The largest database of trusted experimental protocols
> Chemicals & Drugs > Inorganic Chemical > Ferric nitrate

Ferric nitrate

Ferric nitrate, a chemical compound with the formula Fe(NO3)3, is a widely used compound in various industries and research applications.
It is a crystalline solid that is soluble in water and is commonly used as an oxidizing agent, a food preservative, and a mordant in textile dyeing.
Ferric nitrate has a wide range of applications, including in the production of steel, the treatment of water, and the synthesis of other chemical compounds.
Researchers in fields such as materials science, environmental chemistry, and biochemistry may find ferric nitrate useful in their experiments and studies.
This MeSH term provides a concise overview of the key properties and uses of ferric nitrate, helping researchers easily identify its relevance to their work.

Most cited protocols related to «Ferric nitrate»

Protocol full text hidden due to copyright restrictions

Open the protocol to access the free full text link

Publication 2015
Acids ammonium acetate ammonium nitrate Ammonium Oxalate Ascorbic Acid Bicarbonate, Sodium Carbonates Citrate Copper Dietary Fiber Digestion Dithionite Gypsum Ion, Bicarbonate Ions Ligands Mass Spectrometry Metals Microscopy Neutron Activation Analysis Nitrogen Oxides Plant Development Plasma Salts Sodium Citrate Sodium Dithionite sodium phosphate Spectrum Analysis Vision
M1 defined medium containing 0.02% (w/v) of vitamin-free Casamino Acids and 15 mM lactate was used in all physiological experiments [72 (link)]. Growth of the deletion strain under aerobic or anaerobic conditions was determined by recording growth curves in triplicate with a Bioscreen C microbiology reader (Labsystems Oy, Helsinki, Finland) with MR-1 as the control. For aerobic growth, exponential phase cultures were diluted to approximately ~1 × 105 cells/ml in fresh medium, and 400 μl was transferred to the honeycomb plate wells of the Bioscreen C reader. The cultures were shaken at medium intensity continuously, and the turbidity was measured every 30 min at 600 nm and DO (dissolved oxygen) was recorded every hour with an Accumet XL40 meter (Fisher Scientific). For anaerobic growth, exponential phase cultures grown aerobically were centrifuged, purged in nitrogen and suspended in fresh medium to approximately ~1 × 105 cells/ml in an anaerobic glove box. Electron acceptors tested in this study included fumarate (20 mM), nitrate (2 mM), nitrite (1 mM), thiosulfate (3 mM), TMAO (20 mM), and DMSO (20 mM). For electron acceptors containing metals including MnO2 (5 mM), ferric citrate (10 mM), and cobalt(III)-EDTA (200 μM), growth was monitored by the color change of the cultures and cell counting under a microscope (Nikon Optiphot, Nikon, Japan).
Survival of MR-1 and the ΔarcA strain during the stationary phase was examined. Cultures were grown from a single colony under aerobic conditions with vigorous shaking. After the onset of stationary phase, the cultures were divided into two parts. One was kept in the incubator with vigorous shaking and the other was kept still. The cultures were serially diluted into LB and plated onto LB plates every 12 h. Plates from dilutions that gave 100 to 250 colony form units (CFU) per plate were used to minimize statistical variation due to small sample sizes. Experiments were done in triplicate.
Publication 2008
Bacteria, Aerobic casamino acids Cells Cobalt Cultural Evolution Deletion Mutation Edetic Acid ferric citrate Fumarate Lactate Metals Microscopy Nitrates Nitrites Nitrogen Oxidants Oxygen physiology Strains Sulfoxide, Dimethyl Technique, Dilution Thiosulfates trimethyloxamine Vitamins

