Horseradish peroxidase. XXXII. pH dependence of the oxidation of L-(−)-tyrosine by compound I

1978 ◽  
Vol 56 (12) ◽  
pp. 1115-1119 ◽  
Author(s):  
I. Ralston ◽  
H. B. Dunford
Keyword(s):  
Horseradish Peroxidase ◽  
Ph Dependence ◽  
Nonlinear Least Squares ◽  
Compound I ◽  
Ph Profile ◽  
Rate Versus ◽  
Tyrosine Oxidation ◽  
Phenolic Group ◽  
Ph Range ◽  
Single Enzyme

The rate of oxidation of L-(−)-tyrosine by horseradish peroxidase compound I has been studied as a function of pH at 25 °C and ionic strength 0.11. Over the pH range of 3.20–11.23 major effects of three ionizations were observed. The pKa values of the phenolic (pKa = 10.10) and amino (pKa = 9.21) dissociations of tyrosine and a single enzyme ionization (pKa = 5.42) were determined from nonlinear least squares analysis of the log rate versus pH profile. It was noted that the less acidic form of the enzyme was most reactive; hence, the reaction is described as base catalyzed. The rate of tyrosine oxidation falls rapidly with the deprotonation of the phenolic group.

Horseradish peroxidase. XLII. Oxidations of L-tyrosine and 3,5-diiodo-L-tyrosine by compound II

1980 ◽  
Vol 58 (11) ◽  
pp. 1270-1276 ◽  
Author(s):  
Isobel M. Ralston ◽  
H. Brian Dunford
Keyword(s):  
Horseradish Peroxidase ◽  
Reaction Rate ◽  
Acid Group ◽  
Amino Groups ◽  
Compound I ◽  
Ph Profile ◽  
Rate Versus ◽  
Phenolic Group ◽  
Ph Range ◽  
Compound Ii

The oxidations of both L-tyrosine and 3,5-diiodo-L-tyrosine by compound II of horseradish peroxidase were studied over the pH range of approximately 3 to 10 at 25 °C and at a constant ionic strength of 0.11. The rate versus pH profile for the tyrosine – compound II reaction illustrates the influences of at least two acid group ionizations. An enzyme dissociation (pKa ~ 6.2) has a small effect on the reaction rate; whereas, a second pKa of 9.2, which may be attributed to either the enzyme or substrate, has a greater influence on the rate. The oxidation of tyrosine by compound II is fastest at pH 7.6. In the case of the diiodotyrosine – compound II reaction, three acid dissociations are necessary to describe the plot of log (kapp) versus pH. These include two enzyme pKa values of 3.6 and 8.6, and one substrate pKa of 6.6. The rate optimum for the reaction occurs at pH 5.2 and deprotonation of the phenolic group of diiodotyrosine results in a dramatic decrease in kapp. Diiodotyrosine is required in only a 0.5 M equivalent for the conversion of horseradish peroxidase compound I to compound II. The diiodotyrosine pKa values were estimated as 6.4 and 9.4 for the phenolic and amino groups, respectively.

Studies on Horseradish Peroxidase. XII. A Kinetic Study of the Oxidation of Sulfite and Nitrite by Compounds I and II

1973 ◽  
Vol 51 (4) ◽  
pp. 588-596 ◽  
Author(s):  
R. Roman ◽  
H. B. Dunford
Keyword(s):  
Horseradish Peroxidase ◽  
Ground State ◽  
Ph Dependence ◽  
Intermediate Formation ◽  
Ion Concentration ◽  
Compound I ◽  
Hydrogen Ion Concentration ◽  
Ph Range ◽  
Compound Ii ◽  
Kinetics Of

The kinetics of the oxidation of sulfite and nitrite by horseradish peroxidase compounds I and II have been studied as a function of pH at 25° and ionic strength 0.11. The pH dependence of the rate of the reaction between compound I and sulfite over the pH range 2–7 is interpreted in terms of two ground state enzyme dissociations with pka values of 5.1 and 3.3, and that for the compound II reaction with sulfite in terms of a single ground state enzyme dissociation with a pKa value of 3.9. Whereas the reaction between compound I and sulfite produces the native enzyme without the intermediate formation of compound II, the reaction of compound I with nitrite yields compound II. The second-order rate constants for the reactions of compounds I and II with nitrite increase linearly with increasing hydrogen ion concentration over the pH range 6–8.

