Abstract
The solubility of Ba(NO3)2 and Sr(NO3)2 in HNO3 solutions at 25–95°C is characterized by the power dependence on the total concentration of the nitrate ion with the exponent for Ba(NO3)2 equal to −2 in ∼9 M HNO3 and −6 in more concentrated acid solutions. The latter exponent is also characteristic of the more soluble Sr(NO3)2 throughout the examined range of HNO3 concentrations. In strongly acidic solutions, Ba(NO3)2 coprecipitates with Sr(NO3)2. The solubility curve for Ba(NO3)2 in NH4(Na)NO3 solutions suggests formation of a double salt, whereas in UO2(NO3)2 solutions the dependence is the same as in HNO3 solutions.
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