Q10.an aqueous solution contains 5.00x10-2 mol/l of ca2+ and 7.00x10-3 mol/l of so4

2-

. show whether

this solution would precipitate anhydrite caso4 or not provided that the ksp for anhydrite is equal to 10-4.5.

The precipitate will form.

Explanation:

Let's write the equilibrium expression for the solubility product of calcium sulfate:

⇄

The solubility product is defined as the product of the free ions raised to the power of their coefficients, in this case:

Our idea is to find the solubility quotient, Q, and compare it to the K value. A precipitate will only form if Q > K. If Q < K, the precipitate won't form. In this case:

Now given the K value of:

Notice that:

This means the precipitate will form, as we have an excess of free ions and the equilibrium will shift towards the formation of a precipitate to decrease the amount of free ions.

idk what is it? is this a question that you know the answer or u dont