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Cobalt(II) hydroxide or cobaltous hydroxide is the inorganic compound with the formula Co(OH) 2, consisting of divalent cobalt cations Co 2+ and hydroxide anions OH −. The pure compound, often called the "beta form" (β-Co(OH) 2) is a pink solid insoluble in water. [2] [3]
Cobalt(III) hydroxide or cobaltic hydroxide is a chemical compound with formula Co(OH) 3 or H 3 CoO 3. It is an ionic compound, with trivalent cobalt cations Co 3+ and hydroxyl anions OH −. The compound is known in two structurally different forms, "brownish-black" and "green".
Cobalt(II) nitrate exists in the anhydrous form and the hydrate form, of which the hexahydrate is the most common. Cobalt nitrate hexahydrate (Co(NO 3) 2 ·6H 2 O) is a red deliquescence crystal that is easily soluble in water, [12] and its molecule contains cobalt(II) hydrated ions ([Co(H 2 O) 6] 2+) and free nitrate ions. [13]
A part of the spent electrolyte enters the cobalt recovery circuit and is purified by the removal of iron, copper, nickel, and zinc prior to the precipitation of cobalt as its hydroxide. This is accomplished by the addition of more lime to raise the pH until the remaining copper precipitates. This copper is sent back to the copper circuit.
cobalt(II) molybdate: 13762–14–6 Co(NO 3) 2: cobalt(II) nitrate: 10141–05–6 Co(NO 3) 2 •6H 2 O: cobalt(II) nitrate hexahydrate: 10026–22–9 Co(NO 3) 3: cobalt(III) nitrate: 15520–84–0 CoO: cobalt(II) oxide: 1307–96–6 Co(OH) 2: cobalt(II) hydroxide: 21041–93–0 Co(OH) 3: cobalt(III) hydroxide: 1307–86–4 CoS: cobalt(II ...
The following chart shows the solubility of various ionic compounds in water at 1 atm pressure and room temperature (approx. 25 °C, 298.15 K). "Soluble" means the ionic compound doesn't precipitate, while "slightly soluble" and "insoluble" mean that a solid will precipitate; "slightly soluble" compounds like calcium sulfate may require heat to precipitate.
Cobalt(II) oxide is prepared by oxidation of cobalt powder with air or by thermal decomposition of cobalt(II) nitrate or the carbonate. [3] [4] Cobalt(II,III) oxide decomposes to cobalt(II) oxide at 950 °C: [7] 2 Co 3 O 4 → 6 CoO + O 2. It may also be prepared by precipitating the hydroxide, followed by thermal dehydration: [citation needed]
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