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Ch.17 - Additional Aspects of Aqueous Equilibria
Brown - Chemistry: The Central Science 15th Edition
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Brown 15th EditionCh.17 - Additional Aspects of Aqueous Equilibria문제 29a
17장, 문제 29a

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

검증된 단계별 안내
1
Identify the relevant chemical species involved, which are bicarbonate ion (HCO3-) and carbonic acid (H2CO3).
Recognize that the relationship between these species in solution can be described by the Henderson-Hasselbalch equation: pH = pKa + log([A-]/[HA]), where A- is the conjugate base (HCO3-) and HA is the acid (H2CO3).
Find the pKa value for the dissociation of H2CO3 into HCO3-. This value is typically around 6.1 for carbonic acid.
Substitute the known values into the Henderson-Hasselbalch equation: 7.4 = 6.1 + log([HCO3-]/[H2CO3]).
Solve the equation for the ratio [HCO3-]/[H2CO3] by isolating the ratio on one side of the equation.

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주요 개념

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

Buffer Systems

Buffer systems in biological fluids, such as blood, help maintain pH stability. The bicarbonate (HCO3-) and carbonic acid (H2CO3) system is a crucial buffer that resists changes in pH by neutralizing excess acids or bases. This balance is vital for physiological processes, as even slight deviations in pH can affect enzyme activity and metabolic functions.
추천 영상:
가이드 코스
00:45
Buffer Capacity

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 is expressed as pH = pKa + log([HCO3-]/[H2CO3]). This equation allows for the calculation of the ratio of bicarbonate to carbonic acid at a given pH, which is essential for understanding acid-base balance in the blood.
추천 영상:
가이드 코스
02:40
Henderson-Hasselbalch Equation

Physiological pH and Homeostasis

Physiological pH refers to the normal pH range of human blood, which is approximately 7.35 to 7.45. Maintaining this pH is crucial for homeostasis, as it ensures optimal conditions for biochemical reactions. Deviations from this range can lead to acidosis or alkalosis, conditions that can disrupt cellular functions and overall health.
추천 영상:
가이드 코스
02:33
The pH Scale
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교과서 질문

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?

교과서 질문

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

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교과서 질문

A buffer contains 0.10 mol of acetic acid and 0.13 mol of sodium acetate in 1.00 L. b. What is the pH of the buffer after the addition of 0.020 mol of KOH?

교과서 질문

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 0.020 mol of HNO3?

교과서 질문

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?

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