Classify the solute represented in each of the following equations as a strong, weak, or nonelectrolyte: a. K₂SO₄(s) →H₂O 2K⁺(aq) + SO₄²⁻(aq)

Verified step by step guidance

1. Identify the type of compound: K₂SO₄ is an ionic compound.
2. Determine the solubility of the compound in water: K₂SO₄ is soluble in water.
3. Analyze the dissociation equation: K₂SO₄(s) → 2K⁺(aq) + SO₄²⁻(aq) shows complete dissociation into ions.
4. Classify the electrolyte: Since K₂SO₄ completely dissociates into ions, it is a strong electrolyte.
5. Conclude that strong electrolytes are compounds that fully dissociate into ions in solution, conducting electricity efficiently.

Key Concepts

Electrolytes

Electrolytes are substances that dissociate into ions when dissolved in water, allowing the solution to conduct electricity. They are classified into strong electrolytes, which completely dissociate into ions, weak electrolytes, which partially dissociate, and nonelectrolytes, which do not dissociate at all. Understanding these classifications is essential for analyzing solute behavior in aqueous solutions.

Strong Electrolytes

Strong electrolytes are compounds that fully dissociate into their constituent ions in solution. Examples include soluble salts like potassium sulfate (K₂SO₄), which dissociates completely into 2K⁺ and SO₄²⁻ ions in water. This complete dissociation is crucial for understanding the conductivity and chemical behavior of solutions.

Weak Electrolytes

Weak electrolytes are substances that only partially dissociate into ions in solution, resulting in a mixture of ionized and non-ionized molecules. Common examples include acetic acid and ammonia. The degree of dissociation affects the solution's conductivity and pH, making it important to distinguish between weak and strong electrolytes in chemical reactions.