Multiple Choice
Which statement best describes what happens when NaCl dissolves in water?
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6. Chemical Quantities & Aqueous Reactions
Solubility Rules
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Based only on intermolecular forces, which of the following compounds would be most soluble in CH3OH?
A
CH3NH2
B
CCl4
C
NaCl
D
CH3CH2CH3
Verified step by step guidance1
Identify the nature of the solvent, CH3OH (methanol), which is a polar molecule capable of hydrogen bonding due to its -OH group.
Analyze the intermolecular forces present in each solute:
- CH3NH2 (methylamine) can hydrogen bond because it has an -NH2 group.
- CCl4 is nonpolar and only exhibits London dispersion forces.
- NaCl is an ionic compound, which typically dissolves well in polar solvents but requires ion-dipole interactions.
- CH3CH2CH3 (propane) is nonpolar with only London dispersion forces.
Recall the principle 'like dissolves like,' meaning polar solvents dissolve polar solutes or those capable of hydrogen bonding better than nonpolar solutes.
Compare the solutes to methanol: CH3NH2 can form hydrogen bonds with CH3OH, making it highly soluble; CCl4 and CH3CH2CH3 are nonpolar and less soluble; NaCl is ionic and may not dissolve well in methanol due to limited ion-dipole interactions compared to water.
Conclude that based on intermolecular forces, CH3NH2 is the most soluble in CH3OH because it can engage in hydrogen bonding with the solvent.
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