1. If Ksp = 6.4 x 10-9 for magnesium fluoride, what is the concentration of Mg2+ and F- in equilibrium with solid magnesium fluoride? First write the equilibrium expression for Ksp.
2. What is the solubility of lead (II) bromide in 0.330 M sodium bromide?
What causes the difference in solubilities of the lead (II) bromide?
We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
1. If Ksp = 6.4 x 10-9 for magnesium fluoride, what is the concentration of Mg2+...
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.
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
What is the solubility of lead (II) bromide in 0.330 M sodium bromide? What causes the difference in solubilities of the lead (II) bromide?
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.
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
The concentration of Mg2+ at equilibrium (25oC) is 0.000144 M. What is the value of Ksp at this temperature? In the solubility rules, Mg(OH)2 was listed as an "insoluble" salt. It is actually slightly soluble in an equilibrium reaction: Mg (OH)2 (s) Mg2+ (aq) 20H (aq) The concentration of Mg2+ at equilibrium (25°C) is 0.000144 M. What is the value of Ksp at this temperature? Submit Answer Tries o/99
1) Use equilibrium ion concentration to calculate Ksp. The Pb2+ concentration in a saturated solution of lead bromide is measured and found to be 1.19×10-2 M. Use this information to calculate a Ksp value for lead bromide. Ksp =___________ 2) Use solubility to calculate Ksp. The solubility of Fe(OH)2 is measured and found to be 1.15×10-3 g/L. Use this information to calculate a Ksp value for iron(II) hydroxide. Ksp =______________
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?
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?
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...