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Khan Academy offers a comprehensive guide on Bronsted-Lowry acid-base theory, explaining the concepts of acids and bases in chemistry.
Introduction to acid–base reactions (practice) | Khan Academy
Check your understanding of Brønsted–Lowry acids, bases, and conjugate acid–base pairs in this set of free practice questions designed for AP Chemistry students.
Acids and Bases - Khan Academy
Brønsted–Lowry acids and bases. Autoionization of water. Water autoionization and Kw. Definition of pH. Strong acid solutions. Strong base solutions. Acid strength, anion size, and bond energy.
Weak acid–weak base reactions (video) | Khan Academy
To identify conjugate acid base pairs remember there's only one proton or one H plus difference between an acid and it's conjugate base. So when HA donates its proton and turns into A minus, A minus must be the conjugate base to HA.
pH of salt solutions - Khan Academy
pH of salt solutions. The pH of a salt solution is determined by the relative strength of its conjugated acid-base pair. Salts can be acidic, neutral, or basic. Salts that form from a strong acid and a weak base are acid salts, like ammonium chloride (NH4Cl).
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When a weak base and a strong acid are mixed, they react according to the following net-ionic equation: B(aq) + H₃O⁺(aq) → HB⁺(aq) + H₂O(l). If the acid and base are equimolar, the pH of the resulting solution can be determined by considering the equilibrium reaction of HB⁺ with water.
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Identifying weak acids and strong acids (practice) | Khan Academy
Lesson 1: Acids, bases, and pH. Arrhenius acids and bases. Arrhenius acids and bases. pH, pOH, and the pH scale. Brønsted-Lowry acids and bases. Brønsted–Lowry acids and bases. Autoionization of water. Water autoionization and Kw. Definition of pH.
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So we're talking about a conjugate acid-base pair here. HA and A minus. And for our problem HA, the acid, would be NH four plus and the base, A minus, would be NH three or ammonia.