QUESTION 6 (15 points) A) A saturated solution of calcium fluoride CaF2 is found to contain...
10 L of a saturated solution of calcium fluoride, CaF2, was evaporated and found to contain 4.28 millimoles (mmol) fluoride. What is the value of Ksp? CaF2(s) -> <- ca2+ (aq) +2 F- (aq) How did Ksp= [Ca2+] [F-]2 become Ksp= [s] [2s]2= 4s3 Cause I thought it was only Ksp= [s] [s]2 = s3 and why 4.28x10-3 have to devide by 10 and why the [F-] = 4.28 x 10-4 have to eqautes to 2 to have s= 2.14x10-4...
55. In a saturated solution of calcium fluoride, the concentration of the calcium ions is measured to be 2.4x10 M. What is the solubility product of calcium fluoride? 5.1 x 10 (1) 5.7 x 10 (2) 5.7 x 10-10 (3) (4) 5.5 x 101 (5) 2.4 x 10
(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?
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?
A student measures the Ca2+ concentration in a saturated aqueous solution of calcium fluoride to be 2.18x10-6 M. Based on her data, the solubility product constant for calcium fluoride is Submit Answer Retry Entire Group 9 more group attempts remaining
tion 12 of 27 > In a saturated aqueous solution of CaF , the calcium ion concentration is 2.15 x 10-4 M and the fluoride ion concentration is 4.31 x 10M. Calculate the solubility product, Kıp, for CaF, Kop =
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...
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...
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?
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?