Ferric Hydroxide
Ferric Hydroxide - Related Videos
08:21
Optimized Procedure for Determining the Adsorption of Phosphonates onto Granular Ferric Hydroxide using a Miniaturized Phosphorus Determination Method
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Cited by 7 •
2018
This paper introduces a procedure to investigate the adsorption of phosphonates onto iron-containing filter materials, particularly granular ferric hydroxide, with little effort and high reliability. In a buffered solution, the phosphonate is brought into contact with the adsorbent using a rotator and then analyzed via a miniaturized phosphorus determination method.
10:37
Ferric Chloride-induced Murine Thrombosis Models
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Cited by 56 •
2016
We report a refined procedure of the ferric chloride (FeCl3)-induced thrombosis models on carotid and mesenteric artery as well as vein, characterized efficiently using intravital microscopy to monitor time to occlusive thrombi formation.
07:34
Establishment of a Modified Ferric Chloride-Induced Superior Sagittal Sinus Thrombosis
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2025
This study presents a protocol for establishing a reproducible, minimally invasive rat model of superior sagittal sinus thrombosis induced by ferric chloride, utilizing a silk-suture method in combination with laser speckle contrast imaging and high-resolution ultrasound for evaluation.
07:26
Ferric Chloride-induced Thrombosis Mouse Model on Carotid Artery and Mesentery Vessel
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Cited by 49 •
2015
The FeCl3 induced thrombosis model in mice is described herein. A method to monitor thrombus growth by intravital microscopy observation on a mesenteric vessel and by blood flow measurement in the carotid artery is presented.
05:50
Facile Preparation of Ultrafine Aluminum Hydroxide Particles with or without Mesoporous MCM-41 in Ambient Environments
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Cited by 2 •
2017
An ultrafine aluminum hydroxide nanoparticle suspension was prepared via the controlled titration of [Al(H2O)]3+ with L-arginine to pH 4.6 with and without cage-effect confinement within mesoporous channels of MCM-41.
FAQs
Formation is governed by the equilibrium between dissolved iron(III) species, hydroxide ions, and the solid phase. Increasing hydroxide availability promotes precipitation, while the observed amount also depends on iron and hydroxide concentrations. Because the equilibrium is pH-sensitive, changing pH can alter whether iron(III) remains dissolved or appears as a reddish-brown solid during aqueous analysis.
The concentrations of the reacting ions influence how much solid forms and how the precipitation equilibrium is established. Higher or lower concentrations can change the visible intensity and extent of the ferric hydroxide precipitate, so qualitative observations should be interpreted alongside the solution conditions rather than treated as independent of concentration.
A freshly formed precipitate may not have the same properties as one that has remained in solution over time. Aging can influence the material’s structure and product characteristics, contributing to the presence of hydrated forms rather than one precisely defined molecular arrangement. This matters when comparing precipitate appearance or behavior between experiments performed under different time conditions.
The formula Fe(OH)₃ is commonly used to represent the compound, but precipitated material can contain water and may not correspond to one uniform molecular structure. Recognizing this distinction helps explain why its properties can vary with preparation conditions, pH, concentration, and aging, especially when the solid later serves as a precursor to related iron oxides.
In a qualitative analysis, iron(III) ions are brought into contact with hydroxide ions under aqueous conditions. A reddish-brown precipitate provides the characteristic visual observation associated with iron(III). The result should be considered together with the solution’s pH and concentrations, since those conditions influence the precipitation equilibrium and the amount of solid that appears.
Its high surface area provides many sites that can interact with dissolved substances in water. This property supports removal of phosphate, arsenate, and other contaminants, making the material useful beyond simple precipitation chemistry. In treatment applications, performance therefore depends on the solid’s surface properties as well as the composition of the water being processed.
Ferric hydroxide can serve as a precursor to iron oxides and related materials. Its formation provides an intermediate solid whose properties are influenced by hydration, equilibrium conditions, and aging. This role connects aqueous precipitation chemistry with materials preparation, because subsequent changes to the precursor can lead to iron-containing products with different structures or characteristics.