Here are the essential concepts you must grasp in order to answer the question correctly.
Ionization of Weak Acids
Weak acids, like propionic acid, do not fully dissociate in solution. Instead, they establish an equilibrium between the undissociated acid and its ions. The extent of this ionization is characterized by the acid dissociation constant (Ka), which quantifies the strength of the acid and its ability to donate protons (H+) in solution.
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Percent Ionization
Percent ionization is a measure of the degree to which an acid dissociates in solution, expressed as a percentage. It is calculated using the formula: (concentration of ionized acid / initial concentration of acid) × 100%. This value helps to understand the strength of the acid in a given concentration and how it changes with dilution.
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Equilibrium Calculations
To calculate percent ionization, one must set up an equilibrium expression based on the initial concentration of the acid and the change in concentration due to ionization. This involves using the Ka value to find the concentration of ions at equilibrium, allowing for the determination of how much of the acid has ionized relative to its initial concentration.
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