The beaker on the right contains 0.1 M acetic acid solution with methyl orange as an indicator. The beaker on the left contains a mixture of 0.1 M acetic acid and 0.1 M sodium acetate with methyl orange. (a) Using Figures 16.8 and 16.9, which solution has a higher pH?

검증된 단계별 안내

insert step 1> Identify the components of each solution. The right beaker contains only 0.1 M acetic acid, while the left beaker contains a mixture of 0.1 M acetic acid and 0.1 M sodium acetate.

insert step 2> Recognize that acetic acid (CH3COOH) is a weak acid, and sodium acetate (CH3COONa) is its conjugate base.

insert step 3> Understand that the mixture in the left beaker is a buffer solution, which resists changes in pH and typically has a higher pH than a solution of the weak acid alone.

insert step 4> Recall that the pH of a buffer solution can be estimated using the Henderson-Hasselbalch equation: \( \text{pH} = \text{pK}_a + \log \left( \frac{[\text{A}^-]}{[\text{HA}]} \right) \), where \([\text{A}^-]\) is the concentration of the conjugate base and \([\text{HA}]\) is the concentration of the acid.

insert step 5> Conclude that the left beaker, containing the buffer solution, will have a higher pH than the right beaker, which contains only the weak acid.

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주요 개념

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Acid-Base Chemistry

Acid-base chemistry involves the study of acids, bases, and their reactions. Acids are substances that donate protons (H+ ions), while bases accept protons. The strength of an acid or base is often measured by its dissociation in water, which affects the pH of the solution. Understanding the properties of weak acids like acetic acid and their conjugate bases is crucial for predicting pH changes in solutions.

Buffer Solutions

A buffer solution is a system that resists changes in pH upon the addition of small amounts of acid or base. It typically consists of a weak acid and its conjugate base, which can neutralize added acids or bases. In this case, the mixture of acetic acid and sodium acetate acts as a buffer, maintaining a relatively stable pH compared to the acetic acid solution alone, which is more susceptible to pH changes.

pH and Indicators

pH is a measure of the acidity or basicity of a solution, with lower values indicating higher acidity. Indicators like methyl orange change color at specific pH ranges, providing visual cues about the solution's acidity. Understanding how the pH of a solution affects the color change of an indicator is essential for interpreting the results of acid-base reactions and determining which solution has a higher pH.