Search results
Results from the WOW.Com Content Network
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 → ...
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 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.
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.
Nickel electroplating was developed in the first half of the 19th century, with notable experiments made by Golding Bird (1837) and nickel nitrate patent by Joseph Shore (1840). The first practical recipe, an aqueous solution of nickel and ammonium sulfates, was invented by Böttger in 1843 and was in use for 70 years. [8]
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]
Common salts of nickel, such as chloride, nitrate, and sulfate, dissolve in water to give green solutions of the metal aquo complex [Ni(H 2 O) 6] 2+. [45] The four halides form nickel compounds, which are solids with molecules with octahedral Ni centres. Nickel(II) chloride is most common, and its behavior is illustrative of the other halides.
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.