Question

Identify conjugate bases of \(\text{HCO}_{3}^{-}\) and \(\text{HS}^{-}\) respectively.

• A. \(\text{H}_{2}\text{CO}_{3}\) and \(\text{H}_{2}\text{S}\)
• B. \(\text{CO}_{3}^{--}\) and \(\text{S}^{--}\)
• C. \(\text{HCO}_{3}^{--}\) and \(\text{H}_{2}\text{S}\)
• D. \(\text{H}_{2}\text{CO}_{3}^{--}\) and \(\text{S}^{-}\)

Hint:

A conjugate base is formed when an acid loses one proton.

Answer 1

The Correct Option is B

Step 1: Understanding the Concept
According to the Bronsted-Lowry theory, the conjugate base of an acid is obtained by removing one \(\text{H}^{+}\).

Step 2: Apply to Each Ion
\(\text{HCO}_3^{-} - \text{H}^{+} \rightarrow \text{CO}_3^{2-}\)
\(\text{HS}^{-} - \text{H}^{+} \rightarrow \text{S}^{2-}\)

Step 3: Compare the options
The conjugate bases are \(\text{CO}_3^{2-}\) and \(\text{S}^{2-}\), option (B).

Final Answer:
The conjugate bases are CO3 2- and S2-. \[ \boxed{\text{(B) }\text{CO}_{3}^{2-}\text{ and S}^{2-}} \]