Sammy performed the following chemical reaction in a lab
Ag(NO3) (aqueous) + NaCl (aqueous) --> AgCl (s) + Na(NO3)(aqueous) where NO3 is the nitrate ion and Cl is chlorine.
If Sammy just leaves the reaction container out to evaporate the water, and then scrapes out the solid and obtains the mass of the solid formed, he will be obtaining the mass of
a. just the AgCl made
b. the AgCl and the NaNO3 made
c. the AgCl made, the NaNO3 made, and any excess reactant
Let me point out that [NO3]^- is the nitrate ion (you omitted the charge) and Cl is not chlorine but it is the chloride ion (Cl^-).
You will get the AgCl(s), the NaNO3(s) when the water is evaporated, and any of the AgNO3 or NaCl that was left over if they were not there in stoichiometry amounts when the reaction occured.