic pressure formed by dissolving \(50.0 \mathrm{mg}\) of acetylsalicylic acid $\left(\mathrm{C}_{9} \mathrm{H}_{8} \mathrm{O}_{4}\right)\( in \)0.100 \mathrm{~L}\( of water at \)37^{\circ} \mathrm{C} ?$

Calculate the molality of each of the following solutions: (a) \(10.0 \mathrm{~g}\) of benzene \(\left(\mathrm{C}_{6} \mathrm{H}_{6}\right)\) dissolved in \(50.0 \mathrm{~g}\) of carbon tetrachloride \(\left(\mathrm{CCl}_{4}\right),(\mathbf{b}) 5.00 \mathrm{~g}\) of \(\mathrm{NaCl}\) dissolved in \(0.100 \mathrm{~L}\) of water.

Choose the best answer: A colloidal dispersion of one liquid in another is called \((\mathbf{a})\) a gel, \((\mathbf{b})\) an emulsion, \((\mathbf{c})\) a foam (d) an aerosol.
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