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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 59b
Capitolo 18, Problema 59b

A 500.0-mL buffer solution is 0.100 M in HNO2 and 0.150 M in KNO2. Determine if each addition would exceed the capacity of the buffer to neutralize it. b. 350 mg KOH

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Convert the mass of KOH to moles by using its molar mass. The molar mass of KOH is approximately 56.11 g/mol.
Calculate the moles of HNO_2 in the buffer solution using its concentration and volume. Use the formula: moles = concentration (M) × volume (L).
Calculate the moles of KNO_2 in the buffer solution using its concentration and volume. Use the formula: moles = concentration (M) × volume (L).
Determine the buffer capacity by comparing the moles of KOH to the moles of HNO_2 and KNO_2. A buffer can neutralize added acid or base as long as the moles of added substance do not exceed the moles of the buffer components.
Assess if the moles of KOH exceed the buffer capacity. If the moles of KOH are less than or equal to the moles of HNO_2 and KNO_2, the buffer can neutralize the addition. Otherwise, it exceeds the buffer capacity.

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Buffer Solutions

Buffer solutions are mixtures that resist changes in pH when small amounts of acid or base are added. They typically consist of a weak acid and its conjugate base or a weak base and its conjugate acid. In this case, HNO2 is the weak acid, and KNO2 provides the conjugate base, allowing the solution to maintain a stable pH despite the addition of KOH.
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Buffer Solutions

Buffer Capacity

Buffer capacity refers to the amount of acid or base that a buffer can neutralize before a significant change in pH occurs. It is influenced by the concentrations of the acid and base components in the buffer. The greater the concentrations, the higher the buffer capacity, meaning it can neutralize more added acid or base without exceeding its limits.
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Buffer Capacity

Stoichiometry of Neutralization Reactions

Stoichiometry involves the calculation of reactants and products in chemical reactions. In the context of buffer solutions, it is essential to determine how much of the buffer components will react with the added KOH. The neutralization reaction between KOH (a strong base) and HNO2 (a weak acid) will dictate whether the buffer can effectively neutralize the added base without exceeding its capacity.
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Stoichiometry Concept
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