Re-evaluation of the First and Second Stoichiometric Dissociation Constants of Phthalic Acid at Temperatures from (0 to 60) °C in Aqueous Phthalate Buffer Solutions with or without Potassium Chloride. 2. Estimation of Parameters for the Model for the First Dissociation Constant and Tests and Use of the Resulting Activity Coefficient Equations

2006 ◽  
Vol 51 (6) ◽  
pp. 2065-2073 ◽  
Author(s):  
Jaakko I. Partanen ◽  
Arthur K. Covington
Keyword(s):  
Activity Coefficient ◽  
Potassium Chloride ◽  
Dissociation Constant ◽  
Phthalic Acid ◽  
Dissociation Constants ◽  
Estimation Of Parameters ◽  
Buffer Solutions

Determination of Stoichiometric Dissociation Constants of Glycolic Acid in Dilute Aqueous Sodium or Potassium Chloride Solutions at 298.15 K

2001 ◽  
Vol 215 (4) ◽  
Author(s):  
Jaakko I. Partanen ◽  
P.M. Juusola ◽  
P.O. Minkkinen
Keyword(s):  
Potassium Chloride ◽  
Dissociation Constant ◽  
Glycolic Acid ◽  
Dissociation Constants ◽  
Chloride Solutions ◽  
Aqueous Sodium

Equations were determined for the calculation of the stoichiometric (molality scale) dissociation constant, K

Acids, bases and buffer solutions

2018 ◽  
Author(s):  
Dennis Sherwood ◽  
Paul Dalby
Keyword(s):  
First Principles ◽  
Buffer Capacity ◽  
Unique Feature ◽  
Dissociation Constants ◽  
Equilibrium Composition ◽  
Buffer Solutions ◽  
Acid And Base ◽  
Water Ph ◽  
Acids And Bases ◽  
Conjugate Bases

Many reactions in solution involve acids and bases, and so this chapter examines these important reactions in detail. Topics covered include the ionisation of water, pH, pOH, acids and bases, conjugate acids and conjugate bases, acid and base dissociation constants, the Henderson-Hasselbalch equation, the Henderson-Hasselbalch approximation, buffer solutions and buffer capacity. A unique feature of this chapter is a ‘first principles’ analysis of how a reaction buffered at a particular pH achieves an equilibrium composition different from that of the same reaction taking place in an unbuffered solution. This introduces some concepts which are important in understanding the biochemical standard state, as required for Chapter 23.

Second dissociation constant of 3-(N-morpholino)-2-hydroxypropanesulfonic acid and pH of its buffer solutions

1993 ◽  
Vol 65 (8) ◽  
pp. 1084-1087 ◽  
Author(s):  
Y. C. Wu ◽  
P. A. Berezansky ◽  
Daming. Feng ◽  
W. F. Koch
Keyword(s):  
Dissociation Constant ◽  
Buffer Solutions ◽  
Second Dissociation Constant

Which value for the first dissociation constant of carbonic acid should be used in biological work?

1991 ◽  
Vol 260 (5) ◽  
pp. C1113-C1116 ◽  
Author(s):  
R. W. Putnam ◽  
A. Roos
Keyword(s):  
Ionic Strength ◽  
Activity Coefficient ◽  
Dissociation Constant ◽  
Carbonic Acid ◽  
Mass Action ◽  
Bicarbonate Concentration ◽  
Apparent Dissociation Constant ◽  
Logarithmic Form ◽  
Ion Activity ◽  
Hasselbalch Equation

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 gamma H, the activity coefficient of H ions at the prevailing ionic strength. Therefore, pK'1 is greater than pKs by an amount equal to -log gamma H, which, at mu = 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.

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