Question

Which of the following has the highest molar electrical conductance in aqueous solution?

• A. \( [\text{Pt(NH}_3\text{)}_6] \text{Cl}_4 \)
• B. \( [\text{Pt(NH}_3\text{)}_5 \text{Cl}] \text{Cl}_3 \)
• C. \( [\text{Pt(NH}_3\text{)}_4 \text{Cl}_2] \text{Cl}_2 \)
• D. \( [\text{Pt(NH}_3\text{)}_3 \text{Cl}_3] \text{Cl} \)

Hint:

For ionic compounds, the greater the number of dissociated ions in solution, the higher the electrical conductance.

Answer 1

The Correct Option is A

Step 1: Understanding molar electrical conductance.
Molar electrical conductance is related to the number of ions that dissociate in a solution. The more ions present, the higher the electrical conductance. Here, the higher the number of ions produced from dissociation, the higher the conductance. Step 2: Analysis of options.
(A) \( [\text{Pt(NH}_3\text{)_6] \text{Cl}_4 \):} This compound dissociates into more ions, resulting in higher electrical conductance.
(B) \( [\text{Pt(NH}_3\text{)_5 \text{Cl}] \text{Cl}_3 \):} This compound dissociates into fewer ions than option (A).
(C) \( [\text{Pt(NH}_3\text{)_4 \text{Cl}_2] \text{Cl}_2 \):} This compound dissociates into fewer ions than option (A).
(D) \( [\text{Pt(NH}_3\text{)_3 \text{Cl}_3] \text{Cl} \):} This compound dissociates into fewer ions than option (A).
Step 3: Conclusion.
The correct answer is (A) because \( [\text{Pt(NH}_3\text{)}_6] \text{Cl}_4 \) dissociates into more ions, giving the highest electrical conductance.