You are given a $1\mathrm{.}50-g$ mixture of sodium nitrate and sodium chloride. You dissolve this mixture into $100.mL$ of water and then add $38\mathrm{.}0mL$ of $0\mathrm{.}500M$ silver nitrate solution. You produce a white solid, which you then collect, dry, and measure. The white solid has a mass of $0\mathrm{.}641g.$

a$.$ If you had an extremely magnified view of the solution $($to the atomic$-$molecular level$),$ draw the species you would see in the beaker.

b$.$ Write the balanced net ionic equation for the reaction that produces the solid. Include phases and charges.

c$.$ Calculate the concentration of the sodium ion, the nitrate ion, and the chloride ion after the reaction goes to completion. Assume it is $100\%$ yield.