The slightly soluble salt fluorapatite, Cas(PO4)3F, has a Ksp = 1 x 1031. It dissociates in water according to the following equation: Cas(PO4)3F(s) 5Ca2+ +3 PO43- + F Write the Ksp equation for this process: Ksp = 1. 2. Calculate the equilibrium concentrations of Ca2+, PO43- , and F. a. [Ca2] = b. [PO43-]= c. [F] = How many grams of fluorapatite will dissolve in 1L of water? 3. 4. The solubility of the related salt hydroxyapatite, Cas(PO4)30H (Ksp 1 x 10-29), is affected by the pH of the water to which it is added. Calculate the number of grams of hydroxyapatite that will dissolve in 0.250L of a. neutral water. Calculate the number of grams of hydroxyapatite that will dissolve in 0.250L of b. water having a pH 5.5 Thus, the equilibrium concentration of ions is, =5x = 5x 1.01x104-5.05x104 Ca4 POj3x3x1.01x 10 -3.03x104 [Fx 1.01x10-4

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The slightly soluble salt fluorapatite, Cas(PO4)3F, has a Ksp = 1 x 1031. It dissociates in water
according to the following equation:
Cas(PO4)3F(s) 5Ca2+ +3 PO43-
+ F
Write the Ksp equation for this process: Ksp =
1.
2. Calculate the equilibrium concentrations of Ca2+, PO43- , and F.
a. [Ca2] =
b. [PO43-]=
c. [F] =
How many grams of fluorapatite will dissolve in 1L of water?
3.
4. The solubility of the related salt hydroxyapatite, Cas(PO4)30H (Ksp 1 x 10-29), is affected
by the pH of the water to which it is added.
Calculate the number of grams of hydroxyapatite that will dissolve in 0.250L of
a.
neutral water.
Calculate the number of grams of hydroxyapatite that will dissolve in 0.250L of
b.
water having a pH
5.5
Expand
Transcribed Image Text

The slightly soluble salt fluorapatite, Cas(PO4)3F, has a Ksp = 1 x 1031. It dissociates in water according to the following equation: Cas(PO4)3F(s) 5Ca2+ +3 PO43- + F Write the Ksp equation for this process: Ksp = 1. 2. Calculate the equilibrium concentrations of Ca2+, PO43- , and F. a. [Ca2] = b. [PO43-]= c. [F] = How many grams of fluorapatite will dissolve in 1L of water? 3. 4. The solubility of the related salt hydroxyapatite, Cas(PO4)30H (Ksp 1 x 10-29), is affected by the pH of the water to which it is added. Calculate the number of grams of hydroxyapatite that will dissolve in 0.250L of a. neutral water. Calculate the number of grams of hydroxyapatite that will dissolve in 0.250L of b. water having a pH 5.5

Thus, the equilibrium concentration of ions is,
=5x = 5x 1.01x104-5.05x104
Ca4
POj3x3x1.01x 10
-3.03x104
[Fx 1.01x10-4
Expand
Transcribed Image Text

Thus, the equilibrium concentration of ions is, =5x = 5x 1.01x104-5.05x104 Ca4 POj3x3x1.01x 10 -3.03x104 [Fx 1.01x10-4

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