The following aqueous solutions were tested with a light bulb conductivity apparatus, as shown in Figure 4.3. What result—dark, dim, or bright—do you expect from each? (a) 0.10 M hydrofluoric acid (b) 0.10 M sodium chloride (c) 0.10 M glucose (C6H12O6)

Electrolytes are substances that dissociate into ions when dissolved in water, allowing the solution to conduct electricity. Strong electrolytes, like sodium chloride, fully dissociate into ions, while weak electrolytes, such as hydrofluoric acid, only partially dissociate. Nonelectrolytes, like glucose, do not produce ions in solution and therefore do not conduct electricity.

The conductivity of a solution is determined by the presence and concentration of ions. A bright light bulb indicates a high concentration of ions, resulting in strong conductivity, while a dim light suggests fewer ions. A dark result means no significant ion presence, indicating poor or no conductivity.

The concentration of a solute affects the number of ions available for conductivity. In the case of 0.10 M solutions, the degree of ionization is crucial; strong electrolytes like sodium chloride will fully ionize, while weak acids like hydrofluoric acid will only partially ionize, leading to different conductivity outcomes. Glucose, being a nonelectrolyte, will not contribute to conductivity regardless of its concentration.