Conjugate acid of `[Zn(OH)(H_(2)O)_(5)]^(2+)`  is

Options

A. `[Zn(H_(2)O)_(5)]^(2+)`
B. `[Zn(H_(2)O)_(6)]^(+3)`
C. `[Zn(OH)(H_(2)O)_(6)]^(+3)`
D. `[Zn(OH)(H_(2)O)_(6)]^(+2)`

Answer

To find the conjugate acid of the complex ion \([Zn(OH)(H_2O)_5]^{2+}\), we can follow these steps:

### Step 1: Identify the nature of the complex
The given complex \([Zn(OH)(H_2O)_5]^{2+}\) contains a hydroxide ion (\(OH^-\)), which indicates that this complex can act as a base.

**Hint:** Remember that a conjugate acid is formed when a base accepts a proton (\(H^+\)).

### Step 2: Determine how the base behaves
Since \([Zn(OH)(H_2O)_5]^{2+}\) can accept a proton, we can write the reaction as follows:
\[ [Zn(OH)(H_2O)_5]^{2+} + H^+ \rightarrow [Zn(H_2O)_6]^{3+} \]

**Hint:** When a base accepts a proton, it typically forms a new species that is one protonated form of the original base.

### Step 3: Analyze the resulting species
When the hydroxide ion (\(OH^-\)) in the complex accepts a proton, it transforms into water (\(H_2O\)). Therefore, the complex changes from \([Zn(OH)(H_2O)_5]^{2+}\) to \([Zn(H_2O)_6]^{3+}\).

**Hint:** The change in the number of water molecules indicates that one \(OH^-\) has been converted into \(H_2O\).

### Step 4: Determine the charge of the new complex
Initially, the charge of the complex was \(+2\) (from \([Zn(OH)(H_2O)_5]^{2+}\)). When it accepts a proton, the overall charge increases by \(1\) (due to the addition of \(H^+\)), resulting in a new charge of \(+3\).

**Hint:** Keep track of the charge changes when protons are added or removed.

### Step 5: Conclusion
Thus, the conjugate acid of \([Zn(OH)(H_2O)_5]^{2+}\) is \([Zn(H_2O)_6]^{3+}\).

**Final Answer:** The conjugate acid is \([Zn(H_2O)_6]^{3+}\).

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