Chromium(III) sulphate solution 50%

Catalog Number	ACEP10101538
CAS Number	10101-53-8
Structure
Molecular Formula	Cr2(SO4)3
Concentration	50%

Case Study

Chromium Sulfate [Cr₂(SO₄)₃] Solution for Cr Nanotube Deposition

Anaee, R. A., & Hassan, A. R. (2018). Journal of University of Babylon for Engineering Sciences, 26(2), 152-159.

In this study, Cr nanotubes were prepared via electrochemical deposition using anodic aluminum oxide (AAO) as a template.
Preparation of AAO Template
Aluminum sheets with a thickness of 0.5 mm were cut into circular pieces with a diameter of 20 mm to prepare the AAO templates for nanotube deposition. The aluminum samples were cleaned with acetone and treated with 3M NaOH to activate the aluminum surface, followed by electrochemical polishing.
A 0.3 M oxalic acid solution, prepared in distilled water, was used as the anodization electrolyte. Anodization was performed in two steps.
First Step: The aluminum sample was connected to the positive terminal of a power supply as the anode, and a 316L stainless steel rod served as the cathode. A voltage of 30 V was applied in the electrochemical cell for 8 hours at room temperature. The sample was then treated with a mixture of H₃PO₄ and H₂Cr₂O₄ at 60°C for 1 hour to open the pores.
Second Step: Anodization was repeated in the same electrolyte for 6 hours. The sample was then rinsed with deionized water and ethanol, followed by soaking in acetone at 60°C for 1 hour to remove residual aluminum oxide.
Deposition of Cr Nanotubes
Cr nanotubes were deposited using an electrolyte containing 0.5 M chromium sulfate [Cr₂(SO₄)₃] and 30 g/L boric acid. The AAO template served as the cathode in the electrochemical cell, while a chromium rod was used as the anode. A deposition voltage of 10 V was applied for 15 minutes.

Effect of Cr₂(SO₄)₃ Concentration on the Oxidation Rate Constant of Cr₂(SO₄)₃

Amin, N. K., et al. Environmental Technology 43.16 (2022): 2405-2417.

The anodic oxidation of Cr₂(SO₄)₃ was investigated in an air-bubbled separated parallel-plate electrolytic cell. It was found that the oxidation rate constant of Cr₂(SO₄)₃ increased with rising current density and Cr₂(SO₄)₃ concentration.
The data indicated that the total rate constant decreased with increasing Cr₂(SO₄)₃ concentration, regardless of the superficial gas velocity. Moreover, at higher Cr₂(SO₄)₃ concentrations (e.g., 0.25 and 0.5 M), the total rate constant was unaffected by gas bubbling. In contrast, at lower Cr₂(SO₄)₃ concentrations (e.g., 0.05 and 0.01 M), the total rate constant increased with the superficial gas velocity, with the increase being more pronounced at lower Cr₂(SO₄)₃ concentrations.
These results suggest that the anodic oxidation of Cr₂(SO₄)₃ is chemically controlled at high concentrations (>0.05 M). However, when the concentration drops below 0.05 M, diffusion begins to play an increasingly significant role in determining the reaction rate.

Electrolytic Alloying of Iron-Chromium in FeCl₂-Cr₂(SO₄)₃ Electrolyte During Coating Deposition

Sinelnikov, A. F., et al. IOP Conference Series: Materials Science and Engineering. Vol. 1159. No. 1. IOP Publishing, 2021.

This paper presents the research results on the electro-reduction process of iron-chromium alloys in sulfate-chloride electrolytes, focusing on the effects of electrolyte composition and the electrolysis process on kinetics, alloy current efficiency, and the physical and mechanical properties of the coatings.
The figure shows the relationship between electrode potential and current density. In the chromium sulfate electrolyte, the sulfate concentration was varied from 25 to 100 g/l, with a step interval of 25 g/l (represented by curves 1-4). In the iron chloride electrolyte, the iron chloride concentration ranged from 100 to 200 g/l, with intervals of 50 g/l (represented by curves 5-7). Additionally, a mixed electrolyte with 150 g/l FeCl₂ and 50 g/l Cr₂(SO₄)₃ was used (curve 8). The study was conducted at a temperature of 40°C and pH=0.6.
The analysis of the figure shows that the potential of the chromium electrode (curves 1-4) has shifted to the negative region relative to its equilibrium value (φ (for Cr³⁺) = - (0.35 ÷ 0.45) mV). In highly acidic environments, the equilibrium potential of the platinum electrode for chromium (Δϕₑqᵤᵢˡ (Cr³⁺/Cr) = 50 mV) is essentially independent of the concentration of metal cations or current density. Simple calculations show that the polarization value of the electrode is Δϕₚᵒˡ (for Cr³⁺) = 85 ÷ 95 mV. The iron electrode potential (curves 5-7) is more positive compared to its equilibrium value (φ (for Fe²⁺) = - (220 ÷ 260) mV, in highly acidic media Δϕₑqᵤᵢˡ (for Fe²⁺/Fe) = -320 mV), with notable fluctuations in potential depending on changes in Fe²⁺ concentration and current density. The polarization of the iron electrode Δϕₚᵒˡ (for Fe²⁺) is - (60 ÷ 100) mV, which is closer to the opposite sign of the chromium polarization value, indicating the presence of a common factor where the metal potential deviates from its equilibrium value.
When both iron and chromium ions are present in the mixed electrolyte (curve 8), the electrode potential shifts further toward the positive direction, indicating their mutual interaction and participation in the electrolysis process. The electrode potential shows minimal response to changes in current density.

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