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Chapter 13: Problem 25

Explain why vitamin \(\mathrm{C}\) is soluble in water.

Short Answer

Expert verified
Vitamin C is soluble in water due to its polar nature and the presence of several -OH groups, which facilitate hydrogen bonding with water, causing it to dissolve easily.

Step by step solution

01

Understanding the concept of Solubility

Solubility is the ability of a solute (in this case, vitamin C) to dissolve in a solvent (water). This depends primarily on two factors: 'like dissolves like' principle stating that polar substances will dissolve in polar solvents and non-polar substances will dissolve in non-polar solvents, and the solubility rules.
02

Identifying the nature of vitamin C and water

Vitamin C, or ascorbic acid, is a polar molecule because it has several polar bonds due to the presence of multiple -OH groups. Water (H2O) is a polar solvent, meaning it has slightly positive and slightly negative ends.
03

Explaining the solubility of Vitamin C in Water

Because both vitamin C and water are polar, they are attracted to each other. When vitamin C is placed in water, the polar water molecules interact with the polar vitamin C molecules. The positive hydrogen ends of water are attracted to the negatively charged oxygen ends of the vitamin C molecule (from its -OH groups). This is due to hydrogen bonding. These attractions overcome the forces holding the vitamin C molecules together, causing it to dissolve in water.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Polar Molecules
Polar molecules are a fundamental concept to understand why certain substances dissolve in others. These molecules have a distinct separation of charges. This means one end of the molecule is slightly negative, while the other is slightly positive. This happens because of differences in electronegativity between atoms within the molecule, leading to unequal sharing of electrons.

Vitamin \(\text{C}\), also known as ascorbic acid, is a perfect example. It possesses multiple hydroxyl (\(-OH\)) groups, which contribute to its polarity. Water is similarly polar because of its bent shape and the significant electronegativity difference between hydrogen and oxygen atoms.
  • Polar molecules like water and vitamin \(\text{C}\) interact strongly with each other due to their charge differences.
  • These interactions help explain phenomena such as solubility.
Hydrogen Bonding
Hydrogen bonding is a special type of attraction between molecules, a key player in solubility. This bond occurs when a hydrogen atom, which is covalently bonded to a more electronegative atom like oxygen or nitrogen, experiences an attraction to another electronegative atom.

In the case of vitamin \(\text{C}\) dissolving in water, the hydrogen in the hydroxyl groups can form hydrogen bonds with the oxygen of the water molecules. These interactions are crucial because they disrupt the existing intermolecular forces between vitamin \(\text{C}\) molecules, allowing them to disperse in the solvent.
  • Hydrogen bonds are strong compared to typical dipole-dipole attractions, which helps in dissolving polar compounds.
  • These bonds are directional, which means they align the molecules in specific orientations, leading to better solubility.
Like Dissolves Like Principle
The 'Like Dissolves Like' principle is a wonderfully simple yet powerful guideline in chemistry for predicting solubility. This rule states that polar solvents dissolve polar solutes, while non-polar solvents dissolve non-polar solutes. This happens because similar types of intermolecular forces are present.

Since both vitamin \(\text{C}\) and water are polar, they fit the "like" category and hence mix well, providing a classic example of this principle in action. When we put vitamin \(\text{C}\) in water, their similar polar attractions help the molecules to blend.
  • This principle is an easy way to remember basic solubility rules.
  • It applies broadly, beyond vitamin \(\text{C}\), to a wide range of chemical substances.

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Most popular questions from this chapter

What ratio does molarity express?

Name a unit of concentration commonly used to express small concentrations.

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