Apparent dissociation constant

Dissociation Constant Apparent Partition Coefficient Transport Rate Constant (min" )... 

The situation is more interesting when the solution is buffered with a weak acid, say HA. Then, if = (H )[A ]/[HA] is the apparent acid dissociation constant, we have... 

Suppose now that the pH is controlled by a weak base buffer, the equilibrium being written BH B + H, where B signifies a neutral base. The apparent dissociation constant is = (H )[B]/[BH ]. Following the earlier argument, we obtain... 

This equation states that the ratio of oxygenated, heme groups (F) to 02-free heme (1 F) is equal to the nth power of the PO2 divided by the apparent dissociation constant, K. 

In the range pH 8-10 both sets of equilibria are important. The apparent dissociation constant of carbonic acid is... 

Apparent partition coefficient (logZ)) at an ionic strength of / = 0.02M, log P value of the neutral microspecies and the acidic dissociation constant of 5 was calculated (97ANC4143). The distribution coefficient of 5 was determined between 1-octanol and universal buffer in the pH range 3-10 at a... 

The ICS0 is used in a version of the Cheng-Prusoff equation for functional assays. Thus, the apparent Kb (apparent equilibrium dissociation constant for the antagonist-receptor complex) is given by... 

The factor at can be calculated from the known dissociation constants of EDTA, and since the proportions of the various ionic species derived from EDTA will be dependent upon the pH of the solution, a will also vary with pH a plot of log a against pH shows a variation of logoc = 18 at pH = 1 to loga = 0 at pH = 12 such a curve is very useful for dealing with calculations of apparent stability constants. Thus, for example, from Table 2.4, log K of the EDTA complex of the Pb2+ ion is 18.0 and from a graph of log a against pH, it is found that at a pH of 5.0, log a = 7. Hence from equation (30), at a pH of 5.0 the lead-EDTA complex has an apparent stability constant given by ... 

This potential reflects itself in the titration curves of weak polyacids such as poly(acrylic acid) and poly(methacrylic acid) [32]. Apparent dissociation constants of such polyacids change with the dissociation degree of the polyacid because the work to remove a proton from the acid site into the bulk water phase depends on the surface potential of the polyelectrolyte. 

Mehrbach, C., Culberson, C. H., Hawley, S. E. and Pytkowicz, R. M. (1973). Measurement of the apparent dissociation constants of carbonic acid in seawater at atmospheric pressure. Limnol. Oceanog. 18,6,897-907. 

Inhibition of EGF binding by palytoxin could be due to a decrease in receptor affinity, as in the case of TPA-type tumor promoters, and/or a decrease in receptor number. In Swiss 3T3 cells there are two classes of EGF receptors. The dissociation constants for the two EGF receptor classes were determined to be approximately 2 X 10 M and 2 x 10" M, corresponding to approximately 1 x 10 and 1 X 10 receptor molecules per cell, respectively (33). Scatchard analysis revealed that treatment of Swiss 3T3 cells with palytoxin, like PDBu, caused an apparent loss in high-affinity binding (Figure 2). However, in contrast to PDBu, palytoxin also caused a significant (approximately 50%) loss of low affinity EGF binding. 

In vitro binding studies use different cell lines or membrane preparations and generally only yield the apparent dissociation constants for a number of antagonists obtained by comparative displacement of one labelled ligand. Unfortunately few... 

Extensive data are given in the Uterature for the potentiometric titration of polymer acids which may be used to study the behaviour of polyelectrolyte systems under different conditions. For poly(a-D) galacturonic acid there are few data of this kind, especially in connection with the occurrence of a conformational transition induced by pH variations, or with the effect brought about by the addition or the exchange of counterions. Since for a polyacid not exhibiting a conformational transition in the course of titration, pK K denoting the apparent dissociation constant) increases monotonously with degree... 

Fig.l. Change of the apparent dissociation constant with a for the system PGA + (C Hg) NOH at 298 K. The curve was calculated from the model given by Mandel. 

The apparent dissociation constant pK is strongly dependent on the electrical potential on the surface of the macroion, according to the well known equation [11]... 

Figure 3.9 Apparent value of the dissociation constant (K,) for a labeled inhibitor, I, as a function of the concentration of a second inhibitor, J when measured by equilibrium binding methods. The solid circles represent the behavior expected when compounds I and J bind in a mutually exclusive fashion with one another. The other symbols represent the behavior expected when compounds I and J bind in a nonexclusive, but antagonistic (i.e., noncompetitive, a > 1) fashion, to separate binding sites. The data for mutually exclusive binding were fit to the equation (apparent)K, = A, 1 + ([f ] A",) I and that for nonexclusive binding were fit to the equation (apparent)Kt = ( [J] + Kj / Kj + f[I]/y) ) for y values of 5 (closed triangles), 10 (open squares), 20 (closed squares), and 50 (open circles).

In this chapter we described the thermodynamics of enzyme-inhibitor interactions and defined three potential modes of reversible binding of inhibitors to enzyme molecules. Competitive inhibitors bind to the free enzyme form in direct competition with substrate molecules. Noncompetitive inhibitors bind to both the free enzyme and to the ES complex or subsequent enzyme forms that are populated during catalysis. Uncompetitive inhibitors bind exclusively to the ES complex or to subsequent enzyme forms. We saw that one can distinguish among these inhibition modes by their effects on the apparent values of the steady state kinetic parameters Umax, Km, and VmdX/KM. We further saw that for bisubstrate reactions, the inhibition modality depends on the reaction mechanism used by the enzyme. Finally, we described how one may use the dissociation constant for inhibition (Kh o.K or both) to best evaluate the relative affinity of different inhibitors for ones target enzyme, and thus drive compound optimization through medicinal chemistry efforts. 

Woolley, E. M. Hepler, L. G., Apparent ionization constants of water in aqueous organic mixtures and acid dissociation constants of protonated co-solvents in aqueous solution, Anal. Chem. 44, 1520-1523 (1972). 

Fig. 1.2 Dependence of the dissociation degree a of a week electrolyte on molar concentration c for different values of the apparent dissociation constant K (indicated at each curve)... 

The excess electrolyte is often termed the indifferent electrolyte. From the practical point of view, solutions containing an indifferent electrolyte are very often used in miscellaneous investigations. For example, when determining equilibrium constants (e.g. apparent dissociation constants, Eq. 1.1.26) it is necessary only to indicate the indifferent electrolyte and its concentration, as they do not change when the concentrations of the reactants are changed. Moreover, the indifferent electrolyte is important in the study of diffusion transport (Section 2.5), for elimination of liquid... 

Most acid dissociation constants pKa exceed environmental pH values, the exceptions being the highly chlorinated phenols. As a result, these substances tend to have higher apparent solubilities in water because of dissociation. The structure-property relationships apply to the un-ionized or protonated species thus, experimental data should preferably be corrected to eliminate the effect of ionization, thus eliminating pH effects. 

For a binding reaction we can pick whether we show the reaction as favorable or unfavorable by picking the substrate concentration we use. Association constants have concentration units (M-1)- The equilibrium position of the reaction (how much ES is present) depends on what concentration we pick for the substrate. At a concentration of the substrate that is much less than the dissociation constant for the interaction, most of the enzyme will not have substrate bound, the ratio[ES]/[E] will be small, and the apparent equilibrium constant will also be small. This all means that at a substrate concentration much less than the dissociation constant, the binding of substrate is unfavorable. At substrate concentrations higher than the dissociation constant, most of the enzyme will have substrate bound and the reaction will be shown as favorable (downhill). (See also the discussion of saturation behavior in Chap. 8.)... 

---