Which of the following has the highest molar conductivity in solution?

Options

A. `[Pt (NH_3)_6]Cl_4`
B. `[Pt (NH_3)_5Cl]Cl_3`
C. `[Pt (NH_3)_4Cl_2]Cl_2`
D. `[Pt (NH_3)_3Cl_3]Cl`

Answer

To determine which of the given compounds has the highest molar conductivity in solution, we need to analyze the dissociation of each compound into ions. Molar conductivity is directly related to the number of ions produced when a compound dissolves in solution. The more ions produced, the higher the molar conductivity.

### Step-by-Step Solution:

1. **Identify the Compounds**: The compounds given are:
- (i) [Pt(NH₃)₆]Cl₄
- (ii) [Pt(NH₃)₅Cl]Cl₃
- (iii) [Pt(NH₃)₄Cl₂]Cl₂
- (iv) [Pt(NH₃)₃Cl₃]Cl

2. **Dissociation of Each Compound**:
- For **(i) [Pt(NH₃)₆]Cl₄**:
- Dissociates into: [Pt(NH₃)₆]⁴⁺ + 4 Cl⁻
- Total ions = 1 (cation) + 4 (anions) = **5 ions**

- For **(ii) [Pt(NH₃)₅Cl]Cl₃**:
- Dissociates into: [Pt(NH₃)₅Cl]³⁺ + 3 Cl⁻
- Total ions = 1 (cation) + 3 (anions) = **4 ions**

- For **(iii) [Pt(NH₃)₄Cl₂]Cl₂**:
- Dissociates into: [Pt(NH₃)₄Cl]²⁺ + 2 Cl⁻
- Total ions = 1 (cation) + 2 (anions) = **3 ions**

- For **(iv) [Pt(NH₃)₃Cl₃]Cl**:
- Dissociates into: [Pt(NH₃)₃Cl]⁺ + 1 Cl⁻
- Total ions = 1 (cation) + 1 (anion) = **2 ions**

3. **Comparison of Total Ions**:
- [Pt(NH₃)₆]Cl₄ = 5 ions
- [Pt(NH₃)₅Cl]Cl₃ = 4 ions
- [Pt(NH₃)₄Cl₂]Cl₂ = 3 ions
- [Pt(NH₃)₃Cl₃]Cl = 2 ions

4. **Conclusion**:
- The compound with the highest number of ions is **[Pt(NH₃)₆]Cl₄**, which produces a total of 5 ions. Therefore, it has the highest molar conductivity in solution.

### Final Answer:
The compound with the highest molar conductivity in solution is **[Pt(NH₃)₆]Cl₄**.

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