(a) What is the ratio of HCO3 - to H 2 CO 3 in blood of pH 7.4?

Hey everyone. So here we have an ecstatic asset which is a weak acid. And it's going to associate. And to acetate ion and hydro any um ions and solution. The association constant Acetic acid is 1.78. I'm sent to negative five and it asks if we require a buffer of ph 5.25, what would be the ratio of the conjugate base to the weak asset that we would use? Okay Is 1.78 Times 10 to the - in the ph It's 5.25. And since we're dealing with but first we need to use our Henderson Hasselbach equation and this is going to be ph equals P. K. A. Plus the log of the concentration of the conjugate base divided by the concentration of the weak acid. So we're giving the K. And we need to find the P. K. A. So we're gonna use P. K. A. Equals negative law times K. Eight. So the P. K. A. He goes negative law Times 1.78 Times to the -5. And for P. K. A We're gonna get 4.75. So we're going to get 5.25 Equals 4. plus the law. And we can just call this X. So it's attract both sides by 4. And we're going to get 0.5 equals log of X. So to solve for X We're going to do 10. That is 0.5 power dot exe Which is going to be the concentration of the conjugate base divided by the concentration of the weak acid. It's gonna be 3.16. Thanks for watching my video and I hope it was helpful.

Ch.17 - Additional Aspects of Aqueous Equilibria

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Brown 15th Edition

Ch.17 - Additional Aspects of Aqueous Equilibria

Problem 29a

Chapter 17, Problem 29a

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

Verified step by step guidance

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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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

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.

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.

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.

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Related Practice

Textbook Question

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?

Textbook Question

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?

Open Question

A buffer contains 0.15 mol of propionic acid (C2H5COOH) and 0.10 mol of sodium propionate (C2H5COONa) in 1.20 L. (a) What is the pH of this buffer? (b) What is the pH of the buffer after the addition of 0.01 mol of NaOH? (c) What is the pH of the buffer after the addition of 0.01 mol of HI?

Textbook Question

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

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Textbook Question

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?

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?

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

Verified video answer for a similar problem:

Key Concepts

Buffer Systems

Henderson-Hasselbalch Equation

Physiological pH and Homeostasis

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