Kinetics and mechanism of the alkaline hydrolysis of maleimide

The kinetics of hydrolysis of maleimide was carried out within the [OH-] range of 2.46 X 10(-6) to 2.0 M at 30 degrees C. The observed pseudo-first-order rate constants, kobs, follow the empirical equation: kobs = (A1[OH-] + A2[OH-]2)/(1 + A3[OH-]). Both ionized and un-ionized forms of maleimide have been suggested to be involved in hydrolysis. The nucleophilic attacks by hydroxide ion at the carbonyl carbon of both ionized and un-ionized maleimide and by water at the carbonyl carbon of ionized maleimide to form tetrahedral intermediates are considered to be the rate-determining steps. The observed results obtained at different 1,4-dioxane-water compositions have revealed an increase in kobs with a decrease in 1,4-dioxane content which could be attributed to the higher polarity of the transition state compared with the reactant state.     

Degradation kinetics of phentolamine hydrochloride in solution

The degradation kinetics of phentolamine hydrochloride in aqueous solution over a pH range of 1.2 to 7.2 and its stability in propylene glycol- or polyethylene glycol 400-based solutions were investigated. The observed rate constants were shown to follow apparent first-order kinetics in all cases. The pKa determination for phentolamine hydrochloride was found to be 9.55 +/- 0.10 (n = 5) at 25 +/- 0.2 degrees C. This indicated the protonated form of phentolamine occurs in the pH range of this study. The pH-rate profile indicated a pH-independent region (pH 3.1-4.9) exists with a minimum rate around pH 2.1. The catalytic effect of acetate and phosphate buffer species is ordinary. The catalytic rate constants imposed by acetic acid, acetate ion, dihydrogen phosphate ion, and monohydrogen phosphate ion were determined to be 0.018, 0.362, 0.036, and 1.470 L mol-1 h-1, respectively. The salt effect in acetate and phosphate buffers followed the modified Debye-Huckel equation quite well. The ZAZB value obtained from the experiment closely predicts the charges of the reacting species. The apparent energy of activation was determined to be 19.72 kcal/mol for degradation of phentolamine hydrochloride in pH 3.1, 0.1 M acetate buffer solution at constant ionic strength (mu = 0.5). Irradiation with 254 nm UV light at 25 +/- 0.2 degrees C showed a ninefold increase in the degradation rate compared with the light-protected control. Propylene glycol had little or no effect on the degradation of phentolamine hydrochloride at 90 +/- 0.2 degrees C; however, polyethylene glycol 400 had a definite effect.     

Effect of pH on in vitro permeation of ondansetron hydrochloride across porcine buccal mucosa

The influence of drug concentration, pH in donor chamber, and 1-octanol/buffer partition coefficient on transbuccal permeation of ondansetron hydrochloride (pKa, 7.4) across porcine buccal mucosa was studied by using an in-line Franz type diffusion cell at 37 degrees C. The pH was adjusted to several values and the solubility of the drug in different pH was measured. Solubility of ondansetron hydrochloride decreases with increasing pH. The permeability of the drug was evaluated at different donor pH and drug concentrations. Permeability of un-ionized (Pu) and ionized (Pi) species of drug was calculated by fitting the data to a mathematical model. The steady state flux increased linearly with the donor concentration (r2 = 0.9843) at pH 7.4. The permeability coefficient and the partition coefficient of the drug increased with increasing pH. The values of Pu and Pi were 4.86 x 10(-6) cm/sec and 7.18 x 10(-7) (c)m/sec, respectively. The observed permeability coefficients and the permeability coefficients calculated from the mathematical model at various pH showed good linearity (r2 = 0.9799). The total permeability coefficient increased with increasing the fraction of un-ionized form of the drug. The drug permeated through buccal mucosa by a passive diffusion process. The non-ionized species of drug penetrated well through buccal mucosa and the permeation was a function of pH. Transbuccal delivery is a potential route for the administration of ondansetron hydrochloride.     

