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Ch.16 - Aqueous Equilibria: Acids & Bases
Chapter 16, Problem 39c

The following pictures represent aqueous solutions of three acids HA1A = X, Y, or Z2; water molecules have been omitted for clarity.
Three diagrams showing aqueous solutions of acids HA1A = X, Y, or Z2 for strong acid identification.
(c) Which acid, if any, is a strong acid?

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Strong Acids

Strong acids are substances that completely dissociate into their ions in aqueous solution. This means that when a strong acid is added to water, it releases all of its hydrogen ions (H+) into the solution, resulting in a high concentration of H+ ions. Common examples include hydrochloric acid (HCl) and sulfuric acid (H2SO4). Identifying strong acids is crucial for understanding their behavior in chemical reactions and their impact on pH levels.
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Dissociation in Aqueous Solutions

Dissociation refers to the process by which an acid separates into its constituent ions when dissolved in water. For strong acids, this process is complete, while weak acids only partially dissociate. The extent of dissociation affects the acidity of the solution, which can be visualized in diagrams showing the distribution of ions in the solution. Understanding dissociation is essential for predicting the properties and reactivity of acids in solution.
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Acid-Base Theory

Acid-base theory encompasses various models that explain the behavior of acids and bases. The Brønsted-Lowry theory defines acids as proton donors and bases as proton acceptors. This framework helps in understanding how acids interact with water and other substances, influencing the pH and chemical equilibrium in solutions. Recognizing these interactions is vital for identifying strong acids and predicting their effects in chemical reactions.
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