16919-98-5

Basic information

• Product Name: DihydrogenHexabromoIridate(IV)Hydrate
• Synonyms: DihydrogenHexabromoIridate(IV)Hydrate
• CAS NO: 16919-98-5
• Molecular Formula: Br6H4IrO
• Molecular Weight: 691.67216
• Mol File: 16919-98-5.mol
• Article Data: 3

Chemical Properties

• Appearance: /
• CAS DataBase Reference: DihydrogenHexabromoIridate(IV)Hydrate(CAS DataBase Reference)
• NIST Chemistry Reference: DihydrogenHexabromoIridate(IV)Hydrate(16919-98-5)
• EPA Substance Registry System: DihydrogenHexabromoIridate(IV)Hydrate(16919-98-5)

Safety Data

• Hazardous Substances Data: 16919-98-5(Hazardous Substances Data)

Usage

General Description

DihydrogenHexabromoIridate(IV)Hydrate is a chemical compound with the formula H2[IrBr6]·xH2O, where x is the number of water molecules present. It is a hydrated form of dihydrogenhexabromoiridate(IV) and is used in various chemical and industrial applications. DihydrogenHexabromoIridate(IV)Hydrate is composed of dihydrogen cations, hexabromoiridate(IV) anions, and water molecules. It is a dark red solid at room temperature and is highly soluble in water. DihydrogenHexabromoIridate(IV)Hydrate has potential uses in catalysis, chemical synthesis, and as a reagent in organic chemistry.

Upstream product

• 111018-28-1 trans-tetrabromobis(pyridine)iridium(IV) 
• 18400-15-2 [IrBr₆]^(3-) 
• 7782-77-6 cis-nitrous acid 

Relevant articles and documents

Reduction potentials determination of some biochemically important free radicals. Pulse radiolysis and electrochemical methods

In this review reduction potentials of unstable species is described.Both fast kinetics and electrochemical techniques are presented.Examples involving the determination of the reduction potentials of free radicals from amino-acids, peptides and nucleobases are discussed.

Kinetics and equilibria for reactions of the hexachloroiridate redox couple in nitrous acid

The equilibria, kinetics, and mechanisms of the reactions of the IrCl62-/3- redox couple in nitrous acid have been investigated in aqueous solution at 25.0°C in nitric and perchloric acid media by conventional and stopped-flow spectrophotometry. In 1 M HClO4, when IrCl63- and HNO2 are mixed, the equilibrium HNO2 + H+ + IrCl63- ? NO + H2O + IrCl62- is established in a few milliseconds, with +d[IrCl62-]/dt = kf[H+][HNO2][IrCl63-] - kr[NO][IrCl62-], where kf = 1.8 × 104 M-2 s-1 and kr = 1.4 × 106 M-1 s-1. At high [HNO2], this reaction precedes a slow loss of IrCl62- that is due to formation of NO3-. In 1 M NO3- with [HNO2] > [IrCl63-] the rapid equilibrium is followed by zero-order formation of IrCl62-, and with [IrCl63-] > [HNO2] the process is autocatalytic. When IrCl62- is mixed with N(III) at pH ≥2, IrCl62- is consumed with rates that increase with acidity; at pH 62- is only partially consumed. All of these phenomena have been accurately simulated by numerical integration of the set of differential equations that arise from kf and kr as defined above and several previously established processes intrinsic to nitrous acid/nitric acid mixtures. The kf step is interpreted as rate-limiting diffusion-controlled electron transfer from IrCl63- to NO+. The reaction of NO2 with [Fe(TMP)3]2+ (TMP = 3,4,7,8-tetramethylphenanihroline), observed directly by pulse radiolysis, has a rate constant of 1.0 × 107 M-1 s-1; this rate constant, in conjunction with the results of a prior study of the reaction of NO2- with [Fe(TMP)3]3+, has confirmed the choice of thermodynamic data used to analyze the IrCl62-/3- reactions.