Isoxazoles. VII: Hydrolysis of 4-methyl-5-isoxazolylnaphthoquinone derivatives in aqueous solutions

The kinetics for the degradation of 2-(4-methyl-5-isoxazolylamine)-N-(4-methyl-5-isoxazolyl)-1,4 -naphthoquinone-4- imine (1) in solution were investigated at 70 degrees C and at a constant ionic strength of 0.5 over a pH range of 1.75 to 12.85. The degradation rates were determined by absorption and second-derivative UV spectrometry. Two degradation products were identified in acidic and neutral pHs; they are 4-N-(4-methyl-5-isoxazolyl)-1,2-naphthoquinone (2) and 2-methyl-cyanoacetamide (5), respectively. In alkaline pH, two degradation products, 2-hydroxy-N-(4-methyl-5-isoxazolyl)-1,4-naphthoquinone-4-imine (3) and 5-amino-4-methylisoxazole (4), were isolated. The pathway for degradation of 1 in acidic and neutral pH followed consecutive first-order kinetics since 2 undergoes hydrolysis giving 2-hydroxy-1,4-napthoquinone (6) and 2-methylcyanoacetamide (5). No appreciable buffer effect on the degradation of 1 and 2 was observed for any of the buffer species in this study. The pH-rate profiles exhibited specific acid and specific basic catalysis for 1 and specific acid catalysis for 2. The maximum stability for 1 and 2 occurred in the neutral pH region.     

Degradation kinetics of butylmethoxydibenzoylmethane (avobenzone) in aqueous solution

The degradation kinetics of avobenzone in aqueous solution was studied at 60 +/- 0.2 degrees C over a pH range of 2.0-10.0. The degradation rates were determined by high performance liquid chromatography. The reaction is found to follow first-order kinetics and the rate constant for the decomposition at 25 degrees C is estimated by extrapolation. The breakdown of avobenzone is shown to be hydroxide ion catalyzed and the Arrhenius plots showed the temperature dependence of avobenzone degradation.     

Abiotic transformations and decomposition kinetics of 4-carbamoyl-2'-[(hydroxyimino)methyl]-1,1'-(oxydimethylene)-bis(pyridin ium chloride) in aqueous phosphate buffers

The rate of disappearance of 4-carbamoyl-2'-[(hydroxyimino)methyl]-1,1'-(oxydimethylene) bis (pyridinium chloride) (HI-6) from aqueous phosphate buffers (pH 3.0-9.1) was both pH and temperature sensitive. In midrange buffers (pH 6.0-9.1, mu = 0.2 M) at 37, 25, or 4 degrees C the decomposition followed first-order kinetics consistent with hydroxide-promoted decomposition of the un-ionized drug or with hydrolysis of the ionized oxime anion to result in 4-carbamoyl-2'-hydroxy-1,1'-(oxydimethylene)bis(pyridinium) cation (intermediate 1). The subsequent conversion of intermediate 1 to 4-carboxy-2'-hydroxy-1,1'-(oxydimethylene)bis(pyridinium) cation (intermediate 2) followed higher order kinetics which were consistent with either acid- or base-promoted hydrolysis of the B-ring amide functionality. After approximately 138 days in the dark, the sum of the residual HI-6, intermediate 1, and intermediate 2 in the crude decomposition mixture accounted for 89.9 +/- 10.0% of the initial substrate. Minor byproducts included 4-carbamoyl-2'-carboxy-1,1'-(oxydimethylene)bis(pyridinium) cation, 2-pyridinealdoxime, 2-pyridinecarboxaldehyde, 2-hydroxypyridine, isonicotinamide, isonicotinic acid, and traces of cyanide. In addition, 2-cyanopyridine appeared to be a transient intermediate in more alkaline media. In total, this drug resembles other mono- and bis(pyridinium) aldoximes in terms of the decomposition routes in aqueous solutions at intermediate pHs.     

Nefopam hydrochloride degradation kinetics in solution

A stability-indicating reversed-phase high performance liquid chromatographic method was developed for the detection of nefopam hydrochloride and its degradation products under accelerated degradation conditions. The degradation kinetics of nefopam hydrochloride in aqueous solutions over a pH range of 1.18 to 9.94 at 90 +/- 0.2 degrees C was studied. The degradation of nefopam hydrochloride was found to follow apparent first-order kinetics. The pH-rate profile shows that maximum stability of nefopam hydrochloride was obtained at pH 5.2-5.4. No general acid or base catalysis from acetate, phosphate, or borate buffer species was observed. The catalytic rate constants on the protonated nefopam imposed by hydrogen ion and water was determined to be 7.16 X 10(-6) M-1 sec-1, and 4.54 X 10(-9) sec-1, respectively. The pKa of nefopam hydrochloride in aqueous solution was determined to be 8.98 +/- 0.33 (n = 3) at 25 +/- 0.2 degrees C by the spectrophotometric method. The catalytic rate constant of hydroxyl ion on the degradation of nefopam in either protonated or nonprotonated form was determined to be 6.63 X 10(-6) M-1 sec-1 and 4.06 X 10(-6) M-1 sec-1, respectively. A smaller effect of hydroxyl ion on the degradation of nonprotonated than on the degradation of protonated nefopam was observed.(ABSTRACT TRUNCATED AT 250 WORDS)     

