Question

Write a balanced molecular, ionic, and net ionic equation for the following reaction. Assume the reaction occurs in

Answer 1

Answer: The balanced molecular equation is:

$K_2(C_2O_4)(aq)+CaCl_2(aq)\rightarrow 2KCl(aq)+Ca(C_2O_4)(s)$

The ionic equation is:

$2K^+(aq)+C_2O_4^{2-}(aq)+Ca^{2+}(aq)+2Cl^-\rightarrow 2K^+(aq)+2Cl^-(aq)+Ca(C_2O_4)(s)$  

The net ionic equation:

$C_2O_4^{2-}(aq)+Ca^{2+}(aq)\rightarrow Ca(C_2O_4)(s)$

Explanation:

A double displacement reaction is one in which exchange of ions take place. The salts which are soluble in water are designated by symbol (aq) and those which are insoluble in water and remain in solid form are represented by (s) after their chemical formulas.

The balanced molecular equation is:

$K_2(C_2O_4)(aq)+CaCl_2(aq)\rightarrow 2KCl(aq)+Ca(C_2O_4)(s)$

Spectator ions are defined as the ions which does not get involved in a chemical equation or they are ions which are found on both the sides of the chemical reaction present in ionic form.

The ionic equation is:

$2K^+(aq)+C_2O_4^{2-}(aq)+Ca^{2+}(aq)+2Cl^-(aq)\rightarrow 2K^+(aq)+2Cl^-(aq)+Ca(C_2O_4)(s)$

The ions which are present on both the sides of the equation are potassium and chloride ions. and hence are not involved in net ionic equation.

The net ionic equation:

$C_2O_4^{2-}(aq)+Ca^{2+}(aq)\rightarrow Ca(C_2O_4)(s)$