Write the formula for the conjugate acid of each base. Express your answer as a chemical formula. ClO4- HSO4- CO3^2-
The Correct Answer and Explanation is:
To determine the conjugate acid of a base, we need to add a proton (H⁺) to the base. This protonation results in the formation of a conjugate acid.
- ClO₄⁻ (Perchlorate ion):
- The conjugate acid of ClO₄⁻ is formed when it accepts a proton (H⁺).
- Conjugate acid: HClO₄ (Perchloric acid)
- Explanation: Perchlorate (ClO₄⁻) is a base because it has the ability to accept a proton. When ClO₄⁻ accepts H⁺, it forms HClO₄, which is a strong acid.
- HSO₄⁻ (Hydrogen sulfate ion):
- The conjugate acid of HSO₄⁻ is formed when it accepts a proton (H⁺).
- Conjugate acid: H₂SO₄ (Sulfuric acid)
- Explanation: Hydrogen sulfate (HSO₄⁻) is an intermediate ion formed when sulfuric acid (H₂SO₄) dissociates. When HSO₄⁻ accepts a proton, it forms H₂SO₄, which is a strong acid and can further dissociate.
- CO₃²⁻ (Carbonate ion):
- The conjugate acid of CO₃²⁻ is formed when it accepts a proton (H⁺).
- Conjugate acid: HCO₃⁻ (Bicarbonate ion)
- Explanation: Carbonate (CO₃²⁻) is the conjugate base of carbonic acid (H₂CO₃). When CO₃²⁻ accepts a proton, it forms HCO₃⁻, also known as bicarbonate, which is weakly acidic.
Summary of the conjugate acids:
- ClO₄⁻ → HClO₄
- HSO₄⁻ → H₂SO₄
- CO₃²⁻ → HCO₃⁻
In each case, the conjugate acid is formed by protonating the base, which increases the number of hydrogen ions in the formula and thus converts the species into a more acidic form.
