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NSWChemistryQuick questions

Module 5: Equilibrium and Acid Reactions

Quick questions on Brønsted-Lowry acid-base theory explained: HSC Chemistry Module 5

8short Q&A pairs drawn directly from our worked dot-point answer. For full context and worked exam questions, read the parent dot-point page.

What are definitions?
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The definition focuses on the proton transfer itself, not on whether the reaction occurs in water.
What are conjugate acid-base pairs?
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When an acid donates a proton, it becomes a base (because it can now accept the proton back). When a base accepts a proton, it becomes an acid. The acid and base that differ by a single H+H^+ form a conjugate acid-base pair.
What is amphiprotic species?
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An amphiprotic species can act as either a Brønsted-Lowry acid or a Brønsted-Lowry base depending on what it reacts with. The most important examples:
What is comparison with Arrhenius theory?
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Arrhenius (1887): an acid produces H+H^+ in water, a base produces OH−OH^- in water.
What is hydrogen sulfate ion?
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Similarly acts as both an acid and a base.
What is q1?
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Define a Brønsted-Lowry acid and identify the conjugate base of H2SO4H_2SO_4, NH4+NH_4^+ and HCO3−HCO_3^-. [3 marks]
What is q2?
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Calculate the [H3O+][H_3O^+] produced when 0.0500 mol of HCl is dissolved in 250 mL of water, assuming full dissociation. [2 marks]
What is q3?
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Hydrogen carbonate is described as amphiprotic. (a) Write equations showing HCO3−HCO_3^- acting as an acid and as a base in water. (b) Identify the conjugate pairs in each equation.

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