Use the solubility rules to determine if the reaction will happen for the following unbalanced equation. Will the reaction take place? square If the reaction happens, label the solid (s) and aqueous (aq) products. If no reaction happens, choose (aq)for both. Na_(2)SO_(4)(aq)+CuCl_(2)(aq)arrow CuSO_(4)square vee NaClsquare

To determine if the reaction will take place, we need to apply the solubility rules for ionic compounds.<br /><br />Step 1: Identify the ions in the reactants.<br />In this case, the reactants are $Na_{2}SO_{4}(aq)$ and $CuCl_{2}(aq)$. The ions present are $Na^+$, $SO_{4}^{2-}$, $Cu^{2+}$, and $Cl^-$.<br /><br />Step 2: Apply the solubility rules.<br />According to the solubility rules, most sulfates ($SO_{4}^{2-}$) are soluble except for those of calcium, strontium, and barium. Most chlorides ($Cl^-$) are also soluble.<br /><br />Step 3: Determine if a reaction will occur.<br />Since both sulfates and chlorides are generally soluble, no precipitate will form in this reaction. Therefore, the reaction will not take place.<br /><br />Answer: No reaction will take place. Both products will be in the aqueous state: $Na_{2}SO_{4}(aq) + CuCl_{2}(aq) \rightarrow CuSO_{4}(aq) + NaCl(aq)$.