Skip to main content
Ch.17 - Additional Aspects of Aqueous Equilibria
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoBrown 14th EditionCh.17 - Additional Aspects of Aqueous EquilibriaProblema 29b
Capitolo 17, Problema 29b

(b) What is the ratio of HCO3- to H2CO3 in an exhausted marathon runner whose blood pH is 7.1?

Guida verificata passo dopo passo
1
Identify the relevant chemical species involved, which are bicarbonate ion (HCO3-) and carbonic acid (H2CO3).
Use the Henderson-Hasselbalch equation for the bicarbonate buffer system in blood: pH = pKa + log([HCO3-]/[H2CO3]).
Find the pKa value of carbonic acid, which is typically around 6.1 at body temperature.
Substitute the given pH value (7.1) and the pKa value into the Henderson-Hasselbalch equation.
Solve the equation for the ratio [HCO3-]/[H2CO3] by isolating this term and using basic algebraic operations.

Risposta video verificata per un problema simile:

Questa soluzione video è stata consigliata dai nostri tutor come utile per risolvere questo problema.
Durata del video:
2m

Concetti chiave

Ecco i concetti essenziali che devi comprendere per rispondere correttamente alla domanda.

Buffer Systems

Buffer systems in the body, particularly the bicarbonate buffer system, help maintain pH levels in the blood. This system involves a dynamic equilibrium between carbonic acid (H2CO3) and bicarbonate ions (HCO3-), which can absorb excess hydrogen ions (H+) or release them to stabilize pH. Understanding this balance is crucial for analyzing changes in blood pH, especially in physiological conditions like exhaustion.
Video consigliato:
Percorso guidato
00:45
Buffer Capacity

Acid-Base Balance

Acid-base balance refers to the mechanisms the body uses to maintain a stable pH in the blood and other fluids. The normal blood pH range is approximately 7.35 to 7.45, and deviations can indicate metabolic or respiratory issues. In the case of an exhausted marathon runner with a pH of 7.1, this indicates acidosis, which can result from increased lactic acid production and depletion of bicarbonate.
Video consigliato:
Percorso guidato
01:46
Balancing Acidic Redox Reactions

Henderson-Hasselbalch Equation

The Henderson-Hasselbalch equation relates the pH of a solution to the concentration ratio of an acid and its conjugate base. For the bicarbonate buffer system, it can be expressed as pH = pKa + log([HCO3-]/[H2CO3]). This equation is essential for calculating the ratio of bicarbonate to carbonic acid in the blood, allowing for a quantitative understanding of how the body compensates for changes in pH.
Video consigliato:
Percorso guidato
02:40
Henderson-Hasselbalch Equation
Pratica correlata
Domanda del libro di testo

You have to prepare a pH = 3.50 buffer, and you have the following 0.10 M solutions available: HCOOH, CH3COOH, H3PO4, HCOONa, CH3COONa, and NaH2PO4. How many milliliters of each solution would you use to make approximately 1 L of the buffer?

Domanda del libro di testo

A buffer contains 0.10 mol of acetic acid and 0.13 mol of sodium acetate in 1.00 L. (c) What is the pH of the buffer after the addition of 0.02 mol of HNO3?

585
views
Domanda del libro di testo

(a) What is the ratio of HCO3- to H2CO3 in blood of pH 7.4?

1960
views
Domanda del libro di testo

You have to prepare a pH = 3.50 buffer, and you have the following 0.10 M solutions available: HCOOH, CH3COOH, H3PO4, HCOONa, CH3COONa, and NaH2PO4. Which solutions would you use?

1852
views
1
rank
Domanda del libro di testo

You have to prepare a pH = 5.00 buffer, and you have the following 0.10 M solutions available: HCOOH, HCOONa, CH3COOH, CH3COONa, HCN, and NaCN. Which solutions would you use?

747
views