2) The solubility product for calcium fluoride (CaF2, MW largest 78.1 g/mol) is Kp 4.0 x 10-11 What is the mass of...
(15 pts) The solubility product of calcium fluoride (CaF2) is 3.45 x 10-11 at 25°C. Will a fluoride concentration of 1.0 mg/L be soluble in a water containing 150 mg/L of calcium?
The solubility product of calcium fluoride (CaF2) is 3x10^-11. If water contains 250 mg/L calcium, how much fluoride will be soluble?
9) What is the gram solubility of CaF2 in 100.0 mL of pure water at 25 degree C. The solubility product constant of CaF2 is 3.9*10^-11. The molar mass is 78.1 g/mol.
1) The solubility product for cobalt II hydroxide (CO(OH), MW = 92.95 g/mol) is Kp = 5.92 x 10-15 at T = 25. °C. a) What are the molar solubility and the solubility by mass of cobalt II hydroxide in pure water?
1) The solubility product for cobalt II hydroxide (CO(OH), MW = 92.95 g/mol) is Kp = 5.92 x 10-15 at T = 25. °C. a) What are the molar solubility and the solubility by mass of cobalt II hydroxide in pure water?
2 pts) The solubility of InF3 is 4.0 x 10-2 g/100 mL. a) What is the Ksp? Include the chemical equation and Ksp expression. MW (InF3): 172 g/mol b) If 0.050 moles of potassium fluoride are added, what is the solubility of InF3?
2. (2 pts) The solubility of InF3 is 4.0 x 10-2 g/100 mL. a) What is the Ksp? Include the chemical equation and Ksp expression. MW (InF3): 172 g/mol b) If 0.050 moles of potassium fluoride are added, what is the solubility of InF3?
2. The equilibrium constant for the following reaction is called the "solubility product" of calcium fluoride: CaF2(s) - Cal(aq) + 2F-(ay) K = Kp = 3.2 x 10-11 (a) Write an expression for the equilibrium constant of this reaction in terms of concentrations. Why do you suppose we call this a solubility product instead of a solubility quotient or ratio? (b) Calculate the equilibrium concentrations of Ca2+ and F if excess solid CaF is placed in water. (c) in which...
2. The molar solubility of calcium fluoride in water is 2.1 x 104 moles/L. What is the Ksp of CaF2? a) 3.7 x 10-11 b) 2.14 x 10-4 c) 4.6 x 10 d) 9.8 x 10-12
8) (G) Calculate the solubility of solid CaF2 (Kp-4.0x 10-1) in water. (ii) Calculate the solubility of solid CaF2 in a 1.0 L 0.025 M NaF solution. (ii) Explain the difference in solubility of CaF2 in (i) and (ii) If 20.0 mL of 0.10 M Ba(NO3)2 are added to 50.0 mL of 0.10 M Na2COs, will BaCOs precipitate? (Kup for BaCo 2.6 x 10). 9)