Chemistry · Unit 3 · Chemical equilibrium systems · Chemical equilibrium
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The dissociation reactions of carbonic acid (H₂CO₃(aq)) are shown below. H₂CO₃(aq) ⇌ H⁺(aq) + HCO₃⁻(aq) Ka₁ = 4.3 × 10⁻⁷ HCO₃⁻(aq) ⇌ H⁺(aq) + CO₃²⁻(aq) Ka₂ = 4.8 × 10⁻¹¹ Identify an amphiprotic species from the dissociation reactions. Explain your reasoning.
Which of the following species can act as both a Brønsted-Lowry acid and a Brønsted-Lowry base?
Which of the following species can act as both a Brønsted-Lowry acid and a Brønsted-Lowry base in aqueous solution?