Legionella pneumophila (L. pneumophila) strain Lp02, is a thymine auxotrophic derivative of Philadelphia-1 [19] (link). The dotA mutant strain Lp03 is defective in the Dot/Icm Type IV secretion system [68] (link). The flaA mutant L. pneumophila was previously described [69] (link). Bacterial strains were supplemented with a plasmid that complements thymine auxotrophy and expresses green fluorescent protein (GFP) at the post-exponential phase (PE) [22] (link),[45] (link). L. pneumophila was cultured as described previously [22] (link),[45] (link) in ACES-yeast extract broth supplemented with ferric nitrate and L-cysteine. All experiments were performed in the absence of ferric nitrate and L-cysteine from the macrophage culture medium, to allow L. pneumophila multiplication only intracellularly. All in vitro infections were performed at an MOI of 0.5 for 30 minutes followed by rinsing of the infected macrophages which allowed the infection of 20–25% of macrophages with usually 1 organism, unless stated otherwise [28] (link). The quantification of the colony-forming units (CFU) in vitro and in vivo was performed as described [28] (link).
Publication 2009
Bacteria Complement System Proteins Culture Media Cysteine ferric nitrate Green Fluorescent Proteins Infection Legionella pneumophila Macrophage N-(2-acetamido)-2-aminoethanesulfonic acid Plasmids Strains tetraxetan Thymine Type IV Secretion Systems Yeast, Dried
Lactoferrin supplied by the manufacturers was used without further purification. For apolactoferrin, preparation containing 50 mg/mL protein was dissolved in water and dialyzed extensively against 100 mM citrate buffer for 24 h, followed by dialysis against distilled water for 24 h [37 (link)]. Temperature (4 and 20 °C) and buffer pH (2.0–5.0) were modified in order to monitor their impact on iron desaturation. Iron saturation was calculated based on the A280/A466 ratio according to the calibration curve presented in “Results and discussion.” We define the iron saturation level of lactoferrin as the percentage of iron-binding sites occupied by ferric ions assuming that 2 mol of iron(III) ions is bound per 1 mol of protein. Thus, the given values refer to the percentage of differic lactoferrin. For some of these samples, the ICP-MS and ELISA tests were carried out and were used to prepare a calibration curve.
Hololactoferrin was prepared by the reaction of 50 mg/mL lactoferrin solution in 50 mM Tris–HCl, 150 mM NaCl (pH 7.4) with ferric nitrate salt in the presence of nitrilotriacetic acid (NTA) as well as different concentrations of sodium bicarbonate [24 (link)]. After incubation, excess iron was removed by dialysis against the same buffer solution without ferric salts for 24 h and against water for another 24 h. Various incubation times, temperatures, as well as ratios of Lf/Fe/NTA were employed to examine their effect on iron saturation efficiency; detailed conditions are depicted in the captions of figures.
Publication 2013
apolactoferrin Bicarbonate, Sodium Binding Sites Buffers Citrates Dialysis Enzyme-Linked Immunosorbent Assay ferric nitrate Ions Iron Iron Overload Lactoferrin Mol-Iron Nitrilotriacetic Acid PER1 protein, human Proteins Salts Sodium Chloride Tromethamine
Nitrite and nitrate levels were measured as an index of nitric oxide (NO) formation according to the Griess reaction (14 (link)). The level of NO metabolites was expressed as μmol/L for plasma and μmol/mg protein for tissue using sodium nitrite as standard (0-100 μmol/L). Concentration of reduced glutathione (GSH) in tissue homogenate and plasma was determined using DTNB, which develops a yellow color complex with GSH (15 (link)). The content of GSH was calculated using a molar absorption coefficient of 1.36×103 M-1 cm-1 and expressed as μmol/L for plasma and nmol/mg protein for tissue.
Plasma and tissue malondialdehyde (MDA) were determined based on the reaction with TBA (15 (link)). The MDA content was determined using a molar absorption coefficient of 1.56×105 M-1cm-1 and expressed as μmol/mg protein for tissue and μmol/L for plasma. The ferric reducing antioxidant power (FRAP) was determined on the ferric reducing ability of plasma; which is estimated from the reduction of a Fe3+-TPTZ complex to the Fe2+ form at low pH (16 (link)). The FRAP content was expressed as μmol/L for plasma using FeSO4.7H2O solution as standard (0-1500 μmol/L).
PCO content was assayed using a spectrophotometric method based on the color produced by the reaction of DNPH and the carbonyl groups reaction (17 (link)). PCO level was calculated using a molar absorption coefficient of 2.2 × 104 M-1cm-1 and demonstrated as μmoL/mL protein for plasma and μmol/g for tissue. Total thiols (TSH) content was determined based on the reaction with DTNB (15 (link)). Total TSH was calculated using the molar absorption coefficient of 13,600 M-1 cm-l and expressed as μmol/mg protein for tissue.
Publication 2019
A 103 Antioxidants Dithionitrobenzoic Acid Malondialdehyde Molar Nitrates Nitrites Oxide, Nitric Plasma Proteins Reduced Glutathione Sodium Nitrite Spectrophotometry Sulfhydryl Compounds Tissues

