Question

A solution containing cacl2 is mixed with a solution of li2c2o4 to form a solution that is 2.1 × 10-5 m in calcium ion and 4.75 × 10-5 m in oxalate ion. What will happen once these solutions are mixed?

Answer 1

The question is incomplete, complete question is:

A solution containing CaCl2 is mixed with a solution of Li2C2O4 to form a solution that is $2.1\times 10^{-5} M$ in calcium ion and $4.75\times 10^{-5} M$ in oxalate ion. What will happen once these solutions are mixed?

$K_{sp} (CaC_2O_4) = 2.3\times 10^{-9}$

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 = $[Ca^{2+}]=2.1\times 10^{-5} M$

Molar concentration of oxalate ions = $[C_2O_4^{2-}]=4.75\times 10^{-5} M$

ionic product of calcium oxalate in solution :

$K_i=2.1\times 10^{-5} M\times 4.75\times 10^{-5}M=9.975\times 10^{-10}$

Solubility product of calcium oxalate =$K_{sp}=2.3\times 10^{-9}$

Generally precipitation occurs when ionic product of substance in solution exceeds its solubility product.

$K_i>K_{sp}$ (precipitation occurs)

$K_i$ (non precipitation occurs)

$K_i$

$9.975\times 10^{-10}$

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.