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Aqueous solutions of nickel sulfate react with sodium carbonate to precipitate nickel carbonate, a precursor to nickel-based catalysts and pigments. [6] Addition of ammonium sulfate to concentrated aqueous solutions of nickel sulfate precipitates Ni(NH 4) 2 (SO 4) 2 ·6H 2 O. This blue-coloured solid is analogous to Mohr's salt, Fe(NH 4) 2 (SO ...
Heating nickel sulfate dehydrates it, and then 700° it loses sulfur trioxide, sulfur dioxide and oxygen. Nickel sulfite can be formed by bubbling sulfur dioxide through nickel carbonate suspended in water. A solution is formed that slowly loses sulfur dioxide, and which crystallises nickel sulfite hexahydrate.
One commercial method for extraction of nickel from its sulfide ores involves the sulfate salt of [Ni(NH 3) 6] 2+. In this process, the partially purified ore is treated with air and ammonia as described with this simplified equation: [3] NiS + 2 O 2 + 6 NH 3 → [Ni(NH 3) 6]SO 4
As a mineral the ammonium nickel salt, (NH 4) 2 Ni(SO 4) 2 · 6 H 2 O, can be called nickelboussingaultite. [2] With sodium, the double sulfate is nickelblödite Na 2 Ni(SO 4) 2 · 4 H 2 O from the blödite family. Nickel can be substituted by other divalent metals of similar sized to make mixtures that crystallise in the same form. [3]
The first periodatonickalates discovered were sodium nickel periodate (NaNiIO 6 ·0.5H 2 O) and potassium nickel periodate (KNiIO 6 ·0.5H 2 O). P. Ray and B. Sarma obtained these dark purple double salts in 1949, mixing nickel sulfate with potassium or sodium periodate and (as oxidant) a boiling aqueous solution of an alkali persulfate ...
It can be made by oxidising nickel nitrate in a cold alkaline solution with bromine. A mixed oxidation state hydroxide Ni 3 O 2 (OH) 4 is made if oxidation happens in a hot alkaline solution. A Ni 4+ hydroxide: nickel peroxide hydrate NiO 2 · H 2 O, can be made by oxidising with alkaline peroxide. It is black, and unstable and oxidises water.
Nickel maleate can be made from maleic acid and nickel carbonate in boiling water. A dihydrate crystallises from the water solution. [11] Nickel fumarate prepared from fumaric acid and nickel carbonate is pale green as a tetrahydrate, and mustard coloured as an anhydride. It decomposes when heated to 300° to 340° in vacuum.
Nickel carbonates are hydrolyzed upon contact with aqueous acids to give solutions containing the ion [Ni(H 2 O) 6] 2+, liberating water and carbon dioxide in the process. Calcining (heating to drive off CO 2 and water) of these carbonates gives nickel(II) oxide: NiCO 3 → NiO + CO 2. The nature of the resulting oxide depends on the nature of ...