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During the titration of a strong acid with a strong base, pH calculations are primarily based on the concentration of residual hydronium or hydroxide ions. Initially, a strong acid like hydrochloric acid fully dissociates, creating hydronium and chloride ions, resulting in a low pH. The addition of a strong base like sodium hydroxide alters the concentration of hydronium ions by neutralizing them. As more base is added, the pH gradually increases. At the equivalence point, all hydronium ions are neutralized, achieving a neutral pH. Beyond this point, the excess hydroxide ions dictate the pH, making the solution basic. The new pH can be calculated by considering the concentration of these excess hydroxide ions.

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TitrationStrong AcidStrong BasePHHydronium IonsHydroxide IonsNeutralizationEquivalence PointPH Calculation

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3.2 : Titration of a Strong Acid with a Strong Base

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3.1 : Acid–Base Titration: Overview

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3.3 : Titration of a Weak Acid with a Strong Base

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3.4 : Titration of a Weak Base with a Strong Acid

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3.5 : Titration of a Weak Acid with a Weak Base

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3.6 : Solution Composition During Acid/Base Titrations

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3.7 : Mixtures of Acids

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3.8 : Titration in Nonaqueous Solvents

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3.9 : Titration of Polyprotic Base with a Strong Acid

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3.10 : Titration of Polyprotic Acids with a Strong Base

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3.11 : Composition of Polyprotic Acid Solutions as a Function of pH

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3.12 : Buffers: Overview

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3.13 : Buffers: Buffer Capacity

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3.14 : Leveling Effect

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