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The slightly soluble salt fluorapatite, Ca­5(PO4)3F, has a Ksp= 1 x 10-31. It dissociates in water according to the following equation:             Ca­5(PO4)3F(s)   ó 5Ca2+    +   3PO43-     +    F- Write the Kspequation for this process:  Ksp= ___________________________   Calculate the equilibrium concentrations of Ca2+, PO43- , and  F-.   [Ca2+] = _____________________ [PO43- ] = ______________________ [F-] = ______________________

The slightly soluble salt fluorapatite, Ca­5(PO4)3F, has a Ksp= 1 x 10-31. It dissociates in water according to the following equation:             Ca­5(PO4)3F(s)   ó 5Ca2+    +   3PO43-     +    F- Write the Kspequation for this process:  Ksp= ___________________________   Calculate the equilibrium concentrations of Ca2+, PO43- , and  F-.   [Ca2+] = _____________________ [PO43- ] = ______________________ [F-] = ______________________

Chemistry
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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The slightly soluble salt fluorapatite, Ca­5(PO4)3F, has a Ksp= 1 x 10-31. It dissociates in water according to the following equation:

            Ca­5(PO4)3F(s)   ó 5Ca2+    +   3PO43-     +    F-

  1. Write the Kspequation for this process:  Ksp= ___________________________

 

  1. Calculate the equilibrium concentrations of Ca2+, PO43- , and  F-.

 

  1. [Ca2+] = _____________________
  2. [PO43- ] = ______________________
  3. [F-] = ______________________
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