The molar solubility of a salt with the formula Ba3(PO4)2 is equal to 7.4 x 10-8 mol/L. Calculate the Ksp for Ba3(PO4)2. What is the concentration of X- required (molarity) in a solution that is 0.0016 M in M+ in order to cause a precipitate to begin to form? The Ksp for MX is 3. 44 x 10 -10
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The molar solubility of a salt with the formula Ba3(PO4)2 is equal to 7.4 x 10-8 mol/L. Calculate the Ksp for Ba3(PO4)2.
What is the concentration of X- required (molarity) in a solution that is 0.0016 M in M+ in order to cause a precipitate to begin to form? The Ksp for MX is 3. 44 x 10 -10
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