Brønsted-Lowry Acids and Bases Flashcards | A-Level Chemistry OCR | Cognito

Define the term Brønsted-Lowry acid.

A Brønsted-Lowry acid is a proton donor.

For example, HCl acts as a Brønsted-Lowry acid according to the equation:

HCl_(aq) + H₂O_(l) ⇌ H₃O⁺_(aq) + Cl^-_(aq).

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Explain the concept of a conjugate acid-base pair.

A conjugate acid-base pair contains two species that can be interconverted by transfer of a proton.

In the forward direction, an acid releases a proton to form its conjugate base.

In the reverse direction, the conjugate base accepts a proton to form its conjugate acid.

The conjugate pairs, for the equilibrium between HCl and H₂O to form H₃O⁺ and Cl^- ions are:

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How many hydrogen ions can be replaced in monobasic acids?

Monobasic acids can replace one H⁺ ion per molecule.

For example. nitric acid (HNO₃) dissociates according to the equation: HNO_3(aq) ➔ H⁺_(aq) + NO₃^-_(aq)

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What is the formula of the hydronium ion?

H₃O⁺

The hydronium ion is also called the oxonium ion or hydroxonium ion.

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What is the formula for the ionic product of water (K_w)?

K_w = [H⁺_(aq)][OH^-_(aq)]

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Name and give the formulae of the conjugate acid of water.

The conjugate acid of water is the hydronium ion, H₃O⁺.

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Name and give the formulae of the conjugate base of water.

The conjugate base of water is the hydroxide ion, OH^-.

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How many hydrogen ions can be replaced in dibasic acids?

Dibasic acids can replace two H⁺ ions per molecule.

For example. sulfuric acid (H₂SO₄) dissociates according to the equation: H₂SO_4(aq) ➔ 2H⁺_(aq) + SO₄^2-_(aq)

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