For this problem, we have to calculate the molar solubility of barium fluoride ( BaF2 ) in water
Recall that Ksp is an equilibrium constant related to slightly soluble ionic compounds.
The dissociation of slightly soluble PbI2 in solution is as follows:
BaF2(s) ⇌ Ba2+(aq) + 2 F–(aq)
We can construct an ICE table for this dissociation. Remember that solids are ignored in the ICE table and Ksp expression.
What is the molar solubility of barium fluoride ( BaF2 ) in water? The solubility-product constant for BaF2 is 1.7x 10-6 at 25°C.
A) 6.5 x 10-4
B) 7.5 x 10-3
C) 1.8 x 10-3
D) 1.2 x 10-2
E) 5.7 x 10-7
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