Ksp =(Mg+2)(2F-)^2
Ksp = (1.18*10^-3)(2*1.18*10^-3)^2
Ksp = 6.57*10^-9 ( mole/litre)^3
A saturated solution of magnesium fluoride , MgF2, was prepared by dissolving solid MgF2 in water. The concentration of...
Part A A saturated solution of barium fluoride, BaF2, was prepared by dissolving solid BaF2 in water. The concentration of Ba2+ ion in the solution was found to be 7.52�10?3M . Calculate Ksp for BaF2. Part B The value of Ksp for silver carbonate, Ag2CO3, is 8.10�10?12. Calculate the solubility of Ag2CO3 in grams per liter.
A saturated solution of barium fluoride, BaF2, was prepared by dissolving solid BaF2 in water. The concentration of Ba2+ ion in the solution was found to be 7.52×10−3 M . Calculate Ksp for BaF2. The value of Ksp for silver chromate, Ag2CrO4, is 9.0×10−12. Calculate the solubility of Ag2CrO4 in grams per liter.
1. A saturated solution of lead(II) chloride was prepared by dissolving PbCl2 solid in water. The concentration of Pb+2 ion in the solution was found to be 1.62*10^-2M . Calculate Ksp for PbCl2 . 2. The value of Ksp for silver chromate, Ag2CrO4 is 9.0*10^-12 . Calculate the solubility of Ag2CrO4 in grams per liter.
The equilibrium concentration of fluoride ion in a saturated magnesium fluoride solution is
A chemist makes 820. mL of magnesium fluoride (MgF2) working solution by adding distilled water to 130. ml. of a 2.02 mm stock solution of magnesium fluoride in water. Calculate the concentration of the chemist's working solution. Round your answer to 3 significant digits. MM х ? Dilution A chemist makes 820, ml. of magnesium fluoride (MgF2) working solution by adding distilled water to 130. ml. of a 2.02 mm stock solution of magnesium fluoride in water Calculate the concentration...
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
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...
1.. A 52.0-mL volume of 0.35 M CH3COOH (Ka=1.8×10−5) is titrated with 0.40 M NaOH. Calculate the pH after the addition of 29.0 mL of NaOH. 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 1.18×10−3 M . Calculate Ksp for MgF2. 3. The value of Ksp for silver carbonate, Ag2CO3, is 8.10×10−12. Calculate the solubility of Ag2CO3 in grams per...
A chemist prepares a solution of magnesium fluoride (MgF2) by measuring out 0.03 g of magnesium fluoride into a 350. mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in mol/L of the chemist's magnesium fluoride solution. Round your answer to 1 significant digit molL
A chemist makes 560.mL of magnesium fluoride MgF2 working solution by adding distilled water to 160.mL of a 0.00154M stock solution of magnesium fluoride in water. Calculate the concentration of the chemist's working solution. Be sure your answer has the correct number of significant digits.