Henderson-Hasselbalch equation, plot

Henderson-Hasselbalch equation, plot [1.5.2.34, [3.6.52, 531, 3.88ff Heniy adsorption Isotherm see adsorption isotherm Henry constant. 

Figure 26.1 A titration curve for alanine, plotted using the Henderson-Hasselbalch equation. Each of the two legs is plotted separately. At pH < 1, alanine is entirely protonated at pH = 2.34, alanine is a 50 50 mix of protonated and neutral forms at pH 6.01, alanine is entirely neutral at pH = 9.69, alanine is a 50 50 mix of neutral and deprotonated forms at pH > 11.5, alanine is entirely deprotonated.

Figure 3.2(a) shows a plot of log S versus pH for naproxen, based on re-analysis (unpublished) of the shake-flask [49, 77] and microtiter plate [20] data reported in the literature. The dashed curves in Fig. 3.2 were calculated with the simple Henderson-Hasselbalch equations. For pH pKa, the function reduces to the horizontal line log S = log Sq. For pH pXi, log S is a straight line as a function of pH, exhibiting a slope of 1 (and an intercept of log So-pKj). Where the slope is 0.5, the pH equals to the pKj. 

Although Fig. 3.2 properly conveys the shapes of solubility-pH curves in saturated solutions of uncharged species, according to the Henderson-Hasselbalch equation, the indefinite ascendancy of the dashed curves in the plots can be misleading. When pH changes elevate the solubihty, at some value of pH, the solubihty product of the salt wiU be reached, causing the shape of the solubihty-pH curve to level off, as indicated in Fig. 3.2(a) for pH >8.38. 

HEMOGLOBINS POLYMERIZATION RESONANCE RAMAN SPECTROSCOPY HEMOGLOBIN-S POLYMERIZATION HENDERSON-HASSELBALCH EQUATION HENDERSON PLOT Henri-Brown treatment,... 

Figure I-I. Weak acids act as buffers in a pH range near their pK s. According to the Henderson-Hasselbalch equation, when the ratio of conjugate base to conjugate acid, [A ]/[HA] is plotted versus pH, a titration curve is generated that indicates a region of good buffering at pH = pK I pH unit.

This reaction shows that Eh is related to the standard potential ( ° - 0.77 V) and the proportionality of Fe3+ to Fe2+ in the solution phase. A number of J5° values representing various reactions in soils are given in Tables 5.2 and 5.3. Note that Equation 5.16 is analogous to the Henderson-Hasselbalch equation. A plot of Eh versus (Fe3+/Fe3+ + Fe2+) would produce a sigmoidal line with midpoint ° (Fig. 5.2) (recall that the Henderson-Hasselbalch equation gives the pKa at the titration midpoint see Chapter 1). To the left of ° (midpoint in the jc axis E° = 0.77 V) the reduced species (e.g., Fe2+) predominates, whereas to the right of ° (midpoint in the x axis), the oxidized species (e.g., Fe3+) predominates. 

Henderson-Hasselbalch equation lahn-Teller effect Lee-Yang-Parr method Lineweaver-Burk method Mark-Houwink plot Meerwein-Ponndorf theory Michaelis-Menten kinetics Stem-Volmer plot van t Hoff-Le Bel theory Wolff-Kishner theory Young-Laplace equation Ziegler-Natta-type catalyst... 

Henderson—Hasselbalch equation Jahn—Teller effect Lineweaver—Burk method Mark-Houwink plot Meerwein—Ponndorf theory Michaelis—Menten kinetics Stern—Volmer plot van t Hoff—Le Bel theory Wolff—Kishner theory Young—Laplace equation Ziegler—Natta-type catalyst... 

The slope and intercept from plots of pH versus log(a/l-a) were made from the modified Henderson-Hasselbalch equation . The n value, which is the slope of the line, is a measure of the average electrostatic repulsion between charges on the chain. 

The variables in the Henderson-Hasselbalch equation are [H ], [HCO3"] and [CO2]. Any pair of these can be used to plot graphs representing acid-base status for each pair, each member can be plotted linearly or logarithmically. This book has explored two methods of representing add-base status. In the earlier chapters, bicarbonate concentration was plotted as a function... 

From this equation, one can easily calculate the pffa by plotting k>g([A"]/[HA3) versus pH a straight line is obtained with an intercept on the ordinate equd to (Henderson, 1908 Hasselbalch, 1916). 

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