Conjugate acids and bases

Given the equation:

H₂SO₄ + H₂O ↔ H₃O⁺ + HSO₄^{- 1}

What is the acid?

• H₂SO₄

• H₂O

• H₃O⁺

• HSO₄^{- 1}

Tags

NGSS.HS-PS1-2

Given the equation:

H₂SO₄ + H₂O ↔ H₃O⁺ + HSO₄^{- 1}

What is the conjugate acid?

• H₂SO₄

• H₂O

• H₃O⁺

• HSO₄^{- 1}

Given the equation:

H₂SO₄ + H₂O ↔ H₃O⁺ + HSO₄^{- 1}

What is the conjugate base?

• H₂SO₄

• H₂O

• H₃O⁺

• HSO₄^{- 1}

Given the equation:

H₂SO₄ + H₂O ↔ H₃O⁺ + HSO₄^{- 1}

What is the base?

• H₂SO₄

• H₂O

• H₃O⁺

• HSO₄^{- 1}

Given the equation HF + H₂O ↔ H₃O⁺ + F^-1

^{Which is the acid?}

• HF

• H₂O

• H₃O⁺

• F^-1

Given the equation HF + H₂O ↔ H₃O⁺ + F^-1

^{Which is the conjugate acid?}

• HF

• H₂O

• H₃O⁺

• F^-1

Given the equation HF + H₂O ↔ H₃O⁺ + F^-1

^{Which is the conjugate base?}

• HF

• H₂O

• H₃O⁺

• F^-1

Given the equation HF + H₂O ↔ H₃O⁺ + F^-1

^{Which is the base?}

• HF

• H₂O

• H₃O⁺

• F^-1

Given the equation:

PO₄^3‑ + H₂O ↔ HPO₄^2‑ + OH^-

_{Which species is the acid?}

• PO₄^3‑

• H₂O

• HPO₄^2‑

• OH^-

By definition, a Bronsted-Lowry acid is a:

• proton donor

• proton acceptor

• Increases the concentration of H₃O⁺

• Increases the concentration of OH^-