A saturated solution of Au2X is found to have a Au concentration of 4.05 ppm

Question

Au2X(s) <-> 2 Au X ^2-

What is the value of Ksp for Au2X?

how do you convert 4.05 ppm to mol/L?

Answer 1

[Au+] = 4.05 ppm = 4.05 mg/L = 0.00405 g/L =&gt;

0.00405 / 196.9665 g/mol =0.0000206 M

[X2-] = 0.0000206/2 =0.0000103 M

ksp = (0.0000206)^2 ( 0.0000103) =4.37 x 10^-15