Answer :
The question is incomplete, complete question is:
A solution containing CaCl2 is mixed with a solution of Li2C2O4 to form a solution that is [tex]2.1\times 10^{-5} M[/tex] in calcium ion and [tex]4.75\times 10^{-5} M[/tex] in oxalate ion. What will happen once these solutions are mixed?
[tex] K_{sp} (CaC_2O_4) = 2.3\times 10^{-9}[/tex]
Answer:
On mixing of both the solutions no precipitation will occur due to lower value of an ionic product of calcium oxalate from its solubility product.
Explanation:
Molar concentration of calcium ions = [tex][Ca^{2+}]=2.1\times 10^{-5} M[/tex]
Molar concentration of oxalate ions = [tex][C_2O_4^{2-}]=4.75\times 10^{-5} M[/tex]
ionic product of calcium oxalate in solution :
[tex]K_i=2.1\times 10^{-5} M\times 4.75\times 10^{-5}M=9.975\times 10^{-10}[/tex]
Solubility product of calcium oxalate =[tex]K_{sp}=2.3\times 10^{-9}[/tex]
Generally precipitation occurs when ionic product of substance in solution exceeds its solubility product.
[tex]K_i>K_{sp}[/tex] (precipitation occurs)
[tex]K_i<K_{sp}[/tex] (non precipitation occurs)
[tex]K_i<K_{sp}[/tex]
[tex]9.975\times 10^{-10}<2.3\times 10^{-9}[/tex]
On mixing of both the solutions no precipitation will occur due to lower value of an ionic product of calcium oxalate from its solubility product.