Using the balanced reaction, enter the formula, charge(if any), and state of the species (exclude H2O) in solution if Ba(NO3)2(aq) reactant is present in stoichiometric excess. Separate your answers by comma.
NaCl(aq) + Ba(NO3)2(aq) → NR
I think the question wants you to show the ions formed.
Na^+(aq) + Cl^-(aq) + Ba^+2(aq) + 2NO3^-(aq) ==> NR
To determine the formula, charge (if any), and state of the species involved in the reaction between NaCl(aq) and Ba(NO3)2(aq), we need to refer to a solubility table to determine if the compounds are soluble or insoluble in water.
In this case, NaCl(aq) is soluble in water and dissociates into Na+ and Cl- ions:
NaCl(aq) → Na+(aq) + Cl-(aq)
Using the same logic, Ba(NO3)2(aq) is also soluble in water and dissociates into Ba2+ and 2NO3- ions:
Ba(NO3)2(aq) → Ba2+(aq) + 2NO3-(aq)
Since Ba(NO3)2 is present in stoichiometric excess, it means that there is an excess of Ba2+ ions. Therefore, Ba2+(aq) is a spectator ion and does not participate in the reaction.
Consequently, the net ionic equation would be formed by combining the dissociated species that actively participate in the reaction:
Na+(aq) + Cl-(aq) + 2NO3-(aq) → NR
Thus, the formula, charge (if any), and state of the species (excluding H2O) in solution when Ba(NO3)2(aq) is present in stoichiometric excess are:
Na+(aq) - Sodium ion, charge +1, in aqueous solution
Cl-(aq) - Chloride ion, charge -1, in aqueous solution
NO3-(aq) - Nitrate ion, charge -1, in aqueous solution
Note that "NR" represents the non-reactive product.