The number of ions given by `[Pt(NH_(3))_(6)]Cl_(4)` in aqueous solution will be

Options

A. two
B. three
C. five
D. eleven .

Explanation

To determine the number of ions produced by the coordination compound \([Pt(NH_3)_6]Cl_4\) in aqueous solution, we can follow these steps:

### Step 1: Identify the components of the compound
The compound \([Pt(NH_3)_6]Cl_4\) consists of a complex ion \([Pt(NH_3)_6]^{2+}\) and four chloride ions \(Cl^-\). The square brackets indicate that \([Pt(NH_3)_6]\) is a coordination complex where platinum (Pt) is the central metal atom surrounded by six ammonia (NH₃) ligands.

**Hint:** Look for the complex ion within the square brackets and the ions outside of them.

### Step 2: Determine the charge of the complex ion
The complex ion \([Pt(NH_3)_6]^{2+}\) carries a \(+2\) charge. This is because the ammonia ligands are neutral and do not contribute any charge. Therefore, the overall charge of the complex ion is determined solely by the platinum.

**Hint:** Remember that neutral ligands do not affect the charge of the complex.

### Step 3: Identify the ions produced in solution
When \([Pt(NH_3)_6]Cl_4\) is dissolved in water, the chloride ions dissociate from the complex. Since there are four chloride ions, they will dissociate into \(4 Cl^-\) ions.

**Hint:** Look for ions that are outside the brackets; they will dissociate in solution.

### Step 4: Calculate the total number of ions in solution
From the dissociation, we have:
- 1 complex ion: \([Pt(NH_3)_6]^{2+}\)
- 4 chloride ions: \(4 Cl^-\)

Adding these together gives us:
\[ 1 + 4 = 5 \text{ ions} \]

### Conclusion
The total number of ions produced by \([Pt(NH_3)_6]Cl_4\) in aqueous solution is **5**.

**Final Answer:** 5 ions

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