Arsenic, As3+
Most common oxidation states: +3, +5
Characteristics: Gray, very brittle substance; sublimes at 615o. Combines readily with sulfur and oxygen at high temperatures.
Characteristic reactions of As3+:
Hydrogen Sulfide:
In slightly acid solution, yellow As2S3 forms on addition of H2S:
2As3+(aq) + 3H2S(aq) <==> As2S3(s) + 6H+(aq)
Hydrogen sulfide causes no precipitation from neutral or alkaline solutions. The precipitate is soluble in concentrated HNO3 or in ammoniacal H2O2:
As2S3(s) + 8H+(aq) + 2NO3-(aq) <==> 2As3+(aq) + 3S(s) + 2NO(g) + 4H2O(l)
As2S3(s) + 14H2O2(aq) + 12NH3(aq) <==> 2AsO43-(aq) + 3SO42-(aq) + 8H2O(l) + 12NH4+(aq)
The precipitate is insoluble in dilute, nonoxidizing acids such as HCl.
Silver Ion:
Silver ion will precipitate yellow silver arsenite from neutral or slightly basic solution:
3Ag+(aq) + AsO33-(aq) <==> Ag3AsO3(s)
It is insoluble in water, but soluble in aqueous ammonia and in acids.
Oxidizing Agents:
Oxidizing agents readily oxidize arsenites (+3) to arsenates (+5) in alkaline or neutral solutions:
2Cu(OH)2(s) + AsO33-(aq) <==> Cu2O(s) (red) + AsO43-(aq) + 2H2O(l)
No Reaction:
Cl-, SO42-, NH3(aq), OH-