Answer:
[tex]7.5x10^{-3}M[/tex]
Explanation:
Hello,
In this case, since the dissociation barium fluoride is represented at equilibrium by:
[tex]BaF_2(s)\rightleftharpoons Ba^{2+}(aq)+2F^-(aq)[/tex]
Hence, the equilibrium expression is:
[tex]Ksp=[Ba^{2+}][F^-]^2[/tex]
Whereas the molar solubility is represented as the reaction extent [tex]x[/tex]:
[tex]Ksp=[x][2x]^2[/tex]
In such a way, we can solve for [tex]x[/tex]:
[tex]1.7x10^{-6}=4x^3\\\\x=\sqrt[3]{\frac{1.7x10^{-6}}{4} } \\\\x=7.5x10^{-3}M[/tex]
Which as said before, is the molar solubility.
Best regards.
