The conjugate acid of `S_(2)O_(8)^(-2)`

Options

A. `H_(2)S_(2)O_(8)`
B. `H_(2)S_(4)`
C. `HSO_(4)^(-)`
D. `HS_(2)O_(8)^(-)`

Answer

To determine the conjugate acid of \( S_2O_8^{2-} \), we can follow these steps:

### Step 1: Understand the concept of conjugate acids and bases
A conjugate acid is formed when a base accepts a proton (H⁺ ion). In this case, \( S_2O_8^{2-} \) acts as a base.

**Hint:** Remember that the conjugate acid is formed by adding a proton (H⁺) to the base.

### Step 2: Write the reaction for the formation of the conjugate acid
When \( S_2O_8^{2-} \) (the base) accepts a proton, the reaction can be written as:
\[ S_2O_8^{2-} + H^+ \rightarrow HS_2O_8^{-} \]

**Hint:** Pay attention to the charge balance in the reaction.

### Step 3: Identify the conjugate acid
From the reaction, we can see that the conjugate acid formed is \( HS_2O_8^{-} \).

**Hint:** The conjugate acid will have one more hydrogen atom than the base and the charge will be adjusted accordingly.

### Step 4: Conclusion
Thus, the conjugate acid of \( S_2O_8^{2-} \) is \( HS_2O_8^{-} \).

**Final Answer:** The conjugate acid of \( S_2O_8^{2-} \) is \( HS_2O_8^{-} \).

### Summary of Steps:
1. Understand the definition of conjugate acids and bases.
2. Write the reaction showing the base accepting a proton.
3. Identify the resulting conjugate acid.
4. Conclude with the final answer.