The solubility product of BaSO4 at 25 C is 10^-9. What would be the concentration of H2SO4 necessary to precipitate BaSO4 from a solution of 0.01 M Ba+2 ions

Question

abhisar · Answer

I am calculating it to be $\sf 10^{-7}$

abhisar · Answer

But the answer says $\sf 10^{-6}$

abhisar · Answer

Any idea @Photon336 ?

abhisar · Answer

@Rushwr ?

photon336 · Answer

$$ksp = x ^{2} = [Ba ^{2+}][So4^{2-}]$$

$$\frac{ [10^-9] }{ [0.01] } = 10^{-7}$$

by eyeballing this I believe that's when it's saturated.  so it would have to be more than that 10^-6 @abishar 

I agree with @rushwr

abhisar · Answer

Oh Right!!!!!!!!!!!!!

photon336 · Answer

I think that's the concentration when it's saturated that means that it won't precipitate at this concentration , @rushwr what do you think?

abhisar · Answer

I get it now, it should be anything greater than $\sf 10^{-7}$ and hence $\sf 10^{-6}$

abhisar · Answer

Thanx both of you c:
Appreciate it..

photon336 · Answer

Absolutely, anytime