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Ch.18 - Aqueous Ionic Equilibrium
Tro - Chemistry: A Molecular Approach 5th Edition
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoTro 5th EditionCh.18 - Aqueous Ionic EquilibriumProblema 54b
Capitolo 18, Problema 54b

Determine whether or not the mixing of each pair of solutions results in a buffer. a. 75.0 mL of 0.10 M HF; 55.0 mL of 0.15 M NaF b. 150.0 mL of 0.10 M HF; 135.0 mL of 0.175 M HCl d. 125.0 mL of 0.15 M CH3NH2; 120.0 mL of 0.25 M CH3NH3Cl

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1
Identify the components needed for a buffer solution: a weak acid and its conjugate base, or a weak base and its conjugate acid.
Recognize that HF is a weak acid, which is a potential component of a buffer solution.
Note that HCl is a strong acid, which will completely dissociate in solution and does not form a buffer with HF.
Calculate the moles of HF: \( \text{moles of HF} = 0.150 \text{ L} \times 0.10 \text{ M} \).
Calculate the moles of HCl: \( \text{moles of HCl} = 0.135 \text{ L} \times 0.175 \text{ M} \).

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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. Buffers are crucial in maintaining stable pH levels in various chemical and biological processes.
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Buffer Solutions

Weak Acids and Strong Acids

Weak acids, like HF (hydrofluoric acid), partially dissociate in solution, establishing an equilibrium between the undissociated acid and its ions. In contrast, strong acids, such as HCl (hydrochloric acid), completely dissociate in solution. The presence of a strong acid can disrupt the equilibrium of a weak acid, affecting the buffer capacity.
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Calculating Percent Ionization of Weak Acids

pH and Acid-Base Reactions

pH is a measure of the hydrogen ion concentration in a solution, indicating its acidity or basicity. Acid-base reactions involve the transfer of protons (H+) between species, influencing the pH. Understanding how the mixing of different acids affects the overall pH is essential for determining whether a buffer is formed.
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pH of Strong Acids and Bases
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Determine whether or not the mixing of each pair of solutions results in a buffer. d. 175.0 mL of 0.10 M NH3; 150.0 mL of 0.12 M NaOH

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Blood is buffered by carbonic acid and the bicarbonate ion. Normal blood plasma is 0.024 M in HCO3- and 0.0012 M H2CO3 (pKa1 for H2CO3 at body temperature is 6.1).

c. Given the volume from part (b), what mass of NaOH can be neutralized before the pH rises above 7.8?

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Determine whether or not the mixing of each pair of solutions results in a buffer. c. 165.0 mL of 0.10 M HF; 135.0 mL of 0.050 M KOH

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Blood is buffered by carbonic acid and the bicarbonate ion. Normal blood plasma is 0.024 M in HCO3- and 0.0012 M H2CO3 (pKa1 for H2CO3 at body temperature is 6.1).

a. What is the pH of blood plasma?

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Determine whether or not the mixing of each pair of solutions results in a buffer. e. 125.0 mL of 0.15 M NH3; 150.0 mL of 0.20 M NaOH

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Determine whether or not the mixing of each pair of solutions results in a buffer. c. 50.0 mL of 0.15 M HF; 20.0 mL of 0.15 M NaOH

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