1. If Ksp = 6.4 x 10-9 for magnesium fluoride, what is the concentration of Mg2+ and Fin equilibrium with solid magnesium fluoride? First write the equilibrium expression for Ksp.
2. The concentration of Ag+ in a solution saturated with Ag2C2O4 is 2.42 x 10-4 M. Calculate Ksp for Ag2C2O4.
1. If Ksp = 6.4 x 10-9 for magnesium fluoride, what is the concentration of Mg2+...
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
M. A student measures the Mg2+ concentration in a saturated aqueous solution of magnesium fluoride to be 1.15X10 Based on her data, the solubility product constant for magnesium Muoride is
please explain A saturated solution of magnesium fluoride has a concentration [F]of 2.34 x 10-3 M. For this compound, Ksp = 1.17 x 10-3 O (1.17 x 10-32 4(1.17 x 10-33 3(1.17 x 10-333 (1.17 x 10-33 Question 5 0.5 pts Calculate the solubility of magnesium sulfate, MgSO4, when placed into a 0.10 M MgCl2 solution (100% soluble). Mg SO, has a Ksp = 5.9 x 10-3 4.2 10-2M 5.9* 102M 7.7 * 102M 3.5 * 10M 3.5 * 10...
1. Calculate the solubility product constant, Ksp, for strontium fluoride if 1.2×10-3mol of F-ion is present in 2.0 L of a saturated strontium fluoride solution. A.9.0×10-8 B.2.7×10-11 C.6.9×10-9 D.1.1×10-10 E.1.4×10-6 2. Choose the correct equilibrium constant expression (Ksp) for the dissolution of Ag2S . (is the answer D?) A. [ Ag2S ] Ksp = [ Ag+]2 [ S2-] B. Ksp = [ Ag+][ S2-]2 C. [ Ag+] [ S2-] Ka = [ Ag2S ] D. Ksp = [ Ag+]2 [...
A saturated solution of magnesium fluoride , MgF2, was prepared by dissolving solid MgF2 in water. The concentration of Mg2+ ion in the solution was found to be 1.18
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...
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.
4.2 x 10-3 4. Magnesium fluoride (MgF,) is a sparingly soluble salt. It has Kp = 7.4 x 10-9. Calculate the concentration of fluoride ion in a saturated solution of MgF2.
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 solubility of magnesium fluoride in pure water is 1.65 x 10^-3 grams per 100 mL of water. a. Calculate Ksp for magnesium fluoride. b. What is the solubility of magnesium fluoride in a 0.500 M magnesium nitrate solution? c. What could you do to increase the solubility of magnesium fluoride?