Kinetics of the oxidation of reduced nicotinamide adenine dinucleotide by horseradish peroxidase compounds I and II

1986 ◽  
Vol 64 (4) ◽  
pp. 323-327 ◽  
Author(s):  
Mohammed A. Kashem ◽  
H. Brian Dunford
Keyword(s):  
Horseradish Peroxidase ◽  
Active Site ◽  
Nicotinamide Adenine Dinucleotide ◽  
Ph Dependence ◽  
Transient State ◽  
Nicotinamide Adenine ◽  
Compound I ◽  
Single Ionization ◽  
Reduced Nicotinamide Adenine Dinucleotide ◽  
Kinetics Of

The transient state kinetics of the oxidation of reduced nicotinamide adenine dinucleotide (NADH) by horseradish peroxidase compound I and II (HRP-I and HRP-II) was investigated as a function of pH at 25.0 °C in aqueous solutions of ionic strength 0.11 using both a stopped-flow apparatus and a conventional spectrophotometer. In agreement with studies using many other substrates, the pH dependence of the HRP-I–NADH reaction can be explained in terms of a single ionization of pKa = 4.7 ± 0.5 at the active site of HRP-I. Contrary to studies with other substrates, the pH dependence of the HRP-H–NADH reaction can be interpreted in terms of a single ionization with pKa of 4.2 ± 1.4 at the active site of HRP-II. An apparent reversibility of the HRP-II–NADH reaction was observed. Over the pH range of 4–10 the rate constant for the reaction of HRP-I with NADH varied from 2.6 × 105 to5.6 × 102 M−1 s−1 and of HRP-II with NADH varied from 4.4 × 104 to 4.1 M−1 s−1. These rate constants must be taken into consideration to explain quantitatively the oxidase reaction of horseradish peroxidase with NADH.

The mechanism of the nonenzymatic iodination of tyrosine by molecular iodine

1988 ◽  
Vol 66 (9) ◽  
pp. 967-978 ◽  
Author(s):  
H. Brian Dunford ◽  
Adejare J. Adeniran
Keyword(s):  
Ph Dependence ◽  
Acid Catalyst ◽  
Order Rate Constant ◽  
Molecular Iodine ◽  
Base Catalysis ◽  
Slow Step ◽  
Rate Law ◽  
General Acid ◽  
Phenolic Group ◽  
Ph Range

Over the pH range 7–10, at very low buffer concentration, the nonenzymatic iodination of tyrosine obeys the rate law[Formula: see text]where kapp is the measured second order rate constant based upon the total initial concentrations of molecular iodine and tyrosine and K2 (units M) is the equilibrium constant for [Formula: see text]. The value of k′ is 3.5 × 10−8 M∙s−1. There are three plausible mechanisms that fit the experimental data. One, the simplest, is a concerted process in which hypoiodous acid attacks tyrosine with its phenolic group unionized. The other two involve the formation of an iodinated quinoid reactive intermediate species in a rapid pre-equilibrium between unionized tyrosine and either hypoiodous acid or molecular iodine. The pre-equilibrium, if it occurs, favors the initial reactants. It is followed by a slow step in which the quinoid is converted to mono-iodinated tyrosine. Positive deviations from the rate law for pH dependence indicate that some specific acid catalysis (H3O+) is occurring in the pH range 5–7. In the presence of sufficient buffer, general acid–base catalysis is observed with acetic acid acting as a general acid catalyst in the vicinity of pH 5 and carbonate acting as a general base at pH ~ 9.5. The nonenzymatic iodination of tyrosine occurs more rapidly as the pH is increased, in marked contrast to the peroxidase-catalyzed iodination, which has its optimum at low pH.

