When adding a common ion I know that you should have a low molar solubility but...

When adding a common ion I know that you should have a low molar solubility but I got a high molar solubility 0.0376 and I was wondering what could be some reasons for me to get this? Could it be contamination of the solution?
For example, the original was Ca(OH)2 and I got a molar solubility of .022 and a Ksp of 4.26E-5
and when adding a common Ion CaCl2 I got a molar solubility of .0376

Can you please help me understand why i got these results and why they don't support Le Chateliers principle? Thank you I would really appreciate it.

Solutions

Expert Solution

Ca(OH)2-------->Ca⁺² + 2OH-

KSP= [Ca+2][OH-]²= 4.26*10-5

let x= molar solubility of Ca(OH)2, then[ Ca+2]=x and [OH-]= 2x

hence x*4x²= 4.26*10^-5, x= molar solubility = 0.022

when CaCl2 is added, this suppliments, Ca+2 hence

Ca+2= 0.022+x and [OH-]= 2x

KSp= (0.022+x)*4x²= 4.26*10^-5

when solved using excel, x= 0.01661

this is the solubility of Ca(OH)2 now. CaCl2 is more soluble in water than Ca(OH)2. This leads to precipitation of some of Ca(OH)2. The added CaCl2 suppliments of Ca+2. hence Ca+2 concentration increases. Since Solubility product does not change upon addition, less of OH- dissolves.

queen_honey_blossom answered 1 year ago

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