(Solved): Consider the following reaction: NH3(aq)+HNO3(aq)NH4NO3(aq) Generally the extent of ...

Consider the following reaction: ${\mathrm{NH}}_3(\mathrm{aq})+{\mathrm{HNO}}_3(\mathrm{aq})\to {\mathrm{NH}}_4{\mathrm{NO}}_3(\mathrm{aq})$ Generally the extent of a reaction like this example can be controlled by mixing two or more aqueous solution each containing one of the reagents. We will soon compute the extent of reaction using stoichiometry. For now, let's concern ourselves with the concentrations of the spectator ion(s). If we assume that the volume does not change appreciably by mixing the two solution from the sum of the volumes, or by the reaction taking place, then the concentration(s) of the spectator ion(s) after mixing and before the reaction takes place can be computed by dilution, and this(these) concentration(s) will be the same after the reaction "is over". Calculate the concentration of the spectator ion if $58.95\mathrm{mL}$ of a $0.06465\mathrm{mol}{\mathrm{L}}^{-1}$ ammonia solution is mixed with $129.0\mathrm{mL}$ of a $0.09839\mathrm{mol}{\mathrm{L}}^{-1}$ solution of nitric acid. $[\text{ Spectator ion }]=||\mathrm{mol}{\mathrm{L}}^{-1}$