What is the relationship between ΔG and the
ΔG°F for the reaction below?
MgF2(s) → Mg2+(aq) + 2
F-(aq)
ΔG = {ΔG°f [Mg2+ (aq)] + 2 ΔG°f [F- (aq)] - ΔG°f [MgF2 (s)]} + RT ln ([Mg2+] [F-]2/[MgF2]) |
ΔG = {ΔG°f [Mg2+ (aq)] + 2 ΔG°f [F- (aq)]} + RT ln ([Mg2+] [F-]2) |
ΔG = {ΔG°f [Mg2+ (aq)] + 2 ΔG°f [F- (aq)] - ΔG°f [MgF2 (s)]} + RT ln ([Mg2+] [F-])2) |
ΔG = {ΔG°f [Mg2+ (aq)] + 2 ΔG°f [F- (aq)] - ΔG°f [MgF2 (s)]} + RT ln Ksp |
What is the relationship between ΔG and the ΔG°F for the reaction below? MgF2(s) → Mg2+(aq)...
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).
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...
For the following equilibrium, MgF2(s)↽−−⇀Mg2+(aq)+2F−(aq) If Ksp=5.1×10−13, what is the molar solubility of magnesium fluoride: Report your answer in scientific notation with the correct number of significant figures.
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In a saturated solution of MgF2 at 16 °C, the concentration of Mg2+ is 1.44x10 –3 M The equilibrium is represented by the equation MgF2 -->Mg 2+ + 2 F-. A.Write the expression for the solubility product constant, Ksp. B.Calculate the value of Ksp at 16°C for MgF2 Note: Your answer is assumed to be reduced to the highest power possible. C.Calculate the equilibrium concentration of Mg2+ in 1.000 L of saturated MgF2 solution at 16°C to which 0.450 mole of...
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Consider the reaction Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) at 57 ∘C , where [Fe2+]= 3.40 M and [Mg2+]= 0.210 M . help Part D Calculate the standard cell potential for Mg(s) Fe2 (aq)Mg2 (aq)Fe(s) Express your answer to three significant figures and include the appropriate units. View Available Hint(s) ? Value Eo Units Submit Part C What is the value for n? Express your answer as an integer and include the appropriate units (i.e. enter mol for moles). View Available Hint(s) HA ? Value...
Calculate the [F-] present in a satuated solution of magnesium fluoride if Ksp= 7.4 x10^-11 MgF2(s) <—-> Mg 2+ (aq)+ 2F-(aq)