# Predict the products of the following reactions. If no reaction occurs, write “NR” for No Reaction. Do not worry about balancing the equation?

## May 25, 2016

Here's what I got.

#### Explanation:

You can predict if single replacement reactions will take place by using the metal reactivity series.

In general, a metal that is higher in the reactivity series will displace a metal that is lower in the reactivity series. In your case, aluminium, $\text{Al}$, is actually higher in the reactivity series than silver, $\text{Ag}$, which means that silver cannot displace aluminium from aliminium chloride, ${\text{AlCl}}_{3}$.

Therefore, you will have

$\text{AlCl"_ (3(aq)) + "Ag"_ ((s)) -> "N.R.}$

The second reaction will take place because hydrobromic acid, $\text{HBr}$, a strong acid, will react with sodium hydroxide, $\text{NaOH}$, a strong base, to produce aqueous sodium bromide and water.

${\text{HBr"_ ((aq)) + "NaOH"_ ((aq)) -> "NaBr"_ ((aq)) + "H"_ 2"O}}_{\left(l\right)}$

In this case, you're dealing with a neutralization reaction that basically looks like this

overbrace("H"_ 3"O"_ ((aq))^(+))^(color(blue)("coming from HBr")) + overbrace("OH"_ ((aq))^(-))^(color(green)("coming from NaOH")) = 2"H"_ 2"O"_((l))

The third reaction will take place because it results in the formation of silver chloride, $\text{AgCl}$, an insoluble solid that precipitates out of solution.

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

This is a double replacement reaction for which the net ionic equation looks like this

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

Silver chloride is a white insoluble solid that precipitates out of solution. 