A generic salt, AB2, has a molar mass of 293 g/mol and a solubility of 3.90 g/L at 25 °C. What is the Ksp…?

of the salt at 25 degrees C?

Please help. I’m super confused. Thanks. ^_^

Ksp = [A++]*[B-]^2

?M AB2 = 3.90 g/L x 1 mole / 293 g = 0.0133 M

[A++] = 0.0133 M

[ B-] = 0.0266 M

Ksp = [0.0133]*[ 0.0266 ]^2 = 9.41x10E-6
AB2=3.90g/L x 1 mole/ 293 g=0.0133 M

[A++]= 0.0133 M

[B-]= 0.0133 x 2 = 0.0266

Ksp= [0.0133] x [0.0266]^2 = 9.41 x 10^-6
multiply by two, since the equation is AB2 –> A^2+ + 2B^2-

Therefore, 2*.0133=.0266

However, since the solubility equation requires the coefficient to be moved up as a power, you still have to square the .0266
how’d you get the B-