Conjugate base of `[Cu(NH_(3))_(6)]^(2+)` is

Options

A. `[Cu(NH_(3))_(3) NH_(2)^(-)`
B. `[Cu (NH_(3))_(5)NH_(2)]^(+)`
C. `[Cu(NH_(3))_(4)NH_(2)]^(+)`
D. `[Cu(NH_(3))_(4)NH_(2)]^(2+)`

Answer

To find the conjugate base of the complex ion \([Cu(NH_3)_6]^{2+}\), we need to follow these steps:

### Step 1: Identify the Acid
The given complex ion \([Cu(NH_3)_6]^{2+}\) acts as a Brønsted-Lowry acid. This means it can donate a proton (H⁺) to form its conjugate base.

**Hint:** Remember that a conjugate base is formed when an acid donates a proton.

### Step 2: Determine the Proton Loss
In the complex ion \([Cu(NH_3)_6]^{2+}\), there are six ammonia (NH₃) ligands. When one of these ammonia molecules loses a proton (H⁺), it will convert from NH₃ to NH₂⁻ (amido group).

**Hint:** Identify which part of the complex will lose a proton to form the conjugate base.

### Step 3: Write the Conjugate Base
After one ammonia loses a proton, the new complex will be \([Cu(NH_3)_5(NH_2)]^{+}\). The overall charge of the complex will decrease by one because we have lost a positively charged proton.

**Hint:** Keep track of the charge changes when a proton is lost.

### Step 4: Finalize the Conjugate Base
Thus, the conjugate base of the complex ion \([Cu(NH_3)_6]^{2+}\) is \([Cu(NH_3)_5(NH_2)]^{+}\).

**Hint:** Ensure that the final structure reflects the loss of one proton and the corresponding charge adjustment.

### Summary
The conjugate base of \([Cu(NH_3)_6]^{2+}\) is \([Cu(NH_3)_5(NH_2)]^{+}\).