A solution contains 3.0x10^-3 M Mg(NO3)2. What concentrations of KF will cause precipitation of solid MgF2 (Ksp=6.4x10^-9).
For magnesium fluoride,
... ...(1)
Magnesium ion concentration is obtained from magnesium nitrate.
... ...(2)
Substitute equation (2) into equation (1)
Hence, required concentration
A solution contains 3.0x10^-3 M Mg(NO3)2. What concentrations of KF will cause precipitation of solid MgF2...
A solution contains 3.0 x 10^-3 M Mg(NO3)2. What concentrations of KF will cause precipitation of solid MgF2 (Ksp = 6.4x10^-9)?
A solution is prepared by mixing 150mL of 1.00 x 10-2 M Mg(NO3)2 and 250 mL of 1.00 x 10-1 M NaF. How much solid MgF2 (in milligrams) if any will remain? (Ksp of MgF2 is 6.4 x 10-9 )
V 17.34 What is the molar solubility of MgF2 in a 0.40 M. Mg(NO3)2 solution? (K for MgF2 = 8.0 X 10-8.) sp
2. A solution is 0.10M in Mg(NO3)2. a. What concentration of OH is required to just start precipitation of Mg(OH)2? (Ksp = 1.5x10-11) b. If NH3/NH4+ buffer is used to control the pH, and [NH3] = 0.10 M, what concentration of NH4 is required to prevent the precipitation of Mg(OH)2?
A solution contains 7.7 x 10-5 M Na3PO4. What is the minimum concentration of AgNO3 that would cause precipitation of solid Ag3PO4 (Ksp = 1.8 x 10–18)? Concentration =
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...
What is the molar solubility of magnesium fluoride in a solution that is 0.40 M F− ions? The Ksp of MgF2 is 6.4 × 10−9. What is the molar solubility of magnesium fluoride in a solution that is ions? The Ksp of MgF2 is 6.4x10^-9 8.0 × 10−5 8.0 × 10−9 4.0 × 10−8 1.6 × 10−8
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...
You prepare a solution by mixing 400.0 mL of 1 x 10-4 M Mg(NO3)2 and 500.0 mL of 1.00 x 10-4 M NaF. What is the observed outcome? For MgF2, Ksp = 6.4 x 10-9. A. A precipitate forms because Qsp > Ksp. B. No precipitate forms because Qsp > Ksp. C. No precipitate forms because Qsp = Ksp. D. No precipitate forms because Qsp < Ksp. E. A precipitate forms because Qsp < Ksp.
If 15.0 mL of 7.25×10-4 M MgI2 are added to 22.0 mL of 1.80×10-5 M KF, will solid MgF2 (Ksp = 6.4×10-9) precipitate? _____yes/no If a precipitate will not form, what fluoride ion concentration will cause a precipitate of magnesium fluoride to form? If a precipitate will form, what is the minimum [F-] that could have been present without initiating precipitation? Assume the total volume used in the above example. ______M