`S^(-2)` is the conjugate base of `HS^(-)`

Answer

To determine whether `S^(-2)` is the conjugate base of `HS^(-)`, we can follow these steps:

### Step 1: Understand the concept of conjugate acids and bases
A conjugate base is formed when an acid donates a proton (H⁺ ion). The species that remains after the proton is removed is the conjugate base.

**Hint:** Remember that the conjugate base is what you get after an acid loses a proton.

### Step 2: Identify the acid in this case
In this scenario, `HS^(-)` is the species we are considering. It can act as an acid because it can donate a proton.

**Hint:** Look for the species that can lose a proton to identify the acid.

### Step 3: Determine what happens when `HS^(-)` donates a proton
When `HS^(-)` donates a proton (H⁺), it loses that positive charge and transforms into `S^(-2)`.

**Hint:** When an acid donates H⁺, the remaining species is the conjugate base.

### Step 4: Conclude the relationship between `HS^(-)` and `S^(-2)`
Since `HS^(-)` donates a proton to become `S^(-2)`, we can conclude that `S^(-2)` is indeed the conjugate base of `HS^(-)`.

**Hint:** Check if the charge and composition change correctly after the proton donation.

### Final Answer
Yes, `S^(-2)` is the conjugate base of `HS^(-)`.