Question

Which of the following gives the net ionic reaction for the reaction used in this experiment?

Answer 1

Answer: Option (d) is the correct answer.

Explanation:

The given reaction will be as follows.

       $Ba(OH)_{2}(aq) + H_{2}SO_{4}(aq) \rightarrow BaSO_{4}(s) + 2H_{2}O(l)$

In the ionic form, the equation will be as follows.

           $Ba^{2+}(aq) + SO^{2-}_{4}(aq) \rightarrow BaSO_{4}(s)$ ........ (1)

           $H^{+}(aq) + OH^{-}(aq) \rightarrow H_{2}O(l)$ ............ (2)

Hence, for the net ionic equation we need to add both equation (1) and (2). Therefore, the net ionic equation will be as follows.

     $Ba^{2+}(aq) + SO^{2-}_{4}(aq) + H^{+}(aq) + OH^{-}(aq) \rightarrow BaSO_{4}(s) + H_{2}O(l)$        

Now, balancing the atoms on both the sides we get the net ionic equation as follows.

         $Ba^{2+}(aq) + SO^{2-}_{4}(aq) + 2H^{+}(aq) + 2OH^{-}(aq) \rightarrow BaSO_{4}(s) + 2H_{2}O(l)$