Problem: 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 10-4B) 7.5 x 10-3C) 1.8 x 10-3D) 1.2 x 10-2E) 5.7 x 10-7

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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.



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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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