Solubilization of ionized and un-ionized flavopiridol by ethanol and polysorbate 20

Because the ionized species is more polar than its un-ionized counterpart, it is often assumed that the ionized species of the drug does not make a meaningful contribution to solubilization by either cosolvents or surfactants. This report extends previous studies on solubilization of the ionic species by a combination of pH control and complexation to pH control and micellization and to pH control and cosolvency. The total aqueous solubility is expressed as the addition of the concentration of all contributing species: free un-ionized drug [Du], free ionized drug [Di], un-ionized drug micelle [DuM], and ionized drug micelle [DiM] for surfactant, and free un-ionized drug [Dcu] and free ionized drug [Dci] for cosolvent. The equations indicate that under certain conditions the ionized species can be more important in determining the drug total solubility than the un-ionized species. Flavopiridol, a weak base, is used to test these newly generated equations. As expected, the micellar partition coefficient and solubilization power for ionized flavopiridol are both less than those of the un-ionized species. However, at acidic pH, the solubilities of the ionized drug in surfactant micelles [DiM] and in cosolvent-water [Dci] are both much greater than that of the un-ionized drug. This difference is because the solubilization of the ionized drug is proportional to its aqueous solubility, and its solubility [Di] can be as much as 24-fold greater than that of the free un-ionized species [Du].     

2-(3,4-Dichlorophenyl)-N-methyl-N-[2-(1-pyrrolidinyl)-1-substituted- ethyl]-acetamides: the use of conformational analysis in the development of a novel series of potent opioid kappa agonists.

This paper describes the synthesis of a series of N-[2-(1-pyrrolidinyl)ethyl]acetamides (1), methylated at C1 and/or C2 of the ethyl linking group, and their biological evaluation as opioid kappa agonists. Conformational analysis of corresponding desaryl analogues 2 suggested that only those compounds capable of occupying an energy minimum close to that of the known kappa agonist N-[2-(1-pyrrolidinyl)cyclohexyl] acetamide U-50488 might possess kappa agonist properties. Starting from chiral amino acids, other alkyl and aryl substituents were introduced at C1 of the ethyl-linking moiety, giving compounds capable of adopting the same conformation as U-50488. The most potent of these, 2-(3,4-dichlorophenyl)-N-methyl-N-[(1S)-1-phenyl-2-(1-pyrrolidinyl)ethyl] acetamide (8), was 146-fold more active than U-50488 in vitro in the mouse vas deferens model and exhibited potent naloxone-reversible analgesic effects (ED50 = 0.004 mg/kg sc) in an abdominal constriction model.     

Olanzapine degradation kinetics in aqueous solution

The degradation kinetics of olanzapine as a function of pH and temperature has been studied by a spectrophotometric method. The degradation reaction rates were observed to follow first-order kinetics with respect to olanzapine. The hydrolytic reaction was shown to be hydrogen and hydroxide ion-catalyzed and the Arrhenius plots showed the temperature dependence of olanzapine degradation.     

Degradation and epimerization kinetics of moxalactam in aqueous solution

The kinetics of epimerization and degradation of moxalactam in aqueous solution was investigated by HPLC. The pH-rate profiles of the degradation and epimerization were determined separately over the pH range of 1.0-11.5 at 37 degrees C and constant ionic strength 0.5. The degradation and simultaneous epimerization were followed by measuring both of the residual R- and S-epimers of moxalactam and were found to follow pseudo-first-order kinetics. The degradation was subjected to hydrogen ion and hydroxide ion catalyses and influenced by the dissociation of the side chain phenolic group. The epimerization rates were influenced significantly in the acidic region by the dissociation of the side chain carboxylic acid group and in the basic region by hydroxide ion catalysis. The pH-degradation rate profile of moxalactam showed a minimum degradation rate constant between pH 4.0 and 6.0. The pH-epimerization rate profiles of moxalactam showed minimum epimerization rate constants at pH 7.0. The epimerization rate constants of the R- and S-epimers were not very different.     

