Purchase Solution

bicarbonate-carbonic acid buffer system

Not what you're looking for?

Ask Custom Question

Preparing a Buffer. The pH of blood is 7.40. Calculate the [HCO3-] / [H2CO3] ratio of a bicarbonate-carbonic acid buffer system that will effectively maintain a sample of blood at a pH of 7.40. Hint: the Henderson-Hasselbalch equation is useful for this type of problem.

Purchase this Solution
Solution Summary

The solution shows how to prepare the bicarbonate-carbonic acid buffer system that will effectively maintain a sample of blood at a pH of 7.40.

Solution Preview

For this you need to use the BUFFER equation

Ka = [H+] x A-/HA

(which is ...

Purchase this Solution
Free BrainMass Quizzes
Organic Chemistry Naming: Alkanes

This is a quiz which is designed to assist students with learning the nomenclature used to identify organic compounds. This quiz focuses on the organic compounds called Alkanes.

Thermochemistry

The quiz helps in revising basic concepts about thermochemistry.

Functional groups in Organic Chemistry

You will be tested on the names of functional groups in Organic Chemistry. It is very important to know the functional groups to understand Organic reactions.

Periodic table

General Chemistry - Classification of Matter

This test will assess your knowledge on the classification of matter which includes elements, compounds and mixtures.

View More Free Quizzes
Related BrainMass Solutions

  • Chemical and Physiological Buffer Systems

    The bicarbonate system: carbonic acid and bicarbonate ions result with the hydration of CO2. They are weak buffers.

  • Acid-base Equilibrium and High Altitude Disease

    http://en.wikipedia.org/wiki/Bicarbonate Bicarbonate is an alkaline, and a vital component of the pH buffering system[1] of the body (maintaining acid-base homeostasis). 70%-75% of CO2 in the body is converted into carbonic acid (H2CO3), which can

  • prepare a liter of "carbonate buffer" at a pH of 10.10

    pKa = -log Ka So, calculate the pKa of carbonic acid and bicarbonate. pKa (carbonic acid) = -log 4.2x10^-7 = 6.38 pKa (bicarbonate) = -log 4.8x10^-11 = 10.32 This is great!

  • HCO3- as a Buffer

    The buffer system is one of the three compensatory mechanisms that the body uses to maintain a stable pH environment. The Bicarbonate Buffering System is the major system within the body.

  • Maintaining Fluid and Electrolyte Balance

    Chronically, the kidneys begin to adapt to secrete more carbonic acid into the urine while ensuring the blood buffer has enough materials to maintain a proper buffer by increasing reabsorption of the bicarbonate ion HCO3-, which has a role in maintaining

  • Compare the autonomic control of defecation and micturition

    The carbonic anhydrase reactions are important for regulating pH because the bicarbonate ion acts as a buffer.

  • Estimation of pH of solution based on color of 2 indicators

    Furthermore, bicarbonate is technically amphoteric, meaning it can accept or lose a proton, and therefore, acts as a buffer to limit pH changes. What kind of a system do acetic acid and sodium bicarbonate (NaHCO3) form?

  • Bicarbonate Blood Buffer and Competitive Inhibition in Drugs

    Reference: http://www.chemistry.wustl.edu/~edudev/LabTutorials/Buffer/Buffer.html A two part question about how the bicarbonate buffer system in blood works and how competitive inhibition in drugs can affect physiology.

  • Chemistry and Blood pH

    The carbonate buffer system is a key factor in controlling the pH. In this assignment you are to combine several key concepts in explaining this system.

View More Related Solutions