Cobalt, Co2+

Most common oxidation states: +2, +3

M.P. 1495o

B.P. 2870o

Density 8.92 g/cm3

Characteristics: Steel-gray, hard, tough metal. Dissolves easily in HNO3 and also in dilute HCl and H2SO4.

Characteristic reactions of Co2+:

Aqueous Ammonia:

Excess concentrated ammonia reacts with cobalt(II) ion to form a metal complex ion, hexaamminecobalt(II) ion:

Co2+(aq) + 6NH3(aq) <==> [Co(NH3)6]2+

If an insufficient amount of ammonia is present, the reaction results instead in a precipitate of a basic salt, Co(OH)NO3 (blue) or Co(OH)2 (rose-red), which can co-precipitate with other metal ions that form hydroxide precipitates, causing complications when trying to separate metal ions:

Co2+(aq) + OH-(aq) + NO3-(aq) <==> Co(OH)NO3(s) 

Sodium Hydroxide:

Sodium hydroxide first precipitates the basic salt just described. This basic salt is insoluble in excess sodium hydroxide, but is soluble in acids. When heated, the basic salt hydrolyzes to form Co(OH)2. Cobalt(II) hydroxide is slowly oxidized by atmospheric oxygen to form brown Co(OH)3.

Ammonium Thiocyanate:

Addition of a concentrated solution of ammonium thiocyanate to solutions containing cobalt(II) ion results in a blue color, due to formation of a complex ion, tetraisothiocyanatocobaltate(II) ion:

Co2+(aq) + 4NCS-(aq) <==> [Co(NCS)4]2-(aq)

This complex ion is more stable in the presence of acetone; the blue color can be enhanced by addition of about an equal volume of acetone.

No Reaction:

Cl-, SO42-

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