Question

6. The Ksp for Barium Fluoride, BaF2, is 1.0 x 10^-6.

a. Write the Ksp expression for this salt.

b1. Calculate the concentration of the anion. Do not do the algebra. Leave your answer in terms of x.

b2. Calculate the molar solubility. Do not do the algebra. Leave your answer in terms of x.

c. Calculate the concentration of the barium ion if 0.20 moles of KF is added to 1.0liter of the saturated barium fluoride solution. You do need an actual value for this answer.

I need help with C.) I understand that it is a common ion problem, but from there I'm somewhat lost

Answer 1

eve Bah Ba't + zr- s 29 u se the solubility of Bate. ..Ksp = [alt][F]" = s (23) = 45? (en) Kap = 483 ; where, s be the solublety of Bar (1483 = 1x10-6 g 53 - 1x10-6 - oba s = 2.5X10+ S S 6-36 V10-3 - [ B221) = 630x10} CE) 2X6 30x103 0.0126 (22, Molar susulity of Bar = 6-30 x 103 m © Bafz — Balt + 26- 2 x 22 KE --→KER- 0.20m 0.2om 0-20m conc-of RF - 0-20 ml 11 -0.20 mol/L . [Balt) = x -IF-) = 2x+0.20 ... Kap = Balote] = x (Zu-+ 0-20) = 27174712 + 2X @2x x 0 20 + (0-20) = zu [4u²to.sont 0.04) 2XX0:04 (as in very small hence we can neglect higher form of a

Hine, Ksp = 0.042 this o.o4n = 1x106 nx = 2x105 ..come. A Barton = 2x105 m