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Ch.17 - Aqueous Ionic Equilibrium
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoTro 4th EditionCh.17 - Aqueous Ionic EquilibriumProblema 54e
Capitolo 17, Problema 54e

Determine whether or not the mixing of each pair of solutions results in a buffer. e. 105.0 mL of 0.15 M CH3NH2; 95.0 mL of 0.10 M HCl

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Identify the components involved in the solution: CH₃NH₂ is a weak base and HCl is a strong acid.
Calculate the moles of CH₃NH₂ using the formula: moles = concentration (M) × volume (L).
Calculate the moles of HCl using the formula: moles = concentration (M) × volume (L).
Determine if the moles of HCl are less than, equal to, or greater than the moles of CH₃NH₂ to see if there is an excess of weak base or if the strong acid completely neutralizes the weak base.
Conclude whether a buffer is formed: A buffer is formed if there is a significant amount of weak base and its conjugate acid (formed from the reaction with the strong acid) present in the solution.

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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 Bases and Their Conjugate Acids

In this scenario, CH3NH2 (methylamine) is a weak base, and when it reacts with HCl (a strong acid), it forms its conjugate acid, CH3NH3+. The presence of both the weak base and its conjugate acid is essential for the formation of a buffer solution, allowing the system to neutralize added acids or bases.
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Conjugate Acid-Base Relationships

Stoichiometry of Acid-Base Reactions

Stoichiometry involves the calculation of reactants and products in chemical reactions. In this case, determining whether a buffer forms requires calculating the moles of CH3NH2 and HCl to see if they can coexist in a ratio that maintains the buffer capacity. Understanding the stoichiometric relationships helps predict the outcome of mixing these solutions.
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Acid-Base Reaction
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Domanda del libro di testo

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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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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