Skip to main content
Ch.17 - Additional Aspects of Aqueous 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.17 - Additional Aspects of Aqueous EquilibriaProblema 17a
Capitolo 17, Problema 17a

a. Calculate the percent ionization of 0.007 M butanoic acid (𝐾𝑎=1.5×10−5).

Guida verificata passo dopo passo
1
Step 1: Write the ionization equation for butanoic acid (C3H7COOH) in water: C3H7COOH (aq) ⇌ C3H7COO- (aq) + H+ (aq).
Step 2: Set up the expression for the acid dissociation constant (Ka): Ka = [C3H7COO-][H+] / [C3H7COOH].
Step 3: Assume that the initial concentration of butanoic acid is 0.007 M and that the change in concentration due to ionization is x. Therefore, at equilibrium, [C3H7COO-] = x, [H+] = x, and [C3H7COOH] = 0.007 - x.
Step 4: Substitute these equilibrium concentrations into the Ka expression: 1.5 \(\times\) 10^{-5} = (x)(x) / (0.007 - x).
Step 5: Solve the equation for x, which represents the concentration of ionized butanoic acid. Then, calculate the percent ionization using the formula: \(\text{Percent Ionization}\) = \(\left\)( \(\frac{x}{0.007}\) \(\right\)) \(\times\) 100\%.

Risposta video verificata per un problema simile:

Questa soluzione video è stata consigliata dai nostri tutor come utile per risolvere questo problema.
Durata del video:
3m

Concetti chiave

Ecco i concetti essenziali che devi comprendere per rispondere correttamente alla domanda.

Ionization of Weak Acids

Weak acids, like butanoic acid, do not completely dissociate in solution. Instead, they establish an equilibrium between the undissociated acid and its ions. The degree of ionization is crucial for calculating the concentration of ions in solution, which directly affects the acid's strength and its pH.
Video consigliato:
Percorso guidato
01:15
Calculating Percent Ionization of Weak Acids

Equilibrium Constant (Ka)

The acid dissociation constant (Ka) quantifies the strength of an acid in solution. It is defined as the ratio of the concentration of the products (ions) to the concentration of the reactants (undissociated acid) at equilibrium. A smaller Ka value indicates a weaker acid, which is essential for determining the extent of ionization in weak acids like butanoic acid.
Video consigliato:
Percorso guidato
01:14
Equilibrium Constant K

Percent Ionization

Percent ionization is a measure of the extent to which an acid ionizes in solution, expressed as a percentage. It is calculated by dividing the concentration of ionized acid by the initial concentration of the acid, then multiplying by 100. This concept helps in understanding the effectiveness of an acid in solution and is particularly useful for comparing the strengths of different acids.
Video consigliato:
Percorso guidato
06:08
Percent Ionization Example
Pratica correlata
Domanda del libro di testo

(a) Calculate the percent ionization of 0.125 M lactic acid (Ka = 1.4 × 10-4).

941
views
Domanda del libro di testo

Consider the equilibrium B(aq) + H2O(l) ⇌ HB+(aq) + OH–(aq). Suppose that a salt of HB+(aq) is added to a solution of B(aq) at equilibrium. (c) Will the pH of the solution increase, decrease, or stay the same?

472
views
Domanda del libro di testo

(b) Calculate the percent ionization of 0.0075 M butanoic acid in a solution containing 0.085 M sodium butanoate.

522
views
1
comments
Domanda del libro di testo

(b) Calculate the percent ionization of 0.125 M lactic acid in a solution containing 0.0075 M sodium lactate.