Rubidium hydrogen sulfate

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Template:Chembox Rubidium hydrogen sulfate is the rubidium salt of sulfuric acid. It has the formula RbHSO4.

Synthesis

It may be synthesised with water and a stoichiometric amount of rubidium disulfate. Reaction takes place where there is no humidity: [1]

There is an other method of creation. It is similar to the synthesis of sodium sulfate and potassium sulfate. For this reaction there need for rubidium chloride and a little bit warm sulfuric acid. Some hydrogen chloride is also produced during the reaction.

Properties

It is a hydroscopic compound. It has a monocline crystal structure, its structure is P21/n. Parameters of the bonding modes: a = 1440 pm, b = 462,2 pm, c = 1436 pm and β = 118,0°. Its crystals are isomorphs with ammonium hydrogen sulfate crystals. [2]

Its standard enthalpy is −1166 kJ/mol [3] During its dissolution in water there is 15.62 kJ/mol energy produced. [4]

After warming up it resolves to rubidium disulfate and water:[5]

Like potassium and caesium, rubidium has an other hydrogene sulfate compound as well: Rb3H(SO4)2.

Sources

  1. S. B. Rasmussen, H. Hamma, K. M. Eriksen, G. Hatem, M. Gaune-Escard, R. Fehrmann: "Physico-chemical properties and transition metal complex formation in alkali pyrosulfate and hydrogen sulfate melts". VII International Conference on Molten Slags Fluxes and Salts, The South African Institute of Mining and Metallurgy, 2004. Volltext (PDF; 661 kB)
  2. J. P. Ashmore, H. E. Petch: "The Structure of RbHSO4 in its Paraelectric Phase" in Can. J. Phys 1975, 53(24), S. 2694-2702. Template:Hide in printTemplate:Only in print
  3. L. A. Cowan, R. M. Morcos, N. Hatada, A. Navrotsky, S. M. Haile: "High temperature properties of Rb3H(SO4)2 at ambient pressure: Absence of a polymorphic, superprotonic transition" in Solid State Ionics 2008, 179, S. 305-313. Volltext (PDF; 837 kB)
  4. M. de Forcrand: "Sur les chlorures et sulfates de rubidium et de caesium" in Compt. Rend. Hebd. 1906, 143, S. 98. Volltext
  5. R. Abegg, F. Auerbach: "Handbuch der anorganischen Chemie". Verlag S. Hirzel, Bd. 2, 1908. S. 432.Volltext