Question

Let C_NaCl and \[\ce{C{_{BaSO_4}}}\] be the conductances (in S) measured for saturated aqueous solutions of NaCl and BaSO₄ respectively, at a temperature T. Which of the following is false?

Options

• Ionic mobilities of ions from both salts increase with T.

• C_NaCl >> \[\ce{C{_{BaSO_4}}}\], at a given T

• \[\ce{C{_{BaSO_4}}}\] (T₂) > \[\ce{C{_{BaSO_4}}}\] (T₁) for T₂ > T₁

• C_NaCl (T₂) > C_NaCl (T₁) for T₂ > T₁

Answer 1

Ionic mobilities of ions from both salts increase with T.

Explanation:

1. As temperature rises, ionic mobilities decrease due to random motion, resulting in shorter relaxation times and slower drift speeds.
2. NaCl is a totally soluble salt, while BaSO₄ is sparingly soluble, resulting in C₁ >> C₂.
3. As the temperature rises, the conductivity increases.