N-(3-甲基-1-吡咯烷基)-1-丁酮基-苯丙酰胺的合成研究

目的:合成心血管疾病新治疗靶点小分子白介素1受体/髓样分化蛋白88-TIR(Toll/IL-1receptor)(IL-1R/MyD88-TIR)拟似物N-(3-甲基-1-吡咯烷基)-1-丁酮基-苯丙酰胺。方法:以N-叔丁氧羰基-L-缬氨酸羟基琥珀酰亚胺酯为原料,先合成3-甲基-2-叔丁氧羰氨基-1-吡咯烷基-1-丁酮,再合成N-(3-甲基-1-吡咯烷基)-1-丁酮基-苯丙酰胺,产物结构经核磁共振(NMR)和质谱(MS)确证。结果:通过2步反应合成了N-(3-甲基-1-吡咯烷基)-1-丁酮基-苯丙酰胺,反应总收率为81.1%,产物结构经NMR和MS证实为目标化合物。结论:该反应条件温和,操作方便,收率较高。     

Degradation kinetics and mechanism of N6-[(dimethylamino)methylene]mitomycin C in aqueous solutions

The degradation of N6-[(dimethylamino)methylene]mitomycin C, a semisynthetic analogue of mitomycin C, was studied in aqueous solution. The compound degraded rapidly and followed pseudo-first-order kinetics in both acidic (pH less than 5) and basic pH greater than or equal to 9) media. In the near-neutral pH region, however, biphasic kinetics were observed. At the pH of maximum stability (6.5), 10% activity was lost after approximately 6 h at 22 degrees C. Citrate and phosphate species were catalytic at pH 6.5. Spectrophotometric and HPLC methods were used to elucidate the degradation mechanism at pH 7-9. Under these conditions, equilibrium addition of one water molecule into the amidine side chain occurred, followed by parallel formation of mitomycin C and N6-(formyl)mitomycin C. The latter compound subsequently hydrolyzed to mitomycin C.     

Kinetics and mechanism of degradation of cefotaxime sodium in aqueous solution

The degradation kinetics and mechanism of a potent new cephalosporin, cefotaxime sodium, in aqueous solution were investigated at pH 0-10 at 25 degrees and an ionic strength of 0.5. The degradation rates were determined by high-pressure liquid chromatography and were observed to follow pseudo first-order kinetics with respect to cefotaxime sodium concentration. The data suggested that the rate of degradation was influenced significantly by solvolytic, hydrogen ion, and hydroxide ion catalysis. No primary salt effects were observed in the acid or neutral regions; however, a positive salt effect was observed at pH 8.94. Buffer catalysis due to the buffer species employed was not seen during the kinetic studies. The pH-rate profile at 25 degrees indicated that the maximum stability of cefotaxime sodium occurred in the pH 4.5-6.5 region. In aqueous solution, cefotaxime was shown to degrade by two parallel reactions: de-esterification at the C-3 position and beta-lactam cleavage. Good agreement between the theoretical pH-rate profile and the experimental data support the proposed degradation process.     

Stability study of the anticonvulsant enaminone (E118) using HPLC and LC-MS.

The stability of the new chemical synthetic enaminone derivative (E118) was investigated using a stability-indicating high-performance liquid chromatography (HPLC) procedure. The examined samples were analyzed using a chiral HSA column and a mobile phase (pH 7.5) containing n-octanoic acid (5 mM), isopropyl alcohol and 100 mM disodium hydrogen phosphate solution (1:9 v/v) at a flow rate of 1 ml min(-1). The developed method was specific, accurate and reproducible. The HPLC chromatograms exhibited well-resolved peaks of E118 and the degradation products at retention times <5 min. The stability of E118 was performed in 0.1 M hydrochloric acid, 0.1 M sodium hydroxide, water/ethanol (1:1) and phosphate buffer (pH approximately 7.5) solutions. E118 was found to undergo fast hydrolysis in 0.1 M hydrochloric acid solution. The decomposition of E118 followed first order kinetics under the experimental conditions. The results confirmed that protonation of the enaminone system in the molecule enhanced the hydrolysis of E118 at degradation rate constant of 0.049 min(-1) and degradation half-life of 14.1 min at 25 degrees C. However, E118 was significantly stable in 0.1 M sodium hydroxide, physiological phosphate buffer (pH 7.5) and ethanol/water (1:1) solutions. The degradation rate constants and degradation half-lives were in the ranges 0.0023-0.0086 h(-1) and 80.6-150.6 h, respectively. Analysis of the acid-induced degraded solution of E118 by liquid chromatography-mass spectrometry (LC-MS) revealed at least two degradation products of E118 at m/z 213.1 and 113.1, respectively.     

Kinetics of the acidic and enzymatic hydrolysis of benazepril HCl studied by LC.

