Iron(iii)sulfate pentahydrate

• CAS: 142906-29-4
• Catalog Number: ACM142906294
• Category: Main Products
• Molecular Weight: 489.95
• Molecular Formula: Fe₂H₁₀O₁₇S₃
• Synonyms: IRON(III) SULFATE PENTAHYDRATE;Sulfuric acid, iron(3+) salt (3:2), pentahydrate
• IUPAC Name: iron(3+);trisulfate;pentahydrate
• Canonical SMILES: O.O.O.O.O.[O-]S(=O)(=O)[O-].[O-]S(=O)(=O)[O-].[O-]S(=O)(=O)[O-].[Fe+3].[Fe+3]
• InChI Key: YHGPYBQVSJBGHH-UHFFFAOYSA-H
• Exact Mass: 489.77800

Case Study

Study on the Phase Diagram of Iron (III) Sulfate-Water System

Hennings, E., et al. Icarus, 2013, 226(1), 268-271.

This paper reported on the phase diagram of the iron (III) sulfate-water system and the role of sulfuric acid on this system. Experimentally, the freezing curve of the iron(III) sulfate-water system was calculated. The eutectic point was detected at 26.8 ± 0.5 °C with 36.16 ± 0.5 mass% Fe2(SO4)3.
A crystalline acidic iron (III) sulfate hydrate (Fe2(SO4)3·H2SO4·28H2O) was also found in the iron (III) sulfate-water-sulfuric acid ternary system, the iron salt phase with the highest water content ever observed.
The observations regarding crystallization behavior support the notion that concentrated salt solutions can remain in a super-cooled, metastable liquid state for more than a day. This is especially accurate for acidic concentrated iron(III) sulfate solutions, which can maintain their highly viscous, metastable liquid form for weeks.
This research enhances the understanding of physical and chemical processes such as deliquescence and viscous flows on the surface of Mars. Notably, the extensive stability range of acidic ferric sulfate (5-20% H2SO4) and the lowered freezing point within this mixed system provide new insights into the interpretation of mineral transformations on Mars.

Iron(III) Sulfate Pentahydrate for Optical Absorption Spectroscopy of Iron Ions in Aqueous Solutions and Hydrated Crystals

Fontana, I., A. Lauria, et al. Physica status solidi (b), 2007, 244(12), 4669-4677.

Absorption spectra of solutions in water and hydrated crystals containing Fe2+ and Fe3+ ions were examined up to 50,000 cm-1. For the first time, charge transfer transitions of two hydrated ions have been measured.
Preparation of samples
· This work prepared different solutions in water, with Fe2+ ions from various salts: FeSO4·7H2O, FeCl2·4H2O, Fe(NH4SO4)2·6H2O, and Fe(BF4)2·6H2O at various concentrations, to study a broad range of molar extinction coefficients.
· We made water solutions containing Fe3+ by dissolving commercial Fe2(SO4)3·5H2O, Fe(NH4) (SO4)2·12H2O, FeCl3·6H2O, and oxidized Fe(BF4)2 solution.
· Chose solutions of Fe(BF4)2 for selective oxidation from Fe2+ to Fe3+: multiple volumes of 0.3 M H2O2 were added to five identical solutions made by dissolving Fe(BF4)2·6H2O in water-soluble HBF4 solutions with pH ≈ 1. Hydrogen peroxide and Fe2+ undergo a stoichiometric, linear change from Fe2+ to Fe3+ in a redox reaction, while the acidic conditions prevent further oxidation of Fe2+ by water.
· The individual crystals of FeSO4·4H2O and FeCl2·4H2O were produced by evaporated supersaturated solutions at just above 30 °C. Clear, thick enough flakes were made.