what is the net ionic equation for the following reaction? h₂cro₄ + ba(oh)₂\nh₂cro₄⁻ + 2oh⁻ → cro₄⁻ +…

Explanation:

Step1: Write the complete ionic equation

$H_2CrO_4$ is a weak acid and does not fully dissociate. $Ba(OH)_2$ is a strong base and dissociates completely into $Ba^{2 +}$ and $2OH^-$. The reaction is $H_2CrO_4(aq)+Ba(OH)_2(aq)\rightarrow BaCrO_4(s) + 2H_2O(l)$. The complete ionic equation considering the dissociation of $Ba(OH)_2$ is $H_2CrO_4(aq)+Ba^{2+}(aq)+2OH^-(aq)\rightarrow BaCrO_4(s)+2H_2O(l)$.

Step2: Identify spectator ions

There are no spectator - ions in this reaction as $H_2CrO_4$ is a weak acid and $BaCrO_4$ is a solid precipitate. The net ionic equation is written by removing non - reacting species. Since $H_2CrO_4$ is weak, it is written as a whole unit. The net ionic equation is $H_2CrO_4 + 2OH^-\rightarrow CrO_4^{2 -}+2H_2O$. But among the given options, the closest correct one considering the way the options are presented (assuming some simplification or mis - writing in options) and the fact that we consider the acid - base reaction aspects, we first consider the dissociation of the acid in a more general sense for the reaction with the base. $H_2CrO_4$ can be thought of as providing $H^+$ in reaction with the base. The correct net ionic equation considering the reaction of acid and base components is $H_2CrO_4+2OH^-\rightarrow CrO_4^{2 -}+2H_2O$ which can be rewritten in a form similar to the options as $H_2CrO_4^- + 2OH^-\rightarrow CrO_4^-+2H_2O$ (there is a bit of incorrect charge notation in the options but conceptually this is the closest).

Answer:

$H_2CrO_4^- + 2OH^-\rightarrow CrO_4^-+2H_2O$