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Ch.17 - Additional Aspects of Aqueous Equilibria
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Brown 14th EditionCh.17 - Additional Aspects of Aqueous Equilibria문제 29b
17장, 문제 29b

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

검증된 단계별 안내
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.

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주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

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.
추천 영상:
가이드 코스
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.
추천 영상:
가이드 코스
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.
추천 영상:
가이드 코스
02:40
Henderson-Hasselbalch Equation
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