The solubility product for calcium phosphate is 2.0x10^-29. A. Calculate the mol

ID: 825586 • Letter: T

Question

The solubility product for calcium phosphate is 2.0x10^-29.

A. Calculate the molar solubility of calcium phosphate, and the concentrations of

the calcium and phosphate ions at equilibrium.

B. Using Excel, create a spreadsheet that calculates the calcium and phosphate ion

concentrations at equilibrium following the addition of 1.0x10^-8

M to

1.0x10^-7

M calcium chloride, in increments of 1.0x10^-9

M. From this data, plot

the concentration of the phosphate ion versus the concentration of the calcium

ion at equilibrium. (You may want to multiply the concentrations by some

constant value to make it easier to read the axes labels.) Print out and turn in

your plot with sample calculations (handwritten) of the calcium and phosphate

ion concentrations calculated for any three points between 1.0x10^-8

M to

1.0x10^-7

M calcium chloride. (Make sure you plot adheres to the required

standards on page 33 of the lab manual.)

Ca3(PO4)2 ---------------------------------------> 3 Ca 2+ + 2 PO4 3-

x 3x 2x

so solubility product = [Ca2+]^3 [PO43-]^2

molar solubility = 2*10^-29 M

(3x)^3 *(2x)^2 = 2*10^-29

so 108 x^5 = 2*10^-29

so x^5 = 0.1851 * 10^-30

so x= 0.713* 10^-6

so [Ca2+] = 3x = 2.14 *10^-6 M

[PO4 3-] = 2x = 1.426*10^-6M

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