Which Value for the First Dissociation Constant of Carbonic Acid Should Be Used in Biological Work?
The apparent first dissociation constant of carbonic acid has been defined in different ways in the literature. Harned and co-workers (8-10) have defined it in terms of molalities of the participating species, including H ions: Ks = mHmHCO3/mCO2. In contrast, Hastings and Sendroy have defined an app...
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ftwrightuniv:oai:corescholar.libraries.wright.edu:ncbp-1772 2023-05-15T15:52:30+02:00 Which Value for the First Dissociation Constant of Carbonic Acid Should Be Used in Biological Work? Putnam, Robert W. Roos, Albert 1991-05-01T07:00:00Z https://corescholar.libraries.wright.edu/ncbp/752 http://ajpcell.physiology.org/content/260/5/C1113.reprint unknown CORE Scholar https://corescholar.libraries.wright.edu/ncbp/752 http://ajpcell.physiology.org/content/260/5/C1113.reprint Neuroscience, Cell Biology & Physiology Faculty Publications Medical Cell Biology Medical Neurobiology Medical Physiology Medical Sciences Medicine and Health Sciences Neurosciences Physiological Processes text 1991 ftwrightuniv 2021-11-21T09:08:14Z The apparent first dissociation constant of carbonic acid has been defined in different ways in the literature. Harned and co-workers (8-10) have defined it in terms of molalities of the participating species, including H ions: Ks = mHmHCO3/mCO2. In contrast, Hastings and Sendroy have defined an apparent constant in which acidity is expressed as H ion activity: K'1 = aHmHCO3/mCO2. These constants differ by a factor γH, the activity coefficient of H ions at the prevailing ionic strength. Therefore, pK'1 is greater than pKs by an amount equal to -log γH, which, at µ = 0.16 M, is approximately 0.1. It is important that the correct value for the apparent dissociation constant or its logarithmic form be entered in the mass action expression or in the Henderson-Hasselbalch equation in order to prevent significant errors in the computation by means of these equations of quantities that cannot be directly measured. Specifically, for the derivation of bicarbonate concentration from PCO2 and pH (-log aH), pK'1 is to be used and not an uncorrected pKs. Text Carbonic acid Wright State University: CORE Scholar (Campus Online Repository) Hastings ENVELOPE(-154.167,-154.167,-85.567,-85.567) |
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Open Polar |
collection |
Wright State University: CORE Scholar (Campus Online Repository) |
op_collection_id |
ftwrightuniv |
language |
unknown |
topic |
Medical Cell Biology Medical Neurobiology Medical Physiology Medical Sciences Medicine and Health Sciences Neurosciences Physiological Processes |
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Medical Cell Biology Medical Neurobiology Medical Physiology Medical Sciences Medicine and Health Sciences Neurosciences Physiological Processes Putnam, Robert W. Roos, Albert Which Value for the First Dissociation Constant of Carbonic Acid Should Be Used in Biological Work? |
topic_facet |
Medical Cell Biology Medical Neurobiology Medical Physiology Medical Sciences Medicine and Health Sciences Neurosciences Physiological Processes |
description |
The apparent first dissociation constant of carbonic acid has been defined in different ways in the literature. Harned and co-workers (8-10) have defined it in terms of molalities of the participating species, including H ions: Ks = mHmHCO3/mCO2. In contrast, Hastings and Sendroy have defined an apparent constant in which acidity is expressed as H ion activity: K'1 = aHmHCO3/mCO2. These constants differ by a factor γH, the activity coefficient of H ions at the prevailing ionic strength. Therefore, pK'1 is greater than pKs by an amount equal to -log γH, which, at µ = 0.16 M, is approximately 0.1. It is important that the correct value for the apparent dissociation constant or its logarithmic form be entered in the mass action expression or in the Henderson-Hasselbalch equation in order to prevent significant errors in the computation by means of these equations of quantities that cannot be directly measured. Specifically, for the derivation of bicarbonate concentration from PCO2 and pH (-log aH), pK'1 is to be used and not an uncorrected pKs. |
format |
Text |
author |
Putnam, Robert W. Roos, Albert |
author_facet |
Putnam, Robert W. Roos, Albert |
author_sort |
Putnam, Robert W. |
title |
Which Value for the First Dissociation Constant of Carbonic Acid Should Be Used in Biological Work? |
title_short |
Which Value for the First Dissociation Constant of Carbonic Acid Should Be Used in Biological Work? |
title_full |
Which Value for the First Dissociation Constant of Carbonic Acid Should Be Used in Biological Work? |
title_fullStr |
Which Value for the First Dissociation Constant of Carbonic Acid Should Be Used in Biological Work? |
title_full_unstemmed |
Which Value for the First Dissociation Constant of Carbonic Acid Should Be Used in Biological Work? |
title_sort |
which value for the first dissociation constant of carbonic acid should be used in biological work? |
publisher |
CORE Scholar |
publishDate |
1991 |
url |
https://corescholar.libraries.wright.edu/ncbp/752 http://ajpcell.physiology.org/content/260/5/C1113.reprint |
long_lat |
ENVELOPE(-154.167,-154.167,-85.567,-85.567) |
geographic |
Hastings |
geographic_facet |
Hastings |
genre |
Carbonic acid |
genre_facet |
Carbonic acid |
op_source |
Neuroscience, Cell Biology & Physiology Faculty Publications |
op_relation |
https://corescholar.libraries.wright.edu/ncbp/752 http://ajpcell.physiology.org/content/260/5/C1113.reprint |
_version_ |
1766387667837124608 |