At saturation 1.5 x 10^-4 moles caF2 have dissolved in 1L of water. What is Ksp for CaF2 at this temperature?
CaF2(s) ==> Ca^2+ + 2F^-
Ksp = (Ca^2+)(F^-)^2
(Ca^2+) = 1.5 x 10^-4 mols/L
(F^-) = 3.0 x 10^-4 mols/L.
Plug into Ksp and solve. Post your work if you run into trouble.
To find the value of Ksp for CaF2 at this temperature, we need to use the equation:
Ksp = (Ca^2+)(F^-)^2
Given that (Ca^2+) is 1.5 x 10^-4 moles/L and (F^-) is 3.0 x 10^-4 moles/L, we can substitute these values into the equation to find Ksp.
Ksp = (1.5 x 10^-4)(3.0 x 10^-4)^2
To simplify this expression, we need to multiply the numbers and combine the exponents. When multiplying numbers in scientific notation, you multiply the decimal parts and add the exponents.
1.5 x 3.0 x 10^-4 x (10^-4)^2
= 4.5 x 10^-4 x 10^-8
= 4.5 x 10^-4-8
= 4.5 x 10^-12
Therefore, the value of Ksp for CaF2 at this temperature is 4.5 x 10^-12.