What is the molar solubility of barium phosphate (Ba3(PO4)2) at a temperature where the Ksp is (6.00x10^-37) (not at 25°C)?

The molar solubility of the barium salt is obtained as  1.29 * 10^-19 M.What is the solubility?We know that the solubility has to do with the amount of the solute that is able to dissolve in a solvent at a particular temperature. As such, it is clear that the solubility depends on the temperature of the solution.We know that the Ksp can be gotten from the expression of the Ksp as follows;Ksp = [3x]^3 [2x]^2Ksp = 9x^3 * 4x^2Ksp = 36 * x^5Ksp = 36x^5x =[tex]\sqrt[5]{\frac{KSP}{36} }[/tex]x = [tex]\sqrt[5]{6.00x10^-37} /36[/tex]x = 1.29 * 10^-19 MLearn more about molar solubility:https://brainly.com/question/28170449#SPJ1