Formic acid, HCOOH, is a weak electrolyte. What solutes are present in an aqueous solution of this compound?

Verified step by step guidance

1. Identify that formic acid (HCOOH) is a weak acid, which means it partially ionizes in water.
2. Recognize that in an aqueous solution, formic acid will exist primarily as undissociated HCOOH molecules.
3. Understand that a small fraction of HCOOH will dissociate into H+ ions and HCOO- ions (formate ions).
4. Write the chemical equilibrium equation for the dissociation: HCOOH ⇌ H+ + HCOO-.
5. Conclude that the solutes present in the solution are HCOOH, H+, and HCOO-.

Key Concepts

Weak Electrolytes

Weak electrolytes are substances that partially dissociate into ions when dissolved in water. Unlike strong electrolytes, which completely ionize, weak electrolytes exist in equilibrium between their undissociated form and their ions. This means that in a solution of a weak electrolyte, both the intact molecules and the ions are present.

Dissociation of Acids

The dissociation of acids refers to the process by which an acid releases protons (H⁺ ions) into solution. In the case of formic acid (HCOOH), it dissociates into H⁺ and HCOO⁻ (formate ion). This process is crucial for understanding the behavior of acids in solution and their ability to conduct electricity.

Equilibrium in Solutions

In a solution of a weak electrolyte like formic acid, an equilibrium is established between the undissociated acid and its ions. This equilibrium can be represented by the equation: HCOOH ⇌ H⁺ + HCOO⁻. The position of this equilibrium is influenced by factors such as concentration and temperature, affecting the relative amounts of the species present in the solution.