Studies on Horseradish Peroxidase. VII. A Kinetic Study of the Oxidation of Iodide by Horseradish Peroxidase Compound II

1971 ◽  
Vol 49 (18) ◽  
pp. 3059-3063 ◽  
Author(s):  
R. Roman ◽  
H. B. Dunford ◽  
M. Evett
Keyword(s):  
Ionic Strength ◽  
Horseradish Peroxidase ◽  
Kinetic Study ◽  
Rate Constant ◽  
Ph Dependence ◽  
Order Rate Constant ◽  
Acid Dissociation ◽  
Ph Range ◽  
Compound Ii ◽  
Kinetics Of

The kinetics of the oxidation of iodide ion by horseradish peroxidase compound II have been studied as a function of pH at 25° and ionic strength of 0.11. The logarithm of the second-order rate constant decreases linearly from 2.3 × 105 to 0.1 M−1 s−1 with increasing pH over the pH range 2.7 to 9.0. The pH dependence of the reaction is explained in terms of an acid dissociation outside the pH range of the study.

Kinetics and mechanism of covalent addition of S(IV) species to the acridinium cation

1996 ◽  
Vol 74 (3) ◽  
pp. 365-370 ◽  
Author(s):  
Maria P. Ros ◽  
Jesus Thomas ◽  
Guillermo Crovetto ◽  
Juan Llor
Keyword(s):  
Rate Constants ◽  
Carbonyl Compounds ◽  
Nonlinear Least Squares ◽  
Kinetics And Mechanism ◽  
Experimental Conditions ◽  
Ph Profile ◽  
First Order ◽  
Constant Ph ◽  
Ph Range ◽  
Experimental Values

The reaction of acridine with S(IV) species (SO2•H2O, HSO3−, and SO32−) to form the adduct acridine–S(IV) has been studied spectrophotometrically throughout the pH range 2.6–8 in aqueous solutions. The observed pseudo-first-order rate constants, kobs, were determined at 25 °C and ionic strength I = 0.11 M, and the pH profile of the rate reached a maximum at pH ≈ 6.1. At constant pH the kobs values were a linear function of the total S(IV) concentration with slopes that increased significantly with pH. These data are consistent with the rate-determining attack of SO3H− and SO32− upon the C-9 of the acridinium cation. A nonlinear least-squares fitting of the experimental values to the model equation, within the overall pH region studied, yields the pH-independent rate constants k1 = 3.7 ± 0.1 and k2 = (6.24 ± 0.04) × 104 M−1 s−1 for the attack of these two species, respectively. The experimental results agree very well with the kinetic model. Due to the experimental conditions used we did not detect any possible pseudobase formation in the pH range studied. The reactivity of the S(IV) species with acridine follows the order: [Formula: see text] The value obtained for the ratio k1/k2 is similar to the results given for other addition reactions of S(IV) species to the double bond of carbonyl compounds such as benzaldehyde and formaldehyde. Key words: covalent addition, acridine, acridine – S(IV) adducts, kinetics and mechanism.

Studies on Horseradish Peroxidase. XI. On the Nature of Compounds I and II as Determined from the Kinetics of the Oxidation of Ferrocyanide

1973 ◽  
Vol 51 (4) ◽  
pp. 582-587 ◽  
Author(s):  
M. L. Cotton ◽  
H. B. Dunford
Keyword(s):  
Horseradish Peroxidase ◽  
Rate Constant ◽  
Active Sites ◽  
Ph Dependence ◽  
Order Rate Constant ◽  
Second Order ◽  
Compound I ◽  
Order Rate ◽  
Compound Ii ◽  
Kinetics Of

In order to investigate the nature of compounds I and II of horseradish peroxidase, the kinetics were studied of ferrocyanide oxidation catalyzed by these compounds which were prepared from three different oxidizing agents. The pH dependence of the apparent second-order rate constant for ferrocyanide oxidation by compound I, prepared from ethyl hydroperoxide and m-chloroperbenzoic acid, was interpreted in terms of an ionization on the enzyme with a pKa = 5.3, identical to that reported previously for hydrogen peroxide. The second-order rate constant for the compound II-ferrocyanide reaction also showed the same pH dependence for the three oxidizing substrates. However, with more accurate results, the compound II-ferrocyanide reaction was reinterpreted in terms of a single ionization with pKa = 8.5. The same dependence of ferrocyanide oxidation on pH suggests structurally identical active sites for compounds I and II prepared from the three different oxidizing substrates.

