s. At a certain temperature, a saturated solution of magnesium fluoride has a ma
ID: 536332 • Letter: S
Question
s. At a certain temperature, a saturated solution of magnesium fluoride has a magnesium ion concentration of 1.35 x 103 M. Assume that the temperature is constant throughout the experiment and answer the questions below. (a) Calculate the value of Ksp. (b) What is the magnesium ion concentration of 1.000 liter of the saturated magnesium fluoride solution to which 5.81 g of potassium fluoride has been added? The potassium fluoride dissolves completely. Assume that there is no appreciable change in the volume of the solution. (c) If 00 mL of a 3.00 x 103 M solution of magnesium nitrate is mixed with 50.00 mL of 2.00 x 103 M sodium fluoride, will a precipitate form? Show calculations to support your answer.Explanation / Answer
9. For the givem MgF2
(a) Ksp = [Mg2+][F-]^2
with, [Mg2+] = 1.35 x 10^-3 M
Ksp = (1.35 x 10^-3)(2 x 1.35 x 10^-3)^2 = 9.84 x 10^-9
(b) [F-] added = 5.81 g/42 g/mol x 1 L = 0.14 M
[Mg2+] = Ksp/[F-]^2
= 9.84 x 10^-9/(0.14)^2 = 5.02 x 10^-7 M
(c) Qsp = [Mg2+][F-]^2
= (3 x 10^-3 M x 25 ml/75 ml((2 x 10^-3 M x 50 ml/75 ml)^2
= 1.77 x 10^-9
Qsp < Ksp, therefore, no precipitation would occur in this case.
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