Acid-base equilibrium describes the state where the rate of acid and base reactions are equal, resulting in a stable pH. This equilibrium is governed by equilibrium constants like $K_a$ (acid dissociation constant) and $K_b$ (base dissociation constant), which indicate the strength of an acid or base. Understanding these concepts is crucial for predicting the behavior of acids and bases in various solutions and chemical reactions. Buffers, solutions that resist changes in pH, are a practical application of acid-base equilibrium.
Match the term with its correct definition:
| Term | Definition |
|---|---|
| 1. Acid | A. A substance that accepts protons ($H^+$). |
| 2. Base | B. A solution that resists changes in pH. |
| 3. $K_a$ | C. A substance that donates protons ($H^+$). |
| 4. $pH$ | D. Acid dissociation constant. |
| 5. Buffer | E. A measure of the acidity or basicity of a solution. |
Complete the following paragraph using the words: conjugate, equilibrium, $K_b$, protons, water.
Acid-base reactions involve the transfer of _______. In aqueous solutions, _______ plays a crucial role. The strength of a base is quantified by its $_______$ value. The relationship between an acid and its corresponding base is described using the term _______ pair. Acid-base _______ is achieved when the forward and reverse reaction rates are equal.
Explain how the common ion effect influences the solubility of a sparingly soluble salt in an acidic solution. Give a real world example where this effect is utilized.
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