Explicit algebraic stress model

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:

$\mathrm{R}{\mathrm{b}}_{\mathrm{2}}{\mathrm{S}}_{\mathrm{2}}{\mathrm{O}}_{\mathrm{7}}+{\mathrm{H}}_{\mathrm{2}}\mathrm{O}\mathrm{⟶}\mathrm{2}\mathrm{R}\mathrm{b}\mathrm{H}\mathrm{S}{\mathrm{O}}_{\mathrm{4}}$

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.

${\mathrm{H}}_{\mathrm{2}}\mathrm{S}{\mathrm{O}}_{\mathrm{4}}+\mathrm{R}\mathrm{b}\mathrm{C}\mathrm{l}\mathrm{⟶}\mathrm{R}\mathrm{b}\mathrm{H}\mathrm{S}{\mathrm{O}}_{\mathrm{4}}+\mathrm{H}\mathrm{C}\mathrm{l}$

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.

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

After warming up it resolves to rubidium disulfate and water:

$\mathrm{2}\mathrm{R}\mathrm{b}\mathrm{H}\mathrm{S}{\mathrm{O}}_{\mathrm{4}}\mathrm{⟶}\mathrm{R}{\mathrm{b}}_{\mathrm{2}}{\mathrm{S}}_{\mathrm{2}}{\mathrm{O}}_{\mathrm{7}}+{\mathrm{H}}_{\mathrm{2}}\mathrm{O}$

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

Sources

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