The ratio of uranyl ions to complexes in the sulphate leaching solution of the uranium ore depends on the concentration of sulfate in the leachate. When the sulfate concentration is low, the uranium in the leachate is mainly present as uranyl cation UO2+ and neutral complex UO2SO4. As the sulfate concentration in the leaching stain increases, the proportion of uranyl sulfate anion in the solution increases. When the uranium oxide ore is leached with dilute sulfuric acid, the hexavalent uranium in the ore is easily dissolved by sulfuric acid, and the dissolution reaction is:
UO3+H2SO4=UO2SO4+H2O (1)
Uranium usually enters the solution in the form of uranyl ions (UO22+) and further reacts with sulfate to form a di(or tri)sulfate complex:
UO22++nSO42-=UO2(SO4)n2-2n(2)
K= 
The stability constant of the UO2(SO4)n2-2n complex is divided into the following three cases depending on the leaching conditions: when n=l K1=50 n=2 K2=350 n=3 K3=2500 from the reaction (1) and 2) It can be seen that uranium in the sulfuric acid leaching solution is neutral uranyl sulfate (UO2SO4), negative divalent sulfuric acid uranyl complex anion [UO2(SO4)2]2- and negative tetravalent uranyl sulfonate anion [ UO2(SO4)3]4- exists. The reaction formula also shows that increasing the sulfate concentration of the leachate is beneficial to the formation of uranyl complex anions and the reduction of uranyl cations and neutral uranyl sulfate molecules in the solution.
When leaching with sulfuric acid, in addition to the uranium in the ore being dissolved out into the solution, other impurity components are also dissolved to varying degrees, and they are present in the leachate in different forms. For example, quartz can be partially dissolved to form silicic acid SiO2+H2O=H2SiO3 (3) Silicic acid is present in a colloidal form in solution.
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