Assertion The complex `[Co(NH_(3))_(3)CI_(3)]` gives no precipitate with `AgNO_(3)` solution
Reason The given complex is non-ionisable .

Options

A. If both `(A)` and ` (R )` are correct and `(R )` is the correct explanation of `(A ) ` .
B. If both `(A)` and ` (R )` are correct and `(R )` is the correct explanation of `(A ) ` .
C. If`(A)` is correct, but `( R )` is incorrect .
D. Both `(A)` and `(R ) ` are incorrect .

Answer

To analyze the assertion and reason provided in the question, we will break down the information step by step.

### Step-by-Step Solution:

1. **Understanding the Complex**:
The complex given is `[Co(NH₃)₃Cl₃]`. This indicates that cobalt (Co) is coordinated with three ammonia (NH₃) ligands and three chloride (Cl) ligands.

2. **Identifying the Nature of the Complex**:
In coordination chemistry, a complex can be either ionizable or non-ionizable. Ionizable complexes contain counter ions that can dissociate in solution. Non-ionizable complexes do not dissociate into ions in solution.

3. **Analyzing the Composition of the Complex**:
The complex `[Co(NH₃)₃Cl₃]` does not explicitly show any counter ions. The ammonia ligands are neutral, and while chloride is typically an anion, in this case, it is part of the coordination sphere and does not act as a counter ion.

4. **Interaction with AgNO₃**:
When a solution of AgNO₃ is added to a solution containing ions, Ag⁺ ions can react with Cl⁻ ions to form a precipitate of AgCl. However, since `[Co(NH₃)₃Cl₃]` does not dissociate into free Cl⁻ ions (due to the absence of counter ions), there will be no AgCl precipitate formed.

5. **Conclusion on Assertion and Reason**:
- **Assertion**: The complex `[Co(NH₃)₃Cl₃]` gives no precipitate with AgNO₃ solution. This is true.
- **Reason**: The given complex is non-ionizable. This is also true, as there are no free ions present to react with AgNO₃.

6. **Final Statement**:
Both the assertion and the reason are correct, and the reason provided correctly explains the assertion.