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Ch.16 - Acid-Base Equilibria
Brown - Chemistry: The Central Science 15th Edition
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoBrown 15th EditionCh.16 - Acid-Base EquilibriaProblema 60
Capitolo 16, Problema 60

If a solution of HF 1Ka = 6.8 * 10-42 has a pH of 3.65, calculate the concentration of hydrofluoric acid.

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Identify the given values: the pH of the solution is 3.65 and the acid dissociation constant (Ka) for HF is 6.8 \(\times\) 10^{-42}.
Calculate the concentration of hydrogen ions [H^+] using the pH value: [H^+] = 10^{-pH}.
Set up the expression for the acid dissociation constant (Ka) for HF: Ka = \(\frac{[H^+][F^-]}{[HF]}\).
Assume that the initial concentration of HF is 'C' and that the change in concentration due to dissociation is 'x'. Therefore, [H^+] = x, [F^-] = x, and [HF] = C - x.
Substitute the values into the Ka expression: 6.8 \(\times\) 10^{-42} = \(\frac{x^2}{C - x}\). Solve for 'C' using the approximation that x is small compared to C.

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Acid-Base Equilibrium

Acid-base equilibrium refers to the balance between the concentrations of acids and their conjugate bases in a solution. In the case of weak acids like hydrofluoric acid (HF), this equilibrium is described by the acid dissociation constant (Ka), which quantifies the extent to which the acid donates protons (H+) to the solution. Understanding this concept is crucial for calculating the concentration of HF based on its pH.
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pH and pKa Relationship

The pH of a solution is a measure of its acidity, defined as the negative logarithm of the hydrogen ion concentration. The pKa, which is the negative logarithm of the Ka, provides a more convenient way to express the strength of an acid. The relationship between pH, pKa, and the concentrations of the acid and its conjugate base is described by the Henderson-Hasselbalch equation, which is essential for solving problems involving weak acids.
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Concentration Calculations

Concentration calculations involve determining the amount of solute present in a given volume of solution. For weak acids, the concentration can be derived from the pH and the dissociation constant (Ka). By using the pH to find the concentration of hydrogen ions and applying the equilibrium expression for the dissociation of the acid, one can calculate the initial concentration of the acid in the solution.
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