Solid nickel nitrates

6 Group 15 compounds and complexes V.6.1 Nitrogen compounds and complexes V.6.1.1 Solid nickel nitrates 

This solid has been reported as a stable solid in the Ni(N03)2 - H2O system for temperatures below 270 K [34S1E/SCH]. The temperature for the equilibrium conversion of the nonahydrate to the hexahydrate in contact with saturated aqueous solution has not been well established. No values for Ni(N03)2 9H20(cr) are selected in the present review. 

The stable hydrate in equilibrium with a solution saturated in nickel nitrate at 298.15 K is Ni(N03)2-6H20(cr) [34SIE/SCH]. The water content of the commercially available solid tends to vary slightly. The solid can easily lose water on exposure to dry air [72AUF/CAR], [98ELM/GAB], but has also been reported to be slightly deliquescent in 

Calorimetric measurements were done for ratios of H20 Ni(N03)2 6H20 be- 

Goldberg et al. [79GOL/NUT], reviewed the available literature data, and provided tables of recommended values for the activity coefficients and osmotic coefficients for solutions of Ni(N03)2 in water at 298.15 K. However, there were no studies that allowed the tables to be extended to saturated solutions of Ni(N03)2 6.00H20(cr) at 

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NICKEL COMPOUNDS. In laboratory tests, aqueous solutions of nickel salts at ambient temperature caused varying degrees (from less than 1 mpy to more than 60 mpy) of attack of 1100 alloy depending upon the concentration and the specific compound. Most solutions of nickel compounds are inherently corrosive to aluminum alloys. In laboratory tests conducted under conditions of 100% relative humidity at ambient and 54°C (130°F) temperatures, solid nickel chloride was very corrosive to alloys 3003, 5154 and 6061 at both temperatures, solid nickelous acetate caused mild attack of these alloys at ambient temperature and was corrosive (-40 mpy) at 54°C (130°F). NITROGEN. N3. Solid nickelous nitrate caused mild attack at ambient... 

The Hp-zeolite sample was provided by Zeolyst International CP811E-75 (lot 1822-74 Si02/Al203 = 75, surface area -519 m g ). The Ni/Hp zeolite samples were prepared according to the following procedure First, 250 ml of a nickel nitrate aqueous solution (0.14M) was prepared. This solution was divided in two parts one part (40 ml) was used to dissolve urea at room temperature and the other part (210 ml) was used to make a suspension of 1.9 g of HP zeolite (pH = 2). Afterwards, the zeolite suspension was heated to 70 °C and mixed with the urea dissolution. The mixture was taken to 90 °C to start the deposition-precipitation of nickel onto the HP zeolite (Fig. 1). At the end of the chosen DP time (1 to 4 h), the suspension was cooled to 15-20 °C and filtered and the solid was washed three times with 20 ml of distilled hot water (50-60 °C). Finally, the samples were dried at 110 °C for 24 hours. Hereafter, the samples will be referred to as Ni/Hpi, Ni/Hp2, Ni/Hp3 and Ni/Hp4, where the numbers indicate the time in hours of deposition-precipitation used in the preparation of the sample. 

The mixed oxides CeNixOv were prepared by coprecipitation of hydroxides from mixtures of cerium and nickel nitrate using triethylamine (TEA) as precipitating agent, drying at 323 K and calcination in air at 773 K [22]. The metal loading has been verified by microanalysis. The solids will be called CeNix. 

Catalysts were prepared by incipient wetness impregnations using nickel nitrate and tetraamine-platinum (II) nitrate separate impregnations were made with air calcination at 593°C to decompose the nickel salts before platinum was added. After a second calcination, the powders were ball-milled with water to form a coating slurry which was used to coat Poramic (from W. R. Grace) monoliths slurry compositions were adjusted to give 10% solids pickup. The metal levels did not depend on support density. See Table II for final compositions. 

In this experiment you will start with two ionic solids, nickel(II) nitrate hexahydrate, Ni(NO3)2 6H2O, and potassium chloride, KCl. You will dissolve these solids in water and use either a temperature change or a concentration change by evaporation to crystallize relatively soluble salts from the aqueous solution. The solubilities at different temperatures of the four possible compounds involved are given in TABLE 19.1. 

Figure 3 depicts a schematic of how one can arrive at different meso-ciystal structures. Consideration of the coordination environment of the metal ions is crucial for predicting the nature of the resulting meso-ciystal. For example, a nanocomposite mesociystal may be obtained of phase-separated CuO and ZnO (Fig. 3b). This is due to the differing coordination environments of the copper ions (Cu in Jahn-Teller distorted octahedra in CuO) and the zinc ions (Zn in a tetrahedral environment in ZnO). On the other hand, a solid solution of Zno 2Nio sO is formed when zinc and nickel nitrates are employed as precursors, since the coordination environments are similar. One strength of this synthetic approach is the effective charge transfer which can occur in...

When nickel nitrate and sodium carbonate solutions are combined, solid nickel carbonate precipitates, leaving a solution of sodium nitrate. Write the conventional equation, total ionic equation, and net ionic equation for this reaction. 

The net ionic equation tells us that nickel ions from one solution combine with the carbonate ions from the other solution to form solid nickel carbonate. The sodium ions and nitrate ions that were in the separate solutions remain as ions in the combined solution. 

A piece of solid nickel metal is put into an aqueous solution of lead(It) nitrate. 

Nickel Catalyst, dry Nickel Cyanide Nickel Nitrate Nickel Nitrite Nicotine Nicotine Compound, liquid, n.o.s. 2881 1653 2725 2726 1654 3144 1655 37 53 35 35 55 55 Nitriles, toxic, n.o.s. (solid) Nitrites, inorganic, aqueous solutions, n.o.s. Nitrites, inorganic, n.o.s. Nitroanilines Nitroanisole 3276 3219 2627 1661 2730 55 35 35 55 55... 

In the preparation of nickel nitrate hydrazine [Ni(N03)2(N2H4)3] stoichiometric amounts of ammonium nitrate in hydrazine hydrate and nickel metal powder are allowed to react in the ratio of 2 3 1, respectively, at room temperature. The nickel metal dissolves exothermically with the evolution of hydrogen. The solid compound is obtained in 97% yield by the addition of alcohol. 

Figure 13. Specific 2-CP (open symbols) and 2,4-DCP (solid symbols) hydrodechlorination rate constant K) as a function of the average Ni particle diameter ( nO for reaction over Ni catalysts prepared via impregnation with nitrate (0,0), deposition-precipitation (A,A) and impregnation with nickel ethanediamine ( , ) r= 423K reaction data refer to aqueous solutions. (Reprinted from Reference [147], 2003, with permission from Royal Society of Chemistry).

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