Kinetics of formation of the primary compound (compound I) from hydrogen peroxide and turnip peroxidases

1978 ◽  
Vol 56 (7) ◽  
pp. 702-707 ◽  
Author(s):  
Dominique Job ◽  
Jacques Ricard ◽  
H. Brian Dunford
Keyword(s):  
Hydrogen Peroxide ◽  
Compound I ◽  
Ph Profile ◽  
Glycerol Water ◽  
Binding Reaction ◽  
Cyanide Binding ◽  
Kinetics Of Formation ◽  
Ph Range ◽  
Kinetics Of ◽  
Ionizable Groups

A kinetic study of the reaction of two turnip peroxidases (P1 and P7) with hydrogen peroxide to form the primary oxidized compound (compound I) has been carried out over the pH range from 2,4 to 10.8. In the neutral and acidic pH regions, the rates depend linearly on hydrogen peroxide concentration whereas at alkaline pH values the rates display saturation kinetics. A comparison is made with the cyanide binding reaction to peroxidases since the two reactions are influenced in the same manner by ionization of groups on the native enzymes. Two different ionization processes of peroxidase P1 with pKa values of 3.9 and 10 are required to explain the rate pH profile for the reaction with H2O2. Protonation of the former group and ionization of the latter causes a decrease in the rate of reaction of the enzyme with H2O2. In the case of peroxidase P7 a minimum model involves three ionizable groups with pKa values of 2.5, 4, and 9. Protonation of the former two groups and ionization of the latter lowers the reaction rate. In the pH-independent region, the rate of formation of compound I was measured as a function of temperature. From the Arrhenius plots the activation energy for the reaction was calculated to be 2.9 ± 0.1 kcal/mol for P1 and 5.4 ± 0.3 kcal/mol for P7. However, the rates are independent of viscosity in glycerol–water mixtures up to 30% glycerol.

pH Dependence of the oxidation of iodide by compound I of horseradish peroxidase

Biochemistry ◽  
1972 ◽  
Vol 11 (11) ◽  
pp. 2076-2082 ◽  
Author(s):  
R. Roman ◽  
H. B. Dunford
Keyword(s):  
Horseradish Peroxidase ◽  
Ph Dependence ◽  
Compound I

scholarly journals Iodide modulation of the EDTA-induced iodine reductase activity of horseradish peroxidase by interaction at or near the EDTA-binding site

1993 ◽  
Vol 289 (2) ◽  
pp. 575-580 ◽  
Author(s):  
D K Bhattacharyya ◽  
U Bandyopadhyay ◽  
R Chatterjee ◽  
R K Banerjee
Keyword(s):  
Horseradish Peroxidase ◽  
Binding Site ◽  
Reductase Activity ◽  
Electron Flow ◽  
Ph Dependence ◽  
Compound I ◽  
Native Form ◽  
Iodide Oxidation ◽  
Equilibrium Dissociation ◽  
Haem Iron

Horseradish peroxidase (HRP) catalyses the reduction of iodinium ion (I+) to iodide by H2O2 in the presence of EDTA. I+ reduction occurs optimally at pH 6 whereas the enzyme catalyses iodide oxidation optimally at pH 3.5. Thus the two activities reside on the same enzyme with two characteristic pH optima. Iodide modulates the expression of the reductase activity by EDTA. Higher concentrations of iodide inhibit the reductase activity by EDTA. Nitrite, an electron donor, acts similarly to iodide. Both EDTA and nitrite competitively inhibit iodide oxidation, indicating that they compete with iodide for the same binding site for electron flow to the haem iron group. However, unlike iodide, EDTA converts compound I, not into the native enzyme, but into a compound absorbing at 416 nm which reduces I+ and then returns to the native form. The apparent equilibrium dissociation constant, KD, for the formation of the EDTA-HRP complex (15 mM) is doubled in the presence of iodide, indicating interference with EDTA binding by iodide. EDTA binds away from the haem iron centre and not through intramolecular Ca2+. The pH-dependence of EDTA binding indicates that an ionizable group of the enzyme with pKa 5.8, presumably a distal histidine, controls the binding. The data suggest that iodide competes with EDTA for compound I and modulates the iodine reductase activity by limiting the formation of the 416 nm-absorbing active compound.

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