The question is incomplete, complete question is:
A solution containing CaCl2 is mixed with a solution of Li2C2O4 to form a solution that is
in calcium ion and
in oxalate ion. What will happen once these solutions are mixed?
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 = ![[Ca^{2+}]=2.1\times 10^{-5} M](https://tex.z-dn.net/?f=%5BCa%5E%7B2%2B%7D%5D%3D2.1%5Ctimes%2010%5E%7B-5%7D%20M)
Molar concentration of oxalate ions = ![[C_2O_4^{2-}]=4.75\times 10^{-5} M](https://tex.z-dn.net/?f=%5BC_2O_4%5E%7B2-%7D%5D%3D4.75%5Ctimes%2010%5E%7B-5%7D%20M)
ionic product of calcium oxalate in solution :
![K_i=2.1\times 10^{-5} M\times 4.75\times 10^{-5}M=9.975\times 10^{-10}](https://tex.z-dn.net/?f=K_i%3D2.1%5Ctimes%2010%5E%7B-5%7D%20M%5Ctimes%204.75%5Ctimes%2010%5E%7B-5%7DM%3D9.975%5Ctimes%2010%5E%7B-10%7D)
Solubility product of calcium oxalate =
Generally precipitation occurs when ionic product of substance in solution exceeds its solubility product.
(precipitation occurs)
(non precipitation occurs)
![K_i](https://tex.z-dn.net/?f=K_i%3CK_%7Bsp%7D)
![9.975\times 10^{-10}](https://tex.z-dn.net/?f=9.975%5Ctimes%2010%5E%7B-10%7D%3C2.3%5Ctimes%2010%5E%7B-9%7D)
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.