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Ch.17 - Aqueous Ionic Equilibrium
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoTro 4th EditionCh.17 - Aqueous Ionic EquilibriumProblema 38
Capitolo 17, Problema 38

Use the Henderson–Hasselbalch equation to calculate the pH of each solution in Problem 30.

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Identify the components of the buffer solution: the weak acid (HA) and its conjugate base (A^-).
Determine the concentrations of the weak acid [HA] and its conjugate base [A^-] in the solution.
Find the pKa of the weak acid. This can often be found in a table of acid dissociation constants.
Use the Henderson–Hasselbalch equation: \( \text{pH} = \text{pKa} + \log \left( \frac{[A^-]}{[HA]} \right) \).
Substitute the values of pKa, [A^-], and [HA] into the equation to calculate the pH.

Concetti chiave

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Henderson-Hasselbalch Equation

The Henderson-Hasselbalch equation is a mathematical formula used to calculate the pH of a buffer solution. It relates the pH of the solution to the pKa of the acid and the ratio of the concentrations of the conjugate base to the acid. The equation is expressed as pH = pKa + log([A-]/[HA]), where [A-] is the concentration of the base and [HA] is the concentration of the acid.
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Percorso guidato
02:40
Henderson-Hasselbalch Equation

Buffer Solutions

Buffer solutions are mixtures that can resist changes in pH when small amounts of acid or base are added. They typically consist of a weak acid and its conjugate base or a weak base and its conjugate acid. Understanding how buffers work is essential for applying the Henderson-Hasselbalch equation, as it helps in determining how the pH will change in response to the addition of acids or bases.
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Percorso guidato
03:02
Buffer Solutions

pKa and Acid-Base Equilibrium

The pKa is a measure of the strength of an acid in solution, defined as the negative logarithm of the acid dissociation constant (Ka). It indicates the pH at which half of the acid is dissociated into its conjugate base. Knowing the pKa of the acid involved in the buffer system is crucial for using the Henderson-Hasselbalch equation effectively, as it helps predict the pH based on the concentrations of the acid and its conjugate base.
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04:30
Acid-Base Indicators
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