In a demonstration of strong electrolytes, weak electrolytes, and nonelectrolytes, Professor Popsnorkle used a lightbulb apparatus that showed how much a solution conducted electricity by the brightness of the lightbulb. When pure water was tested, the bulb did not light. Then Professor Popsnorkle tested the following aqueous solutions. Which one caused the bulb to burn the brightest? A)table salt, NaCl B)ethanol, CH₃CH₂OH C)table sugar, C₁₂H₂₂O₁₁ D)acetic acid, CH₃COOH E)methanol, CH₃OH

Question

Quizplus · Accepted Answer

Table salt (NaCl) is a strong electrolyte, meaning that when it is dissolved in water, it completely dissociates into ions that can conduct electricity. This results in a very bright lightbulb, indicating a high conductivity of electricity. Ethanol (B) and table sugar (C) are both nonelectrolytes, meaning they do not produce ions in solution and thus cannot conduct electricity. Acetic acid (D) is a weak electrolyte, meaning it partially dissociates into ions in solution and can conduct some electricity, but not to the extent of a strong electrolyte like NaCl. Methanol (E) is also a weak electrolyte.

In a Demonstration of Strong Electrolytes, Weak Electrolytes, and Nonelectrolytes