Jul 2, 2015

$K N {O}_{3}$ is Potassium Nitrate; $A g C l$ is Silver Chloride; That is a double replacement reaction.

#### Explanation:

Potassium Nitrate $K N {O}_{3}$ (aqueous solution) ; Silver Chloride $A g C l$ (solid) ; That is a double replacement reaction.

Jul 2, 2015

Those two compounds are called potassium nitrate and silver chloride.

#### Explanation:

You're dealing with two ionic compounds, the only difference between them being the fact that one is soluble in aqueous solution and the other one is insoluble.

More specifically, potassium nitrate, $K N {O}_{3}$, is soluble in aqueous solution and dissociates into potassium cations, ${K}^{+}$, and nitrate anions, $N {O}_{3}^{-}$.

$K N {O}_{3 \left(a q\right)} \to {K}_{\left(a q\right)}^{+} + N {O}_{3 \left(a q\right)}^{-}$

On the other hand, silver chloride, $A g C l$, is insoluble in aqueous solution. This means that it does not dissociate into silver cations, $A {g}^{+}$, and chloride anions, $C {l}^{-}$.

Silve chloride will actually precipitate out of solution if the right concentrations of silver cations and chloride anions are added together.

In fact, you can get these two products by mixing silver nitrate, $A g N {O}_{3}$, and potassium chloride, $K C l$, both soluble ionic compounds.

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

The net ionic equation will be

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