Final answer:
The conjugate acids for the bases O²⁻, H₂PO₄⁻, SO₄²⁻, and CH₃NH₂ are OH⁻, H₃PO₄, HSO₄⁻, and CH₃NH₃+ respectively. Each conjugate acid results from the corresponding base accepting a proton (H+).
Step-by-step explanation:
The conjugate acids for the given Bronsted-Lowry bases are:
-
- a. For O²⁻, the conjugate acid is OH⁻ as it can accept a proton (H+) to form OH⁻.
-
- b. For H₂PO₄⁻, the conjugate acid is H₃PO₄ because upon gaining a proton, it forms H₃PO₄.
-
- c. For SO₄²⁻, the conjugate acid is HSO₄⁻, which results from the addition of a proton to SO₄²⁻.
-
- d. For CH₃NH₂, the conjugate acid is CH₃NH₃+ since accepting a proton yields this species.