Most recents protocols related to «Ferric nitrate»

Lanthanum nitrate, barium nitrate, zirconium nitrate, ferric nitrate, ammonia water, citric acid and anhydrous ethanol were procured from Shanghai Aladdin Industrial Corporation. All reagents were employed as received without any further purification.
Publication 2024
This was measured using trichloroacetic acid (TCA) as the ferric complex, at 460 nm absorbance [4 ]. Milk samples (4.0 mL) were mixed with 2.0 mL of a 20% TCA solution. The mixture was blended well and then allowed to stand for at least 30 min. It was, thereafter, filtered through a suitable filter paper (Whatman No. 40). The clear filtrate (1.5 mL) was then mixed with 1.5 mL of the ferric nitrate reagent (16.0 g Fe (NO3)). A total of 3.9 mL H2O was dissolved in 50 mL of 2M HNO3 and was then diluted with distilled water to 100 mL; the absorbance was measured at 460 nm using a UV spectrophotometer. As a blank, a mixture of 1.5 mL of ferric nitrate solution and 1.5 mL of water was used. The measurement was carried out within 10 min of the addition of the ferric nitrate solution, as the colored complex is not stable for any length of time. The concentration of thiocyanate was then determined by comparison with standard solutions of known thiocyanate concentrations (10, 15, 20, and 30 g/mL of thiocyanate).
Publication 2024
The analytical-grade
reagents were purchased from Sigma-Aldrich: ferric nitrate nonahydrate
(Fe (NO3)3·9H2O), cobalt nitrate
hexahydrate (Co (NO3)2·6H2O),
silver nitrate (AgNO3), and ammonia solution (NH4OH).
Publication 2024

Protocol full text hidden due to copyright restrictions

Open the protocol to access the free full text link

Publication 2024
Balsa wood (Ochroma pyramidale) was purchased from the company Specialized Balsa Wood and cut to size before mineralization. Ferric nitrate nonahydrate (98%+, Fe(NO3)3·9H2O), ferrous chloride tetrahydrate (FeCl2·4H2O), ferric chloride hexahydrate (FeCl3·6H2O), sodium hydrogen arsenate heptahydrate (98%, Na2HAsO4·7H2O), potassium hydroxide (KOH) were purchased from Alfa Aesar. Reagents were not subjected to any further purification before use.
Publication 2024

Top products related to «Ferric nitrate»

