Impact of the haplotype CYP3A4*16B harboring the Thr185Ser substitution on paclitaxel metabolism in Japanese patients with cancer.

OBJECTIVE: Paclitaxel is one of the most important anticancer drugs for the treatment of various tumors such as non-small cell lung cancer. We investigated the association between CYP3A4 haplotypes and pharmacokinetic parameters of paclitaxel metabolism. METHODS: This study enrolled 235 Japanese patients with cancer who were receiving paclitaxel. These patients were screened for CYP3A4 gene polymorphisms by either direct sequencing or pyrosequencing. Plasma concentrations of paclitaxel and its 3 metabolites were determined by HPLC in 229 patients. RESULTS: Median values of paclitaxel clearance, normalized for body surface area, were lower in the high-dose group (>or=175 mg/m2, n = 199) than in the low-dose group (

Near-infrared analysis of protein secondary structure in aqueous solutions and freeze-dried solids.

Near-infrared spectroscopy (NIR) of various proteins (bovine serum albumin, lysozyme, ovalbumin, gamma-globulin, beta-lactoglobulin, myoglobin, cytochrome-c) was investigated as a possible analytical method of the protein secondary structure in various physical states. The spectra of proteins in aqueous solutions (transmission mode, solvent-compensated) and those in freeze-dried solids (nondestructive diffuse reflection mode) showed several bands at similar frequencies in the combination (4000-5000 cm(-1)) and first overtone (5600-6600 cm(-1)) spectral regions. The normalized second-derivative near-infrared spectra of proteins in aqueous solutions suggested that some bands indicated alpha-helix (4090, 4365-4370, 4615, and 5755 cm(-1)) and beta-sheet (4060, 4405, 4525-4540, 4865, and 5915-5925 cm(-1)) structures. The proteins mostly maintained spectra characteristic of their native structure after freeze-drying, although some reductions in alpha-helical structure and increase in unordered or beta-sheet structures were observed. The near-infrared analysis also showed beta-sheet formation of heat-treated BSA in aqueous solutions and in subsequently freeze-dried solids. The present results thus indicated that the nondestructive near-infrared analysis can be used for the investigation of dehydration-induced changes in protein secondary structures.

Effect of polymer size and cosolutes on phase separation of poly(vinylpyrrolidone) (PVP) and dextran in frozen solutions.

The aim of this study was to elucidate the effect of the molecular weight of polymers on their miscibility in frozen solutions to model the physical properties of freeze-dried pharmaceutical formulations. Thermal analysis of frozen solutions containing poly(vinylpyrrolidone) (PVP) and dextran of various molecular weights was performed at polymer concentrations below the binodal curve at room temperature. Frozen solutions containing PVP 29,000 and dextran 10,200 showed two thermal transitions (glass transition temperature of maximally freeze-concentrated solution: Tg') representing two freeze-concentrated amorphous phases, each containing predominantly one of the polymers. A combination of smaller polymers (PVP 10,000 and dextran 1,060) was freeze-concentrated into an amorphous mixture phase across a wide range of concentration ratios. Combinations of intermediate size polymers separated into two freeze-concentrated phases only at certain concentration ratios. Addition of NaCl prevented the phase separation of PVP and dextran in the aqueous and frozen solutions. Higher concentrations of NaCl were required to retain the miscibility of larger polymer combinations in the freeze-concentrate. The molecular weights of the component polymers, polymer concentration ratio, and cosolute composition are the important factors that determine component miscibility in frozen solutions.

Effect of inorganic salts on crystallization of poly(ethylene glycol) in frozen solutions.

The effect of inorganic salts on eutectic crystallization of poly(ethylene glycol) (PEG) 1500-20,000 in frozen solution was studied to model the polymer and inorganic salt interaction in freeze-dried formulations. Thermal analysis of an aqueous PEG 3000 solution showed a eutectic PEG crystallization exotherm at approximately -47 degrees C and a subsequent PEG crystal melting endotherm at -14.9 degrees C. Addition of sodium chloride prevented the PEG crystallization in the freeze-concentrated solution surrounding ice crystals. Higher concentration NaCl was required to retain higher molecular weight PEG in the amorphous state. Various inorganic salts prevented the PEG crystallization to varying degrees depending mainly on the position of the anion in the Hofmeister's lyotropic series. Some salting-in and 'intermediate' salts (NaSCN, NaI, NaBr, NaCl, LiCl, KCl, and RbCl) inhibited the crystallization of PEG 7500 in frozen solutions. On the other hand, salting-out salts (NaH2PO4, Na2HPO4, Na2SO4, and NaF) did not show an apparent effect on the PEG crystallization. Some salting-out salts induced PEG crystallization in PEG and sucrose combination frozen solutions. The varying abilities of salts to prevent the PEG crystallization in frozen solutions strongly suggested that the solutes had different degrees of miscibility in the freeze-concentrates.

