Indicate whether aqueous solutions of each of the following solutes contain only ions, only molecules, or mostly molecules and a few ions:a. acetic acid, HC₂H₃O₂, a weak electrolyte

Verified step by step guidance

1. Identify the type of solute: Acetic acid (HC₂H₃O₂) is a weak acid and a weak electrolyte.
2. Understand the behavior of weak electrolytes: Weak electrolytes partially dissociate into ions in solution.
3. Write the dissociation equation: HC₂H₃O₂ (aq) ⇌ H⁺ (aq) + C₂H₃O₂⁻ (aq).
4. Recognize the equilibrium: In an aqueous solution, the equilibrium favors the undissociated form of acetic acid, meaning most of the solute remains as molecules.
5. Conclude the composition: The solution contains mostly molecules and a few ions.

Key Concepts

Electrolytes

Electrolytes are substances that dissociate into ions when dissolved in water, allowing the solution to conduct electricity. They can be classified as strong electrolytes, which completely dissociate into ions, or weak electrolytes, which only partially dissociate. Understanding the behavior of electrolytes is crucial for predicting the composition of solutions.

Weak Acids

Weak acids, such as acetic acid (HC₂H₃O₂), do not fully ionize in solution. Instead, they establish an equilibrium between the undissociated molecules and the ions produced. This means that in a solution of a weak acid, there will be a mixture of molecules and ions, with the majority remaining as molecules.

Chemical Equilibrium

Chemical equilibrium occurs when the rate of the forward reaction equals the rate of the reverse reaction, resulting in constant concentrations of reactants and products. In the case of weak acids, this equilibrium is essential for understanding how many molecules remain undissociated compared to the ions present in solution, influencing the overall properties of the solution.