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Rubidium acetate is a rubidium salt that is the result of reacting rubidium metal, rubidium carbonate, or rubidium hydroxide with acetic acid. It is soluble in water like other acetates . [ 2 ]
Alkali metal nitrates are chemical compounds consisting of an alkali metal (lithium, sodium, potassium, rubidium and caesium) and the nitrate ion. Only two are of major commercial value, the sodium and potassium salts. [1] They are white, water-soluble salts with melting points ranging from 255 °C (LiNO 3) to 414 °C (CsNO
rubidium bromide: 7789–39–1 RbC 2 H 3 O 2: rubidium acetate: 563–67–7 RbC 5 H 7 O 2: rubidium acetylacetonate: 66169–93–5 RbCl: rubidium chloride: 7791–11–9 RbF: rubidium fluoride: 13446–74–7 RbH: rubidium hydride: 13446–75–8 RbI: rubidium iodide: 7790–29–6 RbIO 3: rubidium iodate: 13446–76–9 RbIO 4: rubidium ...
Only one alkali metal nitride is stable, the purple-reddish lithium nitride (Li 3 N), which forms when lithium burns in an atmosphere of N 2. [7] Sodium nitride and potassium nitride has been generated, but remains a laboratory curiosity. The nitrides of the alkaline earth metals that have the formula M 3 N 2 are however numerous.
acetate ion: 71-50-1 CH 3 COOCHCH 2: vinyl acetate: 108-05-4 CH 3 COOCH 2 C 6 H 5: benzyl acetate: 140-11-4 CH 3 COO(CH 2) 2 CH(CH 3) 2: isoamyl acetate: 123-92-2 CH 3 COOH: acetic acid ethanoic acid: 64-19-7 CH 3 COONa: sodium acetate: 127-09-3 CH 3 COOK: potassium acetate: 127-08-2 CH 3 COORb: rubidium acetate: 563-67-7 CH 3 COOCs: caesium ...
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.
An acetate is a salt formed by the combination of acetic acid with a base (e.g. alkaline, earthy, metallic, nonmetallic or radical base). "Acetate" also describes the conjugate base or ion (specifically, the negatively charged ion called an anion) typically found in aqueous solution and written with the chemical formula C 2 H 3 O − 2.
In at least one study, rubidium azide was produced by the reaction between butyl nitrite, hydrazine monohydrate, and rubidium hydroxide in the presence of ethanol: C 4 H 9 ONO + N 2 H 4 ·H 2 O + RbOH → RbN 3 + C 4 H 9 OH + 3 H 2 O. This formula is typically used to synthesize potassium azide from caustic potash. [5]