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Ch.18 - Aqueous Ionic Equilibrium
Tro - Chemistry: A Molecular Approach 5th Edition
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Tutti i libri di testoTro 5th EditionCh.18 - Aqueous Ionic EquilibriumProblema 53a
Capitolo 18, Problema 53a

Determine whether or not the mixing of each pair of solutions results in a buffer. a. 100.0 mL of 0.10 M NH3; 100.0 mL of 0.15 M NH4Cl

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1
Identify the components of a buffer solution: a weak base and its conjugate acid, or a weak acid and its conjugate base.
Recognize that NH_3 (ammonia) is a weak base and NH_4^+ (from NH_4Cl) is its conjugate acid.
Calculate the moles of NH_3: \( \text{moles of NH}_3 = 0.10 \text{ M} \times 0.100 \text{ L} \).
Calculate the moles of NH_4^+: \( \text{moles of NH}_4^+ = 0.15 \text{ M} \times 0.100 \text{ L} \).
Determine if both components (NH_3 and NH_4^+) are present in significant amounts to form a buffer.

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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 or a weak base and its conjugate acid. This equilibrium allows the buffer to neutralize added acids or bases, maintaining a relatively stable pH.
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Buffer Solutions

Weak Bases and Conjugate Acids

In the context of buffers, a weak base is a substance that partially ionizes in solution, establishing an equilibrium between the base and its conjugate acid. For example, ammonia (NH3) is a weak base, and when mixed with its conjugate acid, ammonium chloride (NH4Cl), it can form a buffer system that helps maintain pH stability.
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Conjugate Acid-Base Relationships

Henderson-Hasselbalch Equation

The Henderson-Hasselbalch equation is a mathematical formula used to calculate the pH of a buffer solution. It relates the pH to the concentration of the weak acid and its conjugate base, expressed as pH = pKa + log([A-]/[HA]). This equation is essential for determining whether a given mixture can function as a buffer.
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Henderson-Hasselbalch Equation
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