Classify each of the following substances as a nonelectrolyte, weak electrolyte, or strong electrolyte in water: (a) HF (b) C₆H₅COOH (benzoic acid) (c) C₆H₆ (benzene) (d) CoCl₃ (e) AgNO₃.

Verified step by step guidance

1. Identify the type of compound HF is. HF, or hydrofluoric acid, is a binary acid consisting of hydrogen and fluorine.
2. Understand the behavior of HF in water. When dissolved, HF partially ionizes in water, releasing hydrogen ions (H+) and fluoride ions (F-).
3. Recall the definition of electrolytes. Electrolytes are substances that dissolve in water to produce a solution that conducts electricity due to the presence of ions.
4. Determine the extent of ionization. HF does not completely ionize in water but does so partially, which is characteristic of weak acids.
5. Classify the substance based on ionization. Since HF partially ionizes in water, it is classified as a weak electrolyte.

Key Concepts

Electrolytes

Electrolytes are substances that dissociate into ions when dissolved in water, allowing the solution to conduct electricity. They are classified into three categories: strong electrolytes, which completely dissociate into ions; weak electrolytes, which partially dissociate; and nonelectrolytes, which do not dissociate at all.

Strong vs. Weak Electrolytes

Strong electrolytes, such as sodium chloride, fully ionize in solution, resulting in a high concentration of ions. In contrast, weak electrolytes, like acetic acid, only partially ionize, leading to a lower concentration of ions. This distinction is crucial for understanding the conductivity and chemical behavior of solutions.

Hydrofluoric Acid (HF)

Hydrofluoric acid (HF) is a weak acid and a weak electrolyte. When dissolved in water, it partially ionizes into hydrogen ions (H⁺) and fluoride ions (F⁻), but not completely. This partial dissociation is what classifies HF as a weak electrolyte, affecting its conductivity and reactivity in aqueous solutions.