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Chapter 11: Problem 114

For each of the following, choose the pair of substances you would expect to give the most ideal solution. Explain your choices. a. \(\mathrm{CH}_{3}\left(\mathrm{CH}_{2}\right)_{6} \mathrm{CH}_{3}\) and $\mathrm{CH}_{3}\left(\mathrm{CH}_{25} \mathrm{CH}_{3} \text { or } \mathrm{H}_{2} \mathrm{O} \text { and }\right.$ \(\mathrm{CH}_{3}-\mathrm{O}-\mathrm{CH}_{3}\) b. \(\mathrm{CH}_{3} \mathrm{OH}\) and $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}\( or \)\mathrm{CH}_{3} \mathrm{F}\( and \)\mathrm{HF}$

Short Answer

Expert verified
The most ideal solutions would be formed between: a) CH3(CH2)6CH3 and CH3(CH2)25CH3, as they have similar London dispersion forces due to their similar nonpolar structures. b) CH3OH and CH3CH2OH, as they have similar intermolecular forces, including hydrogen bonding, due to their similar molecular structures.

Step by step solution

01

a) Analyze the molecules

For the first pair, we have a saturated hydrocarbon (C10H22) and a larger saturated hydrocarbon (C26H54). For the second pair, we have water (H2O) and dimethyl ether (CH3-O-CH3).
02

a) Compare intermolecular forces

The two saturated hydrocarbons only have London dispersion forces between their molecules since they are nonpolar. As the London dispersion forces increase with the size of the molecules, the two substances will have similar intermolecular forces, making them more likely to form an ideal solution. In the second pair, water molecules form strong hydrogen bonds, while dimethyl ether molecules only have dipole-dipole interactions and induce-dipole forces. These two substances have significantly different intermolecular forces, making them less likely to form an ideal solution.
03

a) Choose the most ideal solution

Based on the similarities in the intermolecular forces, the pair of substances that would likely form the most ideal solution would be CH3(CH2)6CH3 and CH3(CH2)25CH3.
04

b) Analyze the molecules

For the first pair, we have methanol (CH3OH) and ethanol (CH3CH2OH). For the second pair, we have methyl fluoride (CH3F) and hydrogen fluoride (HF).
05

b) Compare intermolecular forces

Methanol and ethanol have similar molecular structures, and both are capable of forming hydrogen bonds; ethanol has an additional carbon and two hydrogens. Thus, both substances in the first pair have similar intermolecular forces, making them more likely to form an ideal solution. In the second pair, methyl fluoride has only dipole-dipole forces, while hydrogen fluoride forms strong hydrogen bonds. These two substances have significantly different intermolecular forces, making them less likely to form an ideal solution.
06

b) Choose the most ideal solution

Based on the similarities in the intermolecular forces, the pair of substances that would likely form the most ideal solution would be CH3OH and CH3CH2OH.

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Most popular questions from this chapter

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