which equation represents the correct net ionic equation for the reaction between ca(oh)₂ and h₂so₄?\nh⁺ +…

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

In this reaction, $CaSO_4$ is a solid and does not dissociate into ions in solution. There are no spectator - ions that cancel out on both sides of the complete ionic equation. But if we consider the general case of acid - base reactions where a soluble salt is formed and we assume $CaSO_4$ is soluble (for the purpose of finding the net ionic equation for the acid - base part), $Ca^{2+}$ and $SO_4^{2 -}$ would be spectator ions. The acid - base reaction is between $H^+$ from $H_2SO_4$ and $OH^-$ from $Ca(OH)_2$. The net ionic equation for the acid - base reaction is $2H^+(aq)+2OH^-(aq)\longrightarrow 2H_2O(l)$, which simplifies to $H^+(aq)+OH^-(aq)\longrightarrow H_2O(l)$.

Answer:

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