An aqueous solution contains 2.1 x 10° mol/L Ca2*. Enough HF was then added to the solution to reach an equilibrium concentration of [HF] = 5.5 x 10“ mol/L. What must be the pH of the solution in order to observe a precipitate of CaF2? (Hint: Assume any change in pH will not change the value of [HF]). Ksp of CaF2 = 5.3 × 10-9 Ka of HF = 7.2 × 10-4 %3D

An aqueous solution contains 2.1 x 10° mol/L Ca2*. Enough HF was then added to the solution to reach an equilibrium concentration of [HF] = 5.5 x 10“ mol/L. What must be the pH of the solution in order to observe a precipitate of CaF2? (Hint: Assume any change in pH will not change the value of [HF]). Ksp of CaF2 = 5.3 × 10-9 Ka of HF = 7.2 × 10-4 %3D

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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