Classify each of the following substances as a strong electrolyte, weak electrolyte, or nonelectrolyte. (a) HBr (b) HF (c) NaClO4 (d) (NH4)2CO3 (e) NH3 (f) Ethyl alcohol

Verified step by step guidance

1. Identify the nature of each substance: acids, bases, salts, or molecular compounds.
2. For acids, determine if they are strong or weak based on common strong acids (e.g., HBr is a strong acid, HF is a weak acid).
3. For salts, check if they are soluble in water. Soluble salts like NaClO4 and (NH4)2CO3 are strong electrolytes.
4. For bases, identify if they are strong or weak. NH3 is a weak base and thus a weak electrolyte.
5. For molecular compounds like ethyl alcohol, determine if they ionize in water. Ethyl alcohol does not ionize, so it is a nonelectrolyte.

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, and weak electrolytes, which only partially dissociate. Nonelectrolytes do not dissociate into ions and therefore do not conduct electricity.

Strong vs. Weak Electrolytes

Strong electrolytes, such as HBr and NaClO4, fully ionize in solution, resulting in a high concentration of ions. Weak electrolytes, like HF and NH3, only partially ionize, leading to a lower concentration of ions. The degree of ionization is crucial for determining the conductivity of the solution.

Examples of Electrolytes

Common examples of strong electrolytes include strong acids and soluble salts, while weak electrolytes include weak acids and bases. For instance, HBr is a strong acid and fully dissociates, while HF is a weak acid and only partially dissociates. Understanding these classifications helps in predicting the behavior of substances in solution.