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10. Magnesium phosphate, Mg3(PO4)2, has a solubility product constant of 2.27 x 103. a. What is...
10. Magnesium phosphate, Mg3(PO4)2, has a solubility product constant of 2.27 x 10. a. What is the molar solubility of Mg3(PO4)2 in 0.925 M potassium phosphate, K3PO4? (6 points) N. b. What is the molar solubility of Mg:(PO)in pure water? (5 points) c. Is the magnesium phosphate more soluble in part (a) or part (b)? Explain why. (3 points)
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10. Magnesium phosphate, Mg3(PO4)2, has a solubility product constant of 2.27 x 109. a. What is the molar solubility of Mg3(PO4)2 in 0.925 M potassium phosphate, K3PO4? (6 points) b. What is the molar solubility of Mg3(PO4)2 in pure water? (5 points) c. Is the magnesium phosphate more soluble in part (a) or part (b)? Explain why. (3 points)
Convert 2.27 grams of magnesium phosphate, Mg3(PO4)2 to moles of Mg3(PO4)2.
The solubility of magnesium phosphate is 2.27 × 10-3 g/1.0 L of solution. What is the Ksp for Mg3(PO4)2? (a) 6.5×10-12 (b) 6.0×10-14 (c) 5.2 × 10-24 (d) 4.8×10-26 (e) 1.0×10-26
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1. What is the molar solubility of Mg3(PO4)2 in a 0.860 M solution of sodium phosphate? The Ksp for Mg3(PO4)2 = 1.04 x 10-24 M 2. What is the molar solubility of Ag2SO4 in a 0.950 M solution of Al2(SO4)3? The Ksp for Ag2SO4 = 1.20 x 10-5 1.33e-5 x M 3. Select all of the following that are true about the common ion effect for dissolving solids. If you add potassium sulfate to a saturated...
The solubility of magnesium phosphate is 2.27* 10-3 g/L. Calculate the molar solubility of magnesium phosphate O A 2.27 x 10-3 g/L OB. 8.63 x 10 mol/L O C 5.97 x 10-7 mol/L OD. 1.03 x 10 mol/L
(a) How many grams of magnesium phosphate, Mg3(PO4)2, would you need if you were required to make 215.0 mL of a magnesium phosphate solution with a concentration of 0.110 mol L-1? (5 marks) Molar masses: Mg3(PO4)2 = 262.9 g mol-1 1 L = 1000 mL g Mg3(PO4)2 and What is the concentration of PO43- ions in the 0.110 mol L-1 solution of magnesium phosphate? (2 marks) mol L-1
(a) If the molar solubility of Mg3(PO4)2 at 25 oC is 6.26e-06 mol/L, what is the Ksp at this temperature? Ksp = (b) It is found that 6.35e-07 g of Cu3(PO4)2 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Cu3(PO4)2. Ksp = (c) The Ksp of PbBr2 at 25 oC is 6.60e-06. What is the molar solubility of PbBr2? solubility = mol/L
The solubility of magnesium phosphate is 8.64 × 10-4 mole per liter of solution. What is the Ksp for Mg3(PO4)2? 1. 6.5 × 10-12 2. 5.2 × 10-14 3. 5.2 × 10-28 4. 4.8 × 10-26 5. 1.0 × 10-26
a) The solubility product, Ksp, of Cd3(PO4)2 is 2.5 x 10-33. What is the solubility (in g/L) of Cd3(PO4)2 in pure water? b) The solubility product of Cu(OH)2 is 4.8 x 10-20. Calculate the value of pCu2+, or -log[Cu2+], in an aqueous solution of NaOH which has a pH of 12.38 and is saturated in Cu(OH)2. c) The equilibrium constant for the formation of Cu(CN)42- is 2.0 x 1030. Calculate the value of pCu2+, or -log[Cu2+], if we were to...