Problem: The solubility of zinc(II) phosphate, Zn3(PO4)2, in pure water is 1.5×10–7 moles per liter. Calculate the value of Ksp for zinc(II) phosphate from this data. a. 2.3×10–14b. 5.1×10–28c. 2.7×10–33d. 8.2×10–33e. 7.6×10–35

FREE Expert Solution

Recall that Ksp is an equilibrium constant related to slightly soluble ionic compounds


The dissociation of slightly soluble ionic compounds in solution is as follows:

MnNm(s)  n Mm+(aq) + m Nn–(aq)


The Ksp expression then is:


Ksp=productsreactants=[nx]n[mx]m


where x = molar solubility of the compound.


Solve Ksp for each:

Zn3(PO4)2; molar solubility = 1.5×10–7

MX(s)  M+(aq) +X(aq)


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Problem Details

The solubility of zinc(II) phosphate, Zn3(PO4)2, in pure water is 1.5×10–7 moles per liter. Calculate the value of Ksp for zinc(II) phosphate from this data. 

a. 2.3×10–14

b. 5.1×10–28

c. 2.7×10–33

d. 8.2×10–33

e. 7.6×10–35

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