MgF2(s) <--> Mg2+(aq) + 2 F–(aq)
In a saturated solution of MgF2 at 18 0C, the concentration of Mg2+ is 1.21 x 10–3 molar. The equilibrium is represented by the equation above.
(a) Write the expression for the solubility-product constant, Ksp, and calculate its value at 18 0C.
(b) Calculate the equilibrium concentration of Mg2+ in 1.000 liter of saturated MgF2 solution at 18 0C to which 0.100 mole of solid KF has been added. The KF dissolves completely. Assume the volume change is negligible.
(c) Predict whether a precipitate of MgF2 will form when 100.0 milliliters of 3.00 x 10–3 molar Mg(NO3)2 solution is mixed with 200.0 milliliters of a 2.00 x l0–3 molar NaF solution at 18 0C. Calculations to support your prediction must be shown.
(d) At 27 0C the concentration of Mg2+ in a saturated solution of MgF2 is 1.17 x 10–3 molar. Is the dissolving of MgF2 in water an endothermic or an exothermic process? Give an explanation to support your conclusion.
MgF2(s) <--> Mg2+(aq) + 2 F–(aq) In a saturated solution of MgF2 at 18 0C, the...
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For the reaction MgF2(s) <=> Mg2+(aq) + 2 F-(aq), at a given temperature, K = 7.4 x 10-11. What MASS (you’ll need to calculate molarity!) of MgF2 could be added to 2L of water, such that ALL the MgF2 dissolves? How soluble is MgF2 in water (qualitative answer…ie, VERY, NOT VERY, etc).
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