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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 55b
Capitolo 17, Problema 55b

If the volume of blood in a normal adult is 5.0 L, what mass of HCl can be neutralized by the buffering system in blood before the pH falls below 7.0 (which would result in death)?

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Identify the buffering system in blood, which is primarily the bicarbonate buffer system: \( \text{HCO}_3^- + \text{H}^+ \rightleftharpoons \text{H}_2\text{CO}_3 \).
Determine the concentration of bicarbonate ions (\( \text{HCO}_3^- \)) in blood, which is typically around 24 mM.
Calculate the total moles of \( \text{HCO}_3^- \) in 5.0 L of blood using the formula: \( \text{moles} = \text{concentration} \times \text{volume} \).
Use the stoichiometry of the reaction to find the moles of \( \text{HCl} \) that can be neutralized, noting that 1 mole of \( \text{HCO}_3^- \) neutralizes 1 mole of \( \text{HCl} \).
Convert the moles of \( \text{HCl} \) to mass using the molar mass of \( \text{HCl} \) (36.46 g/mol) with the formula: \( \text{mass} = \text{moles} \times \text{molar mass} \).

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Buffering System

A buffering system in biological fluids, such as blood, helps maintain a stable pH by neutralizing acids and bases. In blood, bicarbonate (HCO3-) and carbonic acid (H2CO3) are key components that resist changes in pH, allowing the body to function optimally despite metabolic processes that produce acids.
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Buffer Capacity

pH Scale

The pH scale measures the acidity or basicity of a solution, ranging from 0 (very acidic) to 14 (very basic), with 7 being neutral. In biological systems, a pH below 7.0 indicates acidosis, which can be life-threatening. Understanding how pH changes in response to acid addition is crucial for determining the buffering capacity of blood.
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The pH Scale

Neutralization Reaction

A neutralization reaction occurs when an acid reacts with a base to produce water and a salt, effectively reducing the acidity of the solution. In this context, the hydrochloric acid (HCl) introduced into the blood will react with the bicarbonate ions in the buffering system, and calculating the mass of HCl that can be neutralized involves stoichiometry and the concentrations of the reactants.
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Lewis Dot Structures: Neutral Compounds
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The fluids within cells are buffered by H2PO4- and HPO42- . b. Could a buffer system employing H3PO4 as the weak acid and H2PO4- as the weak base be used as a buffer system within cells? Explain.

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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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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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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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