(15 pts) The solubility product of calcium fluoride (CaF2) is 3.45 x 10-11 at 25°C. Will...
The solubility product of calcium fluoride (CaF2) is 3x10^-11. If water contains 250 mg/L calcium, how much fluoride will be soluble?
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 calcium fluoride that can dissolve in 250.0 mL of water? 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 calcium fluoride that can dissolve in 250.0 mL of water?
5. The molar solubility for calcium fluoride, CaF2, is 2.0 x 10' M at 25°C. Calculate the solubility product constant for calcium fluoride a. 1.4 x 102 b. 8.0 x 10-8 c. 1.6 x 10-11 d. 3.2 x 10" e. 4.2 x 10-24 e. None of these statements is liue. 15. Which of the following statements regarding complex ions is true? a. Complex ions are formed of a metal ion and a ligand. b. The metal ion is a Lewis...
Calcium fluoride (CaF2) has a Ksp of 3.45∙10-11. If I have a 0.150 M solution of sodium fluoride, what concentration of calcium acetate will begin precipitation of the fluoride ions?
QUESTION 6 (15 points) A) A saturated solution of calcium fluoride CaF2 is found to contain a concentration of fluoride ions [F] = 3.0 x 10-6 M. What is the value of the solubility product of this salt?
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
Given the average concentration of calcium ion in natural water is 3.8×10^-4 M, and that the solubility product Ksp for CaF2 is 4×10^-11, calculate the maximum molar concentration of fluoride ion. Find the concentration fluoride in ppm scale as well.
What is the gram solubility of CAF2 in 100. mL of pure water at 25°c? The solubility product constant of CAF2 at 25°c is 3.9x10^-11
Calcium fluoride, CaF2, is an insoluble salt (Ksp = 1.46 x 10-10) that can be formed by precipitation by mixing solutions of calcium nitrate and sodium fluoride. Suppose 200.0 mL of a 0.600 M Ca(NO3)2(aq) solution are mixed with 400.0 mL of a 0.0600 M NaF(aq) solution. Will a precipitate form? How much calcium fluoride could form?