A saturated solution is formed when a salt is added to water until equilibrium i

Question

A saturated solution is formed when a salt is added to water until equilibrium is established between the undissolved salt and its ions in solution. This process can be represented by the equation: Ag3PO4(s) right left harpoons 3Ag^+ (aq) + P04^3 - (aq) At a particular temperature, the concentration of silver ions in a saturated solution of silver phosphate is 1.17E - 4 M. What is the equilibrium constant, Ksp, for this salt at this particular temperature? Please record your answer to the correct number of significant figures. To enter x 10^n, please use En. For example 1.23 x 10^ - 5 should be entered as 1.23E - 5

Explanation / Answer

Ag3PO4 <-> 3Ag+ and PO4-3

IF [Ag+] = 1.17*10^-4

Calculate Ksp

Ksp, by definition is given by:

Ksp = [Products]^P

where [Products] = concentration of the products (ions in solutoin)

P = is the stoichiometric coefficient of each susbtance

From Equation

Ag3PO4 <-> 3Ag+ and PO4-3

Ksp = [Ag+]^3 [PO4-3]

We have the [Ag+] but we need to calculate [PO4-3]

You can see that there is 3 moles of Ag+ ions per 1 mol of PO4-3 ion

This means that, by sotichiometry:

3[Ag+] =  [PO4-3]

Therefore:

[Ag+] = 1.17*10^-4

[PO4-3] = 3[Ag+] = 3*(1.17*10^-4) = 3.51*10^-4

Now we can calculate Ksp

Ksp = [Ag+]^3 [PO4-3] = ((1.17*10^-4)^3 )* (3.51*10^-4) = 5.62*10^-16

Ksp = 5.62*10^-16

If you need the notation they are asking us

Ksp = 5.62E-16

Hope it helps!

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