Effect of counterions on the physical properties of l-arginine in frozen solutions and freeze-dried solids.

The objective of this study was to elucidate the physical properties of L-arginine and various counterion combinations in frozen aqueous solutions and in freeze-dried solids. L-Arginine remains amorphous in the highly concentrated non-ice phase in frozen solutions with a Tg (glass transition temperature of maximally freeze-concentrated solutes) of -41.4 degrees C. Some acids and salts (e.g., H3PO4, H2SO4, HNO3, and NaH2PO4) raised the Tg , whereas others (e.g., HCl, CH3COOH, HCOOH, Na2HPO4, and NaCl) had little effect or lowered the L-arginine Tg . Co-lyophilization with phosphoric acid also raised the glass transition temperature (Tg) of amorphous freeze-dried L-arginine solids. Arginine-H3PO4 combinations exhibited properties that led to either the stabilization or destabilization of a model protein (lactate dehydrogenase: LDH) during freeze-drying, depending on their concentration ratios. Fourier-transform infrared (FT-IR) and diffusion reflectance near-infrared (NIR) spectra indicated the presence of interactions between the amino and/or guanidyl groups of L-arginine and phosphate ions in the amorphous freeze-dried cakes. It was postulated that the interaction between L-arginine and the multivalent counterions, as well as an increase in hydrogen bonding network, reduced the mobility of molecules in the frozen solutions and freeze-dried solids.

Effects of sodium tetraborate and boric acid on nonisothermal mannitol crystallization in frozen solutions and freeze-dried solids.

The purpose of the present study was to elucidate the effects of sodium tetraborate (borax) and boric acid on the crystallization of mannitol in frozen aqueous solutions and freeze-dried solids. Thermal analysis of frozen solutions showed that sodium tetraborate inhibits mannitol crystallization at sodium tetraborate/mannitol molar concentration ratios of approximately 0.05, which is much lower than the other co-solutes studied (boric acid, sucrose, sodium phosphate buffer). Inhibition of the mannitol crystallization in frozen solutions resulted in highly amorphous mannitol in the freeze-dried solids. Mannitol remained in an amorphous state in some of the combination freeze-dried solids, even at elevated temperatures. Changes in the thermal transition temperatures (glass transition temperature of maximally freeze-concentrated solute ( T'g) and glass transition temperature of freeze-dried solid (Tg)) suggested reduced mannitol molecular mobility with increases in the sodium tetraborate ratio. Fourier-transform infrared spectroscopy (FT-IR) analysis of the bovine serum albumin secondary structure showed apparent protein structure-stabilizing effects of the amorphous mannitol and sodium tetraborate combination during the freeze-drying process. The mannitol and sodium tetraborate combination also protected lactate dehydrogenase (LDH) from inactivation during freeze-drying. We conclude that the complex formation and the accompanying reduction in molecular mobility make sodium tetraborate an effective mannitol crystallization inhibitor in frozen solutions and freeze-dried solids.

Inhibition of mannitol crystallization in frozen solutions by sodium phosphates and citrates.

Effects of co-solutes on the physical property of mannitol and sorbitol in frozen solutions and freeze-dried solids were studied as a model of controlling component crystallinity in pharmaceutical formulations. A frozen mannitol solution (500 mM) showed a eutectic crystallization exotherm at -22.8 degrees C, whereas sorbitol remained amorphous in the freeze-concentrated fraction in the thermal scan. Various inorganic salts reduced the eutectic mannitol crystallization peak. Trisodium and tripotassium phosphates or citrates prevented the mannitol crystallization at much lower concentrations than other salts. They also raised transition temperatures of the frozen mannitol and sorbitol solutions (T(g)': glass transition temperature of maximally freeze-concentrated amorphous phase). Crystallization of some salts (e.g., NaCl) induced crystallization of mannitol at above certain salt concentration ratios. Thermal and near-infrared analyses of cooled-melt amorphous sorbitol solids indicated increased intermolecular hydrogen-bonding in the presence of trisodium phosphate. The sodium phosphates and citrates should prevent crystallization of mannitol in frozen solutions and freeze-dried solids by the intense hydrogen-bonding and reduced molecular mobility in the amorphous phase.

Mass variation tests for coating tablets and hard capsules: rational application of mass variation tests.

