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Ch.13 - Properties of Solutions
Chapter 13, Problem 7

The structures of vitamins E and B6 are shown below. Predict which is more water soluble and which is more fat soluble. [Section 13.3]

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Identify the structural features of each vitamin that influence solubility.
Vitamin E has a long hydrocarbon tail, which is nonpolar and hydrophobic, making it more fat soluble.
Vitamin B6 contains several polar groups, such as hydroxyl (OH) groups, which can form hydrogen bonds with water, making it more water soluble.
Consider the overall polarity of each vitamin: Vitamin E is less polar due to its hydrocarbon tail, while Vitamin B6 is more polar due to its functional groups.
Conclude that Vitamin E is more fat soluble and Vitamin B6 is more water soluble based on their structural features.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Solubility Principles

Solubility refers to the ability of a substance to dissolve in a solvent. Water solubility is influenced by the presence of polar functional groups, which interact favorably with water molecules, while fat solubility is associated with nonpolar characteristics that dissolve in lipids. Understanding these principles helps predict how vitamins behave in biological systems.
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Chemical Structure of Vitamins

The chemical structure of vitamins, including the presence of functional groups such as hydroxyl (-OH) or carboxyl (-COOH), plays a crucial role in determining their solubility. For instance, vitamins with more hydrophilic groups tend to be more water-soluble, while those with long hydrocarbon chains are typically more fat-soluble. Analyzing the structures of vitamins E and B6 is essential for making solubility predictions.
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Hydrophilic vs. Hydrophobic

Hydrophilic substances are attracted to water and tend to dissolve in it, while hydrophobic substances repel water and are more soluble in fats. This distinction is vital when predicting the solubility of vitamins, as it directly relates to their functional roles in the body. Recognizing which vitamin has hydrophilic or hydrophobic characteristics aids in understanding their absorption and transport mechanisms.
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Related Practice
Open Question
Which two statements about gas mixtures are true? [Section 13.1] (a) Gases always mix with other gases because the gas particles are too far apart to feel significant intermolecular attractions or repulsions. (b) Just like water and oil don’t mix in the liquid phase, two gases can be immiscible and not mix in the gas phase. (c) If you cool a gaseous mixture, you will liquefy all the gases at the same temperature. (d) Gases mix in all proportions in part because the entropy of the system increases upon doing so.
Open Question
The density of toluene (C7H8) is 0.867 g/mL, and the density of thiophene (C4H4S) is 1.065 g/mL. A solution is made by dissolving 8.10 g of thiophene in 250.0 mL of toluene. Assuming that the volumes of the solute and solvent are additive, what is the molarity of thiophene in the solution?
Open Question
If you compare the solubilities of the noble gases in water, you find that solubility increases from smallest atomic weight to largest, specifically: Ar < Kr < Xe. Which of the following statements is the best explanation? [Section 13.3] (a) The heavier the gas, the more it sinks to the bottom of the water and leaves room for more gas molecules at the top of the water. (b) The heavier the gas, the more dispersion forces it has, and therefore the more attractive interactions it has with water molecules. (c) The heavier the gas, the more likely it is to hydrogen-bond with water. (d) The heavier the gas, the more likely it is to make a saturated solution in water.
Open Question
You take a sample of water that is at room temperature and in contact with air and put it under a vacuum. Right away, you see bubbles leave the water, but after a little while, the bubbles stop. As you keep applying the vacuum, more bubbles appear. A friend tells you that the first bubbles were water vapor, and that the low pressure had reduced the boiling point of water, causing the water to boil. Another friend tells you that the first bubbles were gas molecules from the air (oxygen, nitrogen, and so forth) that were dissolved in the water. Which friend is most likely to be correct? What, then, is responsible for the second batch of bubbles? [Section 13.4]
Textbook Question

The figure shows two identical volumetric flasks containing the same solution at two temperatures. (b) Does the molality of the solution change with the change in temperature? [Section 13.4]

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Textbook Question

This portion of a phase diagram shows the vapor–pressure curves of a volatile solvent and of a solution of that solvent containing a nonvolatile solute. (b) What are the normal boiling points of the solvent and the solution? [Section 13.5]

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