A reversed-phase high-performance liquid chromatographic (HPLC) method was developed and validated for the kinetic investigation of the chemical and enzymatic hydrolysis of benazepril hydrochloride. Kinetic studies on the acidic hydrolysis of benazepril hydrochloride were carried out in 0.1 M hydrochloric acid solution at 50, 53, 58 and 63 degrees C. Benazepril hydrochloride appeared stable in a pH 7.4 phosphate buffered solution at 37 degrees C and showed susceptibility to undergoing in vitro enzymatic hydrolysis with porcine liver esterase (PLE) in a pH 7.4 buffered solution at 37 degrees C. Benazeprilat appeared to be the major degradation product in both (chemical and enzymatic) studies of hydrolysis. Statistical evaluation of the proposed HPLC methods revealed their good linearity and reproducibility. Relative standard deviation (R.S.D.) was less than 4.76, while detection limits for benazepril hydrochloride and benazeprilat were 13.0 x 10(-7) and 9.0 x 10(-7) M, respectively. Treatment of the kinetic data of the acidic hydrolysis was carried out by non-linear regression analysis and k values were determined. The kinetic parameters of the enzymatic hydrolysis were determined by non-linear regression analysis of the data using the equation of Michaelis-Menten.     

Stability of batanopride hydrochloride in aqueous solutions.

The degradation of batanopride hydrochloride, an investigational antiemetic drug, was studied in aqueous buffer solutions (pH 2-10; ionic strength, 0.5; 56 degrees C) in an attempt to improve drug stability for parenteral administration. Degradation occurs by two different mechanisms depending on the pH of the solution. In acidic media (pH 2-6), the predominant reaction was intramolecular cyclization followed by dehydration to form a 2,3-dimethylbenzofuran. There was no kinetic or analytical (high-performance liquid chromatography) evidence for the formation of an intermediate; therefore, the rate of dehydration must have been very rapid compared with the rate of cyclization. In alkaline media (pH 8-10), the primary route of degradation was cleavage of the C-O alkyl ether bond. In the intermediate pH range (pH 6-8), both reactions contributed to the overall degradation. Both degradation reactions followed apparent first-order kinetics. The pH-rate profile suggests that batanopride hydrochloride attains its optimal stability at pH 4.5-5.5. Citrate buffer was catalytic at pH 3 and 5, and phosphate buffer was catalytic at pH 8. No catalytic effect was observed for the borate buffer at pH 9-10.     

Kinetics of sorption of ionizable solutes by plastic infusion bags

Aqueous solutions of several ionizable substances were stored in plastic infusion bags and the sorption of the substances monitored with time. The substances used were p-nitrophenol, p-toluidine, warfarin sodium [3-(alpha-acetonylbenzyl)-4-hydroxycoumarin sodium salt] and trifluoperazine hydrochloride (10-[3-(4-methyl-1-piperazinyl)propyl]-2-(trifluoromethyl)phenothiazine dihydrochloride). The rate and extent of sorption for each substance varied with pH and was consistent with a preferential uptake of the un-ionized species. The uptake of p-nitrophenol and p-toluidine was adequately described by a diffusion model derived assuming that sorption is rate-controlled by the diffusivity of the solute in the plastic matrix, and that only the un-ionized species was sorbed by the plastic matrix. However, the uptake of warfarin sodium and trifluoperazine hydrochloride was described more accurately by a diffusion model in which the diffusional resistance of the plastic matrix and of an interfacial resistance barrier both contributed to the diffusional resistance encountered in the sorption process. It appeared that the rate of uptake of the un-ionized form of these solutes was diminished due to the influence of interfacial or aqueous diffusional barriers. Solute lipophilicity and degree of ionization appeared to be important factors determining the relative contribution of the respective barriers to the overall diffusional resistance.     

Kinetic study of alkaline induced hydrolysis of the skeletal muscle relaxant chlorzoxazone using ratio spectra first derivative spectrophotometry

2-Amino-4-chlorophenol was found to be the alkaline induced degradation product and the synthetic precursor of chlorzoxazone. The aim of this work is to study different factors affecting the degradation process due to the high toxicity of 2-amino-4-chlorophenol. Chlorzoxazone was found to follow pseudofirst order kinetics. Ratio spectra first derivative spectrophotometry (DR(1)) was developed for monitoring the change in chlorzoxazone concentration during the degradation process. Kinetic parameters (rate constant (K) and half-life (t(0.5))) were calculated at different temperatures (40-120 degrees C) and different sodium hydroxide concentrations (3-10 M). Activation energy at 3 and 8 M sodium hydroxide concentration and alkaline induced catalysis constant at 60, 70 and 80 degrees C were also calculated.