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Ch.18 - Aqueous Ionic Equilibrium
Tro - Chemistry: A Molecular Approach 6th Edition
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoTro 6th EditionCh.18 - Aqueous Ionic EquilibriumProblema 78e
Capitolo 18, Problema 78e

A 30.0-mL sample of 0.165 M propanoic acid is titrated with 0.300 M KOH. Calculate the pH at each volume of added base: one-half equivalence point.

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Identify the reaction: Propanoic acid (CH₃CH₂COOH) reacts with KOH to form propanoate ion (CH₃CH₂COO⁻) and water.
Determine the moles of propanoic acid initially present using the formula: \( \text{moles} = \text{concentration} \times \text{volume} \).
Calculate the volume of KOH needed to reach the equivalence point using the stoichiometry of the reaction and the initial moles of propanoic acid.
Find the volume of KOH at the one-half equivalence point, which is half of the volume needed to reach the equivalence point.
At the one-half equivalence point, the concentration of propanoic acid equals the concentration of propanoate ion, so the pH equals the \( pK_a \) of propanoic acid. Use the \( pK_a \) value to determine the pH.

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Titration

Titration is a quantitative analytical technique used to determine the concentration of a solute in a solution. It involves the gradual addition of a titrant (in this case, KOH) to a solution containing the analyte (propanoic acid) until the reaction reaches its equivalence point, where stoichiometrically equivalent amounts of acid and base have reacted.
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03:04
Acid-Base Titration

Equivalence Point and Half-Equivalence Point

The equivalence point in a titration is the stage at which the amount of titrant added is stoichiometrically equivalent to the amount of substance in the sample. The half-equivalence point occurs when half of the acid has been neutralized, which is significant because it allows for the calculation of pH using the Henderson-Hasselbalch equation, as the concentrations of the acid and its conjugate base are equal.
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At the Equivalence Point

Henderson-Hasselbalch Equation

The Henderson-Hasselbalch equation relates the pH of a solution to the pKa of the acid and the ratio of the concentrations of the conjugate base to the acid. It is expressed as pH = pKa + log([A-]/[HA]). At the half-equivalence point, the pH equals the pKa of the acid, simplifying the calculation of pH in buffer solutions.
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Henderson-Hasselbalch Equation
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