Phenylketonuria
William L. Nyhan, Georg F. Hoffmann, Aida I. Al-Aqeel, Bruce A. Barshop in Atlas of Inherited Metabolic Diseases, 2020
In the presence of a defect in phenylalanine hydroxylase, the first compound that accumulates is phenylalanine itself. In classic PKU, the plasma concentration of phenylalanine is virtually always above 1200 μmol/L. It is transaminated (see Figure 15.1) to form phenylpyruvic acid, the phenylketone for which the disease was named. There is a roughly linear relationship between the concentrations of phenylalanine in the blood and the urinary excretion of phenylpyruvic acid [44]. This is the compound that is responsible for the positive ferric chloride (FeCl3) test. A deep green color is seen on the addition of 10 percent (FeCl3) to the urine of patients with untreated PKU (see Figure 15.2). Phenylpyruvic acid is subsequently converted to phenyllactic acid, phenylacetic acid, and phenylacetylglutamine. Phenylpyruvate is also hydroxylated in the ortho position, ultimately yielding orthohydroxyphenylacetic acid. These are not abnormal metabolites, but normal ones that occur in abnormal amounts in PKU. It is current theory that it is this abnormal chemical milieu in which the patient with PKU lives that produces the severely impaired mental development and other manifestations of the disease.
For The Want of a Nail … Trace Elements in Health and Disease
Owen M. Rennert, Wai-Yee Chan in Metabolism of Trace Metals in Man, 2017
In the acidic environment of the stomach, three events set the stage for the absorption of the metal by the small intestine. Much of the ferric iron becomes soluble as ferric chloride. Proteins are denatured to liberate ferric iron, and small particles of metallic iron of fortification are oxidized first to ferrous iron. It is in the small intestine that the solution chemistry of iron determines its biological fate. The stomach contents are rapidly neutralized in the duodenum. Most of the iron precipitates as insoluble ferric hydroxides, phosphates, and carbonates. Some iron binds to molecules present in foods such as phytic acid and fibers — constituents of many plant foods — and is made unavailable for transport. The ferrous iron is rapidly oxidized to form ferric ion unless there are large amounts of reducing agents such as vitamin C present. That fraction of the iron which forms soluble, low molecular weight complexes with sugars and amino acids is the only metal that can be effectively transported to the blood.11 Heme iron is transported into the intestinal cells where it is oxidized to release the metal ion for further metabolism.
Methods of Phyto-Constituent Detection
Ravindra Kumar Pandey, Shiv Shankar Shukla, Amber Vyas, Vishal Jain, Parag Jain, Shailendra Saraf in Fingerprinting Analysis and Quality Control Methods of Herbal Medicines, 2018
Legal's test: Mix the test drug with a mixture of sodium nitroprusside and pyridine. Treatment with methanol alkali to produce a deep red color.Feigel's test: Shake the acidified test drug with solvent ether and add few drops of saturated alcoholic solution of potassium hydroxide in a porcelain crucible heated over a flame until cooling. It produces a light pink color with a 1% ferric chloride solution.Baljel's tests: Mix the test drug with a solution of sodium picrate to give it a yellow-orange color.
Ferric chloride ingestion with corrosive gastritis
Published in Clinical Toxicology, 2022
Mark Pucci, Pavlos Theodorou, Neel Patel
Ferric chloride, or iron (III) chloride (FeCl3), is a compound with industrial uses including copper etching and water treatment. It forms a strongly acidic solution with high iron content, and therefore has the potential for severe toxicity to humans, although oral ingestions are rare. A retrospective study which included 13 cases of accidental or intentional oral ingestion of ferric chloride found major symptoms and signs were: nausea and vomiting, sore throat, abdominal pain, oral ulceration, metabolic acidosis, aspiration pneumonia, respiratory failure, diarrhea, and hypotension [1]. Common laboratory findings include leucocytosis, metabolic acidosis, coagulopathy, and elevated serum iron concentration [1,2]. Direct corrosive effects can lead to gastrointestinal tract ulceration and inflammation, with perforation and necrosis in severe cases [1–3]. Desferrioxamine as an iron chelating agent may be indicated if there are features of severe iron toxicity, but supportive care and management of complications remain the mainstay of treatment [1].
How useful are ferric chloride models of arterial thrombosis?
Published in Platelets, 2020
Steven P. Grover, Nigel Mackman
Additional studies have demonstrated that ferric chloride exposure can lead to aggregation of erythrocytes and platelets independently of the endothelial surface [9]. In an in vitro microfluidic system exposure of washed erythrocyte or platelets to ferric chloride under flow was sufficient to induce aggregation and accumulation on a non-endothelialized chamber surface [9]. Moreover, in this microfluidic system ferric chloride exposure induced plasma protein agglutination [9]. The ability of ferric chloride to rapidly induce aggregation of cells and proteins suggests that a physiochemical mechanism is likely involved. Indeed, ferric chloride is a flocculant, a chemical species that facilitates binding of molecules, that is used in chemical processes to remove suspended impurities [10].
Preparation, characterization and dynamical mechanical properties of dextran-coated iron oxide nanoparticles (DIONPs)
Published in Artificial Cells, Nanomedicine, and Biotechnology, 2018
Hatice Kaplan Can, Serap Kavlak, Shahed ParviziKhosroshahi, Ali Güner
Iron-oxide nanoparticles were prepared by co-precipitation method which is probably the simplest and offers some advantages: simple and rapid preparation, easy control of particle size and composition, various possibilities to modify the particle surface state allowing making homogenous and stable dispersions in liquid or solid media. Iron oxides (Fe3O4 or γFe2O3) are usually prepared by an aging stoichiometric mixture of ferrous and ferric salts in aqueous medium. Ferric chloride hexahydrate (FeCl3·6H2O) and ferrous chloride tetrahydrate (FeCl2·4H2O), in the 2 M HCl were mixed at 95 °C (Fe2+/Fe3+ = ½). After this process, the mixture was dropped into 220 ml of NaOH (2.2 mol/l) solution under vigorous stirring for about 35 min. Black precipitate immediately formed and the precipitate of magnetite was transformed into γ-Fe2O3 particles by repeated treatment with HNO3 (2.0 mol/l) and FeNO3 (0.3 mol/l) solutions (Scheme 1). The acidic precipitate was isolated by decantation on a magnet, separated by centrifugation (6000 rpm), then washed in acetone and dispersed in deionized water.
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