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Bit of a mixup here.
So, find the maximum F- ions present in a 0.032 M Ba(NO3)2 where the ksp of BaF2 = 3.2x10^-8.
So I first write the Ksp expression which is Ksp= [Ba2+] * [F-]^2. So I solve for F- concentration by letting [Ba2+] equal 0.032M. In a quiz from chad's videos the concentration was not multiplied by 2, since BaF2 dissociates into Ba and 2F-? Why is it not multiplied by 2 because in DAT destroyer 2012 #122 the final calcium concentration is multiplied by 3.
On a side note, I understand if I am solving more molar solubility the expression I use is ksp=4x^3
So, find the maximum F- ions present in a 0.032 M Ba(NO3)2 where the ksp of BaF2 = 3.2x10^-8.
So I first write the Ksp expression which is Ksp= [Ba2+] * [F-]^2. So I solve for F- concentration by letting [Ba2+] equal 0.032M. In a quiz from chad's videos the concentration was not multiplied by 2, since BaF2 dissociates into Ba and 2F-? Why is it not multiplied by 2 because in DAT destroyer 2012 #122 the final calcium concentration is multiplied by 3.
On a side note, I understand if I am solving more molar solubility the expression I use is ksp=4x^3