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A solution contains 1.0 x 10-5 M Na3PO4. What is the minimum concentration of AgNO3 that would cause precipitation of solid Ag3PO4 (ksp = 1.8 x 10-18)?

Sagot :

The minimum concentration of AgPO4 that will cause precipitation of Ag3PO4 is [tex]5.64*10^-^5M[/tex]

Data;

  • Ksp of Ag3PO4 = 1.8*10^-18
  • concentration of Na3PO4 = 1.0*10^-5 M

The KSP value of the Precipitate

[tex]ksp = [Ag]^3[PO_4][/tex]

The ksp value of [tex]AgPO_4 = 1.8*10^-^1^8\\[/tex]

Let's substitute the values and solve for the cation

[tex]1.8*10^-^1^8= [Ag]^3[1.0*10^-^5]\\\\[/tex]

This becomes

[tex][Ag]^3=\frac{1.8*10^-^1^8}{1.0*10^-^5}\\ \\[/tex]

[tex][Ag]=\sqrt[3]{1.8*10^-^1^3}\\\\[/tex]

[tex][Ag] = 5.64 * 10 ^-5M[/tex]

From the above calculation, we can say that the minimum concentration of AgPO4 that will cause precipitation of Ag3PO4 is 5.64*10^-5M

Learn more on solubility and ksp value of solutions here;

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