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| Cobalt Oxide (Co3O4)--Low Sodium Electronic Grade |
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| Assay (As Co) |
72.5% minimum |
| Sulfer |
40 ppm maximum |
| Chromium (Cr) |
20 ppm maximum |
| Calcium (Ca) |
3 ppm maximum |
| Copper (Cu) |
5 ppm maximum |
| Iron (Fe) |
100 ppm maximum |
| Magnesium (Mg) |
100 ppm maximum |
| Manganese (Mg) |
30 ppm maximum |
| Nickel (Ni) |
50 ppm maximum |
| Sodium (Na) |
50 ppm maximum |
| Zinc (Zn) |
3 ppm maximum |
| Average particle size, d50, in microns: 2.0 Typical |
Cobalt oxide is derived from cobalt, a ferromagnetic metal used in various
alloy forms for their heat resistance and magnetic properties. Cobalt is a fairly rare metal, comprising only 0.001
percent of the earth's crust, but is widely dispersed and commonly found and obtained in association with other
mining activities. It is found in ores of iron, nickel, copper, silver, manganese, zinc and arsenic. Alloys of
cobalt are useful for their stability at high temperatures. Superalloys are used near their melting points, where
steel would become too soft. Cobalt is used as a hardener (eg., for tools), for glass to metal seals (where its
low-expansion is an advantage), and precision springs (where its elasticity is an advantage),
Historical Background
Cobalt was isolated in 1735 by Georg Brandt, although compounds
containing cobalt have been used for thousands of years. It has been detected in ancient Egyptian statuettes and
ancient Chinese pottery. Cobalt was first named in the 16th century when found in arsenic ores, thought to be copper
ores, but which because of their arsenic content were poisonous.
Cobalt Oxide
Cobalt oxide is used in two covalent states, CoO and Co3O4. The latter form is the most commonly used
in manufacturing ceramics, glass and enamels, and in preparing catalysts and cobalt metal powder. In combination
with lead, cobalt oxide provides a brillian blue glaze on ceramics--which explains the scare about blue ceramics
several years ago. It is prepared by heating cobaltus hydroxide or oxide in air at 100 degrees centigrade. At lower
temperatures oxygen may be absorbed while leaving the crystal structure unchanged. At temperatures above 900 degrees
centigrade, oxygen is lost, and cobalt moxoxide is formed. Like the other oxides of cobalt, the tetroxide form
reduces to the metal when heated in hydrogen.
If you believe you have a use for cobalt oxide, contact us. We will be happy to discuss and help you implement
your application.
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