Chemical elements
    Physical Properties
    Chemical Properties
      Uranium Difluoride
      Uranium Tetrafluoride
      Uranous Oxyfluoride
      Uranium Hexafluoride
      Uranyl Fluoride
      Uranium Trichloride
      Uranium Tetrachloride
      Uranium Pentachloride
      Uranyl Chloride
      Uranyl Chlorate
      Uranyl Perchlorate
      Uranium Tetrabromide
      Uranyl Bromide
      Uranium Tetra-iodide
      Uranyl Iodide
      Uranyl Iodate
      Uranous Oxide
      Uranous Hydroxide
      Uranium Pentoxide
      Urano-uranic Oxide
      Uranium Trioxide
      Ammonium Diuranate
      Ammonium Hexa-uranate
      Hydroxylamine Uranate
      Hydroxylamine Potassio-uranate
      Barium Uranate
      Barium Diuranate
      Bismuth Uranate
      Iron Uranate
      Lithium Uranate
      Potassium Uranate
      Potassium Diuranate
      Potassium Tetra-uranate
      Potassium Hexa-uranate
      Rubidium Uranate
      Silver Diuranate
      Sodium Uranate
      Sodium Diuranate
      Sodium Triuranate
      Sodium Penta-uranate
      Strontium Uranate
      Zinc Uranate
      Peruranic acid
      Ammonium Peruranate
      Barium Peruranates
      Lithium Peruranate
      Nickel Peruranate
      Potassium Peruranate
      Sodium Peruranates
      Uranium Monosulphide
      Uranium Sesquisulphide
      Uranium Disulphide
      Uranium Oxysulphide
      Uranyl Sulphide
      Uranium Sulphite
      Uranyl Sulphite
      Complex Uranyl Sulphites
      Uranium Sulphate
      Uranium Dithionates
      Uranyl Sulphate
      Uranyl Pyrosulphate
      Uranyl Thiosulphate
      Uranyl Dithionate
      Uranium Sesquiselenide
      Uranium Diselenide
      Uranyl Selenide
      Uranyl Selenite
      Uranyl Selenate
      Uranium Telluride
      Uranium Nitrides
      Uranous Nitrate
      Uranyl Nitrate
      Uranium Monophosphide
      Uranous Phosphide
      Uranyl Hypophosphite
      Uranyl Phosphite
      Uranous Phosphates
      Uranyl Phosphates
      Complex Uranyl Phosphates
      Uranyl Aminophosphates
      Uranous Arsenide
      Uranyl Metarsenite
      Uranous Arsenate
      Uranyl Arsenates
      Complex Uranyl Arsenates
      Uranous Antimonide
      Uranous Antimonate
      Uranium Carbide
      Complex Uranyl Carbonates
      Ammonium Uranyl Carbonate
      Calcium Uranyl Carbonate
      Potassium Uranyl Carbonate
      Sodium Uranyl Carbonate
      Thallium Uranyl Carbonate
      Potassium Uranyl Ferrocyanide
      Uranyl Platinocyanide
      Uranyl Cyanate
      Uranyl Thiocyanate
      Uranium Silicide
      Uranium Boride
      Uranyl Perborate
    PDB 1anv-3pu4

Uranyl Sulphate, UO2SO4

Uranyl Sulphate, UO2SO4, is obtained as amber-yellow non- fluorescent crystals when uranyl hydroxide is dissolved in concentrated sulphuric acid and the solution is evaporated; or when either of its hydrates is heated to 300° C. The trihydrate, UO2SO4.3H2O, crystallises from a solution of uranyl hydroxide in dilute sulphuric acid; or it may be obtained by dissolving urano-uranic oxide in concentrated sulphuric acid, diluting the solution, and boiling with nitric acid in order to oxidise the uranous salt present; or by triturating potassium hydrogen sulphate with uranyl hydroxide, taking up with water, and concentrating the solution. It forms yellowish-green prismatic crystals, which under the microscope show a beautiful fluorescence. They have density at 16.5° C. = 3.280. In the air the crystals slowly effloresce; on heating they lose more water, and at 115° C. yield the monohydrate. This hydrate, in moist air, takes up water again and reforms the trihydrate.

