Discover the answers you need at Westonci.ca, where experts provide clear and concise information on various topics. Connect with a community of professionals ready to help you find accurate solutions to your questions quickly and efficiently. Experience the convenience of finding accurate answers to your questions from knowledgeable experts on our platform.

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;

https://brainly.com/question/15546566

https://brainly.com/question/9866138