I balanced the equation:
HBr(aq) +NH3(aq)->NH4Br
I need to find the ionic equation
and
the net ionic equation
For the balanced equation remember to put (aq) behind NH4Br, and the ionic equation is wrong....
To find the ionic equation and net ionic equation of a chemical reaction, you need to determine the state of each species in the reaction. The state is usually represented as (s) for solid, (l) for liquid, (g) for gas, and (aq) for aqueous solution. In an ionic equation and net ionic equation, only the species that dissociate into ions in water are included.
Let's start with the balanced equation:
HBr(aq) + NH3(aq) → NH4Br
To write the ionic equation, you need to break down the soluble ionic compounds into their constituent ions. In this case, NH4Br will dissociate into NH4+ and Br- ions. However, HBr and NH3 are both molecular compounds and do not dissociate in water, so they will remain in their molecular form.
Ionic equation:
HBr(aq) + NH3(aq) → NH4+(aq) + Br-(aq)
Next, to write the net ionic equation, you remove the spectator ions. Spectator ions are those that appear on both sides of the equation and do not participate in the reaction. In this case, NH4+ is a spectator ion because it is present on both sides.
Net ionic equation:
HBr(aq) + NH3(aq) → Br-(aq)
Therefore, the ionic equation is HBr(aq) + NH3(aq) → NH4+(aq) + Br-(aq), and the net ionic equation is HBr(aq) + NH3(aq) → Br-(aq).
H^+(aq) + NH3 ==> NH4^+(aq)
H^+(aq) + Br^-(aq) + NH3 ==> NH4^+(aq) + Br^-(aq)
Cancel ions common to both sides. In this case, cancel the Br^-.