The following pictures represent aqueous solutions of three acids HA1A = X, Y, or Z2; water molecules have been omitted for clarity.

(c) Which acid, if any, is a strong acid?

Verified step by step guidance

1. Identify the components in each diagram: red spheres represent hydrogen ions (H+), blue spheres represent anions (A-), and white spheres represent undissociated acid molecules (HA).
2. Recall that a strong acid completely dissociates in water, meaning it will produce a high concentration of H+ and A- ions with no undissociated HA molecules.
3. Examine each diagram to determine the extent of dissociation: look for the presence of H+ and A- ions versus undissociated HA molecules.
4. Compare the diagrams: the one with the highest number of H+ and A- ions and no undissociated HA molecules represents the strong acid.
5. Conclude which acid (X, Y, or Z) is the strong acid based on the diagram that shows complete dissociation.

Key Concepts

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.

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.

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.