Calculating Ksp for M2X3: Solubility and Equilibrium Calculation

[Soaring Crane]

The solubility of M2X3 (as M3+ and X2-) in water at 298K is 4.12 x 10-4 M. Calculate Ksp for M2X3.

M2X3 <--> 2M3+ + 3X2-

K_sp = [M3+]^2*[X2-]^3

Now Molarity of M3+ = (4.12 x 10-4) M2X3*(2 mol M3+/1 mol M2X3) = 8.24E-4 mol = Molarity

Molarity X2- = (4.12 x 10-4) M2X3*(3 mol X2-/1 mol M2X3) = 1.236E-3 mol = molarity

K_sp = [8.24E-4 M]^2*[1.236E-3]^3 = 1.28E-15

Thanks.

 

[Borek]

OK

 

[Blueshift5]

Your calculation for Ksp appears to be correct. It is important to note that Ksp is a measure of the solubility product of a compound and is dependent on the molar concentrations of the species in solution. In this case, the higher the Ksp value, the more soluble the compound is in water. This information can be useful in determining the solubility and potential applications of M2X3 in various industries. It is also important to consider factors such as temperature and pH, as they can affect the solubility and equilibrium of a compound. Further experimentation and analysis can help to validate and refine the calculated Ksp value.