Solubility of CaF2 at 25°C is S= 20 x 10 mol/L. Calculate Kp 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...
POST-LABORATORY QUESTIONS student analyzed a saturated CaF2 solution by the ion-exchange chromatography/titration method and found that [Ca] 2.14 x 10 M. Write out the expression for Ksp of CaF and determine the numerical value of Ksp Suppose a student overtitrates the eluent from the CaSO, experiment (that is, she titrates to a persistent deep pink endpoint). Will the calculated value of Ksp be too high, too low, or unaffected? Explain. 2. 3. The value of Kp for lead (lIl) chromate...
References CHEMWORK The Kp for CaF2(8) is 4.0x10-" Calculate the solubility of CaF2(s). Ignore any potential reaction of the ions with water. Solubility for CaFz(s) = mol/L Submit Show Hints
APP-17 A 4 Problem Set 13 CHEM 1252 October 21, 2019 Textbook Reading Assignment: 14.6-10 Additional Practice Problems: 1466 -68.20.73.75.27.79.83.86-87,89,101,107,111-115,119 1. Ammonia and hydrogen sulfide can both be formed directly from their elements. At 90 "C... Nale) + 3H2(e) -2NH3G) * = 120 Hale) + SC) - H256) K = 0.068 Find Kat 90 °C for the following reaction 2NH3(e) + 35() - 3H.SG) + Nale) K? 2. The equilibrium constant for the following reaction is called the solubility product...
Learning Goal: To learn how to calculate the solubility from Kspand vice versa. Consider the following equilibrium between a solid salt and its dissolved form (ions) in a saturated solution: CaF2(s)⇌Ca2+(aq)+2F−(aq) At equilibrium, the ion concentrations remain constant because the rate of dissolution of solid CaF2 equals the rate of the ion crystallization. The equilibrium constant for the dissolution reaction is Ksp=[Ca2+][F−]2 Ksp is called the solubility product and can be determined experimentally by measuring thesolubility, which is the amount...
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)
Assuming that the solubility of PbBr2(s) is 2.1x10 mol/L at 25°C, calculate the Ksp for this salt. Ignore any potential reactions of the ions with water.
Assuming that the solubility of PbCl2(s) is 1.6x10-2 mol/L at 25°C, calculate the Ksp for this salt. Ignore any potential reactions of the ions with water. Ksp = _______ The solubility of Pb(IO3)2(s) in a 2.00x10-2 M KIO3 solution is 7.7x10-8 mol/L. Calculate the Ksp value for Pb(IO3)2(s). Ksp = _______
Help please! Show work xercise 14.16 thodynamic 2. The equilibrium constant for the following reaction is called the fluoride: constant for the following reaction is called the "solubility product of calcium CaF2(s) - Ca2+(aq) + 2F (aq) K = K = 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...
For CaF2 Kap = 3.9 x 10-" (molar mass = 78 g mol-') at 25°C. How many grams of this salt can be dissolved in 100 mL water at 25°C? (A) 0.8 mg (B) 1.2 mg (C) 1.7 mg (D) 2.0 mg (E) 2.4 mg