Sourced in Germany, United States, India, United Kingdom, Italy, China, Spain, France, Australia, Canada, Poland, Switzerland, Singapore, Belgium, Sao Tome and Principe, Ireland, Sweden, Brazil, Israel, Mexico, Macao, Chile, Japan, Hungary, Malaysia, Denmark, Portugal, Indonesia, Netherlands, Czechia, Finland, Austria, Romania, Pakistan, Cameroon, Egypt, Greece, Bulgaria, Norway, Colombia, New Zealand, Lithuania
Sodium hydroxide is a chemical compound with the formula NaOH. It is a white, odorless, crystalline solid that is highly soluble in water and is a strong base. It is commonly used in various laboratory applications as a reagent.
Sourced in United States, Germany, India, Italy, United Kingdom, Australia, China, Singapore, France, Poland, Chile, Egypt, Mexico, Brazil, Spain
Ferric chloride is an inorganic compound with the chemical formula FeCl3. It is a crystalline solid that is soluble in water and other polar solvents. Ferric chloride is commonly used as a coagulant in water treatment and as a mordant in textile dyeing.
Sourced in Germany, United States, United Kingdom, India, Italy, France, Spain, Australia, China, Poland, Switzerland, Canada, Ireland, Japan, Singapore, Sao Tome and Principe, Malaysia, Brazil, Hungary, Chile, Belgium, Denmark, Macao, Mexico, Sweden, Indonesia, Romania, Czechia, Egypt, Austria, Portugal, Netherlands, Greece, Panama, Kenya, Finland, Israel, Hong Kong, New Zealand, Norway
Hydrochloric acid is a commonly used laboratory reagent. It is a clear, colorless, and highly corrosive liquid with a pungent odor. Hydrochloric acid is an aqueous solution of hydrogen chloride gas.
Sourced in United States, Germany, India, Mexico, China, Brazil, Singapore, Italy, United Kingdom
Ferric chloride hexahydrate is a chemical compound with the formula FeCl3·6H2O. It is a crystalline solid that is soluble in water and other polar solvents. Ferric chloride hexahydrate is commonly used as a coagulant in water treatment, as a mordant in dyeing, and in various other industrial applications.
Sourced in Germany, United States, United Kingdom, Italy, India, France, China, Australia, Spain, Canada, Switzerland, Japan, Brazil, Poland, Sao Tome and Principe, Singapore, Chile, Malaysia, Belgium, Macao, Mexico, Ireland, Sweden, Indonesia, Pakistan, Romania, Czechia, Denmark, Hungary, Egypt, Israel, Portugal, Taiwan, Province of China, Austria, Thailand
Ethanol is a clear, colorless liquid chemical compound commonly used in laboratory settings. It is a key component in various scientific applications, serving as a solvent, disinfectant, and fuel source. Ethanol has a molecular formula of C2H6O and a range of industrial and research uses.
Sourced in India, United States, Germany
Ferric nitrate is an inorganic chemical compound with the chemical formula Fe(NO3)3. It is a crystalline solid that is used in various laboratory and industrial applications.
Sourced in United States, Germany, India
Ferric nitrate nonahydrate is a chemical compound with the formula Fe(NO3)3·9H2O. It is a crystalline solid that is soluble in water. Ferric nitrate nonahydrate is commonly used as a laboratory reagent and in various industrial applications.
Sourced in United States, Germany, India, Italy, United Kingdom, Singapore, Switzerland, Spain, France, China, Canada, Japan, Australia
Sodium nitrate is an inorganic compound with the chemical formula NaNO3. It is a crystalline solid that is commonly used as a laboratory reagent and in various industrial applications.
Sourced in United States, Germany, India, United Kingdom, Italy, China, Poland, France, Spain, Sao Tome and Principe, Mexico, Brazil, Japan, Belgium, Singapore, Australia, Canada, Switzerland
Silver nitrate is a chemical compound with the formula AgNO3. It is a colorless, water-soluble salt that is used in various laboratory applications.
Sourced in United States, Germany, Italy, Spain, France, India, China, Poland, Australia, United Kingdom, Sao Tome and Principe, Brazil, Chile, Ireland, Canada, Singapore, Switzerland, Malaysia, Portugal, Mexico, Hungary, New Zealand, Belgium, Czechia, Macao, Hong Kong, Sweden, Argentina, Cameroon, Japan, Slovakia, Serbia
Gallic acid is a naturally occurring organic compound that can be used as a laboratory reagent. It is a white to light tan crystalline solid with the chemical formula C6H2(OH)3COOH. Gallic acid is commonly used in various analytical and research applications.

More about "Ferric nitrate"

Ferric nitrate, also known as iron(III) nitrate or Fe(NO3)3, is a versatile chemical compound with a wide range of applications in various industries and research fields.
This crystalline solid is soluble in water and is commonly used as an oxidizing agent, a food preservative, and a mordant in textile dyeing.
One of the key applications of ferric nitrate is in the production of steel, where it is used as a pickling agent to remove rust and scale from the surface of steel.
It is also employed in the treatment of water, where it can be used as a coagulant to remove impurities and suspended particles.
Ferric nitrate also finds use in the synthesis of other chemical compounds, such as sodium nitrate, silver nitrate, and gallic acid.
These compounds have diverse applications, ranging from food preservation to photography and pharmaceuticals.
Researchers in fields like materials science, environmental chemistry, and biochemistry often utilize ferric nitrate in their experiments and studies.
For instance, it can be used as a catalyst in the synthesis of nanomaterials or as a reagent in the analysis of environmental samples.
It is important to note that ferric nitrate should be handled with care, as it can be corrosive and may react with other chemicals.
Proper safety precautions, such as the use of personal protective equipment (PPE) and proper storage and disposal methods, should be observed when working with this compound.
Overall, ferric nitrate is a versatile and widely used chemical that plays a crucial role in various industries and research applications.
Its unique properties and diverse uses make it an essential component in many scientific and industrial processes.