How do you balance this equation: AgNO_3 + NaCl -> AgCI + NaNO_3?

Sep 19, 2016

Explanation:

$A g N {O}_{3} \left(a q\right) + N a C l \left(a q\right) \rightarrow A g C l \left(s\right) \downarrow + N a N {O}_{3} \left(a q\right)$

Silver chloride will precipitate from solution as a curdy white because of its exceptional insolubility in water. The other materials are along for the ride and will remain in water as the aquated ions, $N {a}^{+} \left(a q\right)$, $N {O}_{3}^{-} \left(a q\right)$ etc.

We could write the business end of this equation, as the net ionic equation:

$A {g}^{+} \left(a q\right) + C {l}^{-} \left(a q\right) \rightarrow A g C l \left(s\right) \downarrow$

Note that as in all stoichiometrically balanced equations, (i) mass is conserved, and (ii) charge is conserved.