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Nickel nitrate is the inorganic compound Ni(NO 3) 2 or any hydrate thereof. In the hexahydrate, the nitrate anions are not bonded to nickel. Other hydrates have also been reported: Ni(NO 3) 2. 9H 2 O, Ni(NO 3) 2. 4H 2 O, and Ni(NO 3) 2. 2H 2 O. [3] It is prepared by the reaction of nickel oxide with nitric acid: NiO + 2 HNO 3 + 5 H 2 O → Ni ...
Be(NO 3) 2: beryllium nitrate: 13597–99–4 Be(NO 3) 2 •4H 2 O: beryllium nitrate tetrahydrate: 13510–48–0 Be(NO 3) 2 •3H 2 O: beryllium nitrate trihydrate: 7787–55–5 BeO: beryllium oxide: 1304–56–9 Be(OH) 2: beryllium hydroxide: 13327–32–7 BeS: beryllium sulfide: 13598–22–6 BeSO 4: beryllium sulfate: 13510–49–1 ...
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(II) chloride (or just nickel chloride) is the chemical compound NiCl 2. The anhydrous salt is yellow, but the more familiar hydrate NiCl 2 ·6H 2 O is green. Nickel(II) chloride, in various forms, is the most important source of nickel for chemical synthesis. The nickel chlorides are deliquescent, absorbing moisture from the air to form ...
Nickel nitrate commonly crystallises with six water molecules, [1] but can also be anhydrous, or with two, four or nine waters. [11] triphenylphosphine oxide nickel nitrate [(C 6 H 6) 3 PO] 2 Ni(NO 3) 2 is non ionic, with nitrato as a ligand. It can be made from nickel perchlorate. It is yellow and melts at 266 °C. [12]
Nickel terephthalate can be made by a double decomposition of sodium terephthalate and nickel nitrate. Nickel terephthalate precipitates. Its solubility is 0.38 g/100g water at 25 °C. In ammonium hydroxide a violet solution forms. Boiling acetic acid converts the nickel to nickel acetate.
Nickel thorium nitrate has formula NiTh(NO 3) 6 · 8 H 2 O. Nickel atoms can be substituted by other ions with radius 0.69 to 0.83 Å. The nitrates are coordinated on the thorium atom and the water to the nickel. Enthalp of solution of the octahydrate is 7 kJ/mol. Enthalpy of formation is -4360 kJ/mol.
Evaporating the resulting solution yields hydrated neodymium(III) nitrate, where the hexahydrate form is the most common. Heating the hexahydrate further will obtain the anhydrous form. Reacting neodymium(III) chloride with sodium arsenate in solution would obtain neodymium(III) arsenate , [ 10 ] which is a faint pink powder that is insoluble ...