For this problem, we’re being asked to calculate the Ksp of barium fluoride.
Since the barium fluoride is an ionic compound, it forms ions when dissociating in water. The dissociation of barium fluoride in water is as follows:
The fluoride is from Group 7A and has a charge of –1. Barium is from Group 2A and has a charge of +2:
BaF2(s) ⇌ Ba2+(aq) + 2 F–(aq)
We can construct an ICE table for the dissociation of BaF2.
Remember that solids are ignored in the ICE table and Ksp expression.
At 25 °C the solubility of barium fluoride is 7.52 x 10-3 mol/L. Calculate the value of Ksp at this temperature. Enter your answer in exponential format (example: 1.23E-4) with two decimal places.
a. 1.70 x 10-6
b. 5.65 x 10-5
c. 1.13 x 10-4
d. 7.70 x 10-6
e. 1.71 x 10-5
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