Uranyl sulphate is readily soluble in water, but accurate solubility determinations have not been made. According to O. de Coninck, the trihydrate dissolves in about twenty times its weight of water at ordinary temperature, and the solubility decreases with rise in temperature. The heat of solution at 18° to 20° C. is +5100 calories.

The equivalent conductivities of solutions containing ½UO2SO4 in v litres at 25° C. are as follows:

v =481632641282565121024
Λ =17.120.525.532.041.553.267.785.2103.4

The difference between Λ32 and Λ1024, 71.4, is, as in the case of uranyl chloride and nitrate, unusually high, probably because dissociation takes place in stages. If the solutions are kept for some time, the conductivity increases owing to the increase in hydrogen ions due to hydrolysis. The migration velocity of the uranyl ion at 25° C. is, according to Dittrich, 56. The conductivities at higher temperatures have been determined as follows (for ½UO2SO4 in v litres):

v =81664256
Λ at 35° C. =48.261.982.9117.2
Λ at 50°C. =59.169.898.9141.3
Λ at 65° C. =70.287.0114.3162.2

Freezing-point determinations show that uranyl sulphate dissociates in dilute solutions to a much less extent than the chloride or nitrate.

Solutions of uranyl sulphate are fairly stable in diffused daylight, even in presence of alcohol, but readily undergo reduction when placed in direct sunlight or in ultra-violet light.

Uranyl acid sulphate

Uranyl acid sulphate, UO2SO4.H2SO4, is obtained in fine yellow fluorescent crystals when a solution of uranyl sulphate in moderately concentrated sulphuric acid is evaporated at 200° C. It is very deliquescent and readily soluble in water. By evaporating at 60° C. a solution containing uranyl sulphate (1 molecule) and sulphuric acid (5 molecules), similar crystals of composition 2UO2SO4.H2SO4.5H2O are obtained.

Basic uranyl sulphates of composition 3U2O3.SO3.2H2O and 4U2O3. SO3.7H2O have been obtained by evaporating at 250° C. solutions of uranyl sulphate containing 3 and 15 per cent, respectively. The former yields citron-yellow, and the latter greyish-yellow, microscopic crystals.

Ammonio-uranyl Sulphates

Uranyl sulphate forms yellow addition compounds with ammonia, of composition UO2SO4.xNH3, where x = 2, 3, or 4, the colour of which deepens with increasing ammonia content.

Complex uranyl sulphates, of composition

R2SO4.UO2SO4.2H2O, (R = NH4, K, Rb),
R2SO4.UO2SO4.3H2O, (R = NH4, Cs, Na, K, Tl),

have been described. They are usually obtained from a solution of the diuranate in sulphuric acid, or by crystallisation in vacuo of solutions of the mixed salts.

The potassium salt

The potassium salt, K2SO4.UO2SO4.2H2O, may also be prepared by triturating uranyl hydroxide with potassium hydrogen sulphate, taking up the mixture with water, and evaporating the solution. It was in this salt that Becquerel first discovered radioactivity. It yields yellow fluorescent crystals of density at 191° C.=3.363. The crystals, like those of the corresponding ammonium and rubidium salts, belong to the monoclinic system. The salt is stable towards water. When heated, it becomes anhydrous at 120° C.

The double salt

The double salt, 2K2SO4.UO2SO4, is obtained by dissolving uranyl sulphate and excess of potassium sulphate in hot water, and crystallising from the hot solution. At temperatures below 80° C. the salt is decomposed by water thus:

2K2SO4.UO2SO4K2SO4.UO2SO4 + K2SO4.

A double salt with hydroxylamine sulphate, (NH2OH)2H2SO4.2UO2SO4.5H2O, and an ethylenediammonium uranyl sulphate, C2H4(NH2)2H2SO4.UO2SO4.4H2O, have been prepared.
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