which equation represents the correct net ionic equation for the reaction between ca(oh)₂ and h₂so₄?\no h⁺ +…

Explanation:

Step1: Write the balanced molecular equation

$Ca(OH)_2(aq)+H_2SO_4(aq)\longrightarrow CaSO_4(s)+2H_2O(l)$

Step2: Write the complete ionic equation

$Ca^{2 +}(aq)+2OH^-(aq)+2H^+(aq)+SO_4^{2 -}(aq)\longrightarrow CaSO_4(s)+2H_2O(l)$

Step3: Identify spectator ions

$CaSO_4$ is a solid and $H_2O$ is a liquid, so they do not dissociate further. There are no spectator - ions in this reaction as $CaSO_4$ precipitates out. But if we consider the general concept of acid - base reactions and assume $CaSO_4$ is soluble (for the purpose of finding the net ionic equation for the acid - base part), the $Ca^{2+}$ and $SO_4^{2 -}$ are spectator ions. After canceling them out, the net ionic equation for the acid - base reaction (neutralization) is $2H^+(aq)+2OH^-(aq)\longrightarrow 2H_2O(l)$ which simplifies to $H^+(aq)+OH^-(aq)\longrightarrow H_2O(l)$.

Answer:

$H^++OH^-\longrightarrow H_2O$