The mass variation test is a simplified alternative test version of the content uniformity test. In the case of coating tablets and capsules, the mass variation test is principally applied to test the inner cores or fillings containing the active ingredient. However, some exceptions exist in pharmacopoeias. The effects of tablet coating and capsule shell on the results of the mass variation test were studied. The mass variation of outer crusts (coatings, capsule shells) and inner cores (core tablets, fillings) was measured separately in several products. The effects of coating on weight variability were very large for sugar-coated tablets. Relative standard deviation (RSD) of the formulation weight (RSD(W)) of sugar-coated tablets (2.73%) was larger than that of plain tablets (0.77%). The cause of the large RSD(W) is the large variation the weight of sugar-coating accounting for 44% of formulation weight. In the case of film-coated tablets, the effect of coating weight on the mass variation test was very small because the rate of coating in comparison to the whole weight was small. In the case of hard capsules, the usage of whole formulation weight resulted in underestimation of variations of filling weight. The differences between dosage forms in the applicability of the mass variation test are caused by differing weight proportions and variability of the outer coatings or shells. To avoid the underestimation of mass variation for hard capsules, a corrected acceptance value is useful. For all the dosage units, the mass variation test can principally be applied to determine which mass is expected to be proportional to the content of the active ingredient. However, some modification of acceptance values enables application of the mass variation tests to inapplicable cases, such as when the RSD of drug concentration (RSD(C)) is larger than 2%.

Effect of sodium tetraborate (borax) on the thermal properties of frozen aqueous sugar and polyol solutions.

The effect of sodium tetraborate (Na(2)B(4)O(7), borax) on the thermal property of frozen aqueous sugar and polyol solutions was studied through thermal analysis. Addition of borax raised the thermal transition temperature (glass transition temperature of maximally freeze-concentrated solutes; T(g)') of frozen sucrose solutions depending on the borax/sucrose concentration ratios. Changes in the T(g)' of frozen mono- and disaccharide solutions suggested various forms of complexes, including those of a borate ion and two saccharide molecules. Borax exerted the maximum effect to raise the oligosaccharide and dextran T(g)'s at borax/saccharide molar ratios of approximately 1-2 (maltose and maltooligosaccharides), 2 (dextran 1060), 5 (dextran 4900), and 10 (dextran 10200). Further addition of borax lowered T(g)'s of the saccharide solutions. Borax also raised T(g) and T(g)' temperatures of frozen aqueous glycerol solutions. The decreased solute mobility in frozen solutions by the borate-polyol complexes suggested higher collapse temperature in the freeze-drying process and improved stability of biological systems in frozen solutions.

Protection of protein secondary structure by saccharides of different molecular weights during freeze-drying.

The protective effects of saccharides with various molecular weights (glucose, maltose, maltotriose, maltotetraose, maltopentaose, maltoheptaose, dextran 1060, dextran 4900, and dextran 10200) against lyophilization-induced structural perturbation of model proteins (BSA, ovalbumin) were studied. Fourier transform infrared (FT-IR) analysis of the proteins in initial solutions and freeze-dried solids indicated that maltose conferred the greatest protection against secondary structure change. The structure-stabilizing effect of maltooligosaccharides decreased in increasing the number of saccharide units. Larger molecules of dextran also showed a smaller structure-stabilizing effect. Increasing the effective saccharide molecular size by a borate-saccharide complexation reduced the protein structure-stabilizing effect of all of the saccharides except glucose. The results indicate that the larger saccharide molecules, and/or the complex formation with borate ion, reduce the free and accessible hydroxyl groups to interact with and stabilize the protein structure by a water-substitution mechanism.

Abnormal dissolutions of chlorpromazine hydrochloride tablets in water by paddle method under a high agitation condition.

All sugar-coated tablets of chlorpromazine hydrochloride except for those produced by one manufacture showed concave dissolution profiles in water by paddle method at 100 rpm but not at 50 rpm. The study was undertaken to clarify the agitation-dependent abnormal dissolutions. The strange dissolutions were also observed in water at different ionic strengths but not in buffer solutions of pH 1.2, 4.0 and 6.8. When monitored, the pH's of water in dissolution vessels for the abnormal tablets increased with time at 100 rpm and some of them exceeded pH 8 but did not at 50 rpm. The solubility of chlorpromazine hydrochloride decreased with the increase of pH which was too low to dissolve the whole amount of drug contained in a tablet at pH 8. The elevation of pH seemed to be mainly brought about by dissolution of calcium carbonate popularly used for sugar-coated tablets, because larger amount of calcium ion was dissolved out from the abnormal tablets at 100 rpm than from a normal tablet and from them at 50 rpm. These findings indicate that the concave dissolution profiles should be caused by the decrease of drug solubility with increase in pH of water, probably because of dissolution of calcium carbonate. We should pay attention to the change in pH of water which may differ depending on the agitation speed of dissolution tests.