# Question #f4231

Oct 9, 2014

${\text{AgNO"_text(3(aq]) + "HCl"_text((aq]) -> "AgCl"_text((s]) + "HNO}}_{\textrm{3 \left(a q\right]}}$

#### Explanation:

To write the complete ionic equation:

• Break all soluble strong electrolytes (compounds with (aq) beside them) into their ions
• indicate the correct formula and charge of each ion
indicate the correct number of each ion
write (aq) after each ion
• Bring down all compounds with (s), (l), or (g) unchanged.

The molecular equation is

${\text{AgNO"_text(3(aq]) + "HCl"_text((aq]) -> "AgCl"_text((s]) + "HNO}}_{\textrm{3 \left(a q\right]}}$

How did I get this equation? Consider each reactant or product separately:

$\text{1 mole}$ of ${\text{AgNO}}_{3}$ contains $\text{1 mole}$ of ${\text{Ag}}^{+}$ and $\text{1 mole}$ of ${\text{NO}}_{3}^{-}$ ions.

${\text{Ag"_text((aq])^(+) + "NO"_text(3(aq])^(-) + "H"_text((aq])^(+) + "Cl"_text((aq])^(-) -> "AgCl"_text((s]) darr + "H"_text((aq])^(+) + "NO}}_{\textrm{3 \left(a q\right]}}^{-}$

The net ionic equation is

${\text{Ag"_text((aq])^(+) + "Cl"_text((aq])^(-) -> "AgCl}}_{\textrm{\left(s\right]}} \downarrow$