How do you write the total ionic equation and net ionic equation for the reaction of silver nitrate and potassium chloride?

1 Answer
Feb 9, 2016

Answer:

Total ionic equation:
#Ag^(+)(aq) +NO_3^(-)(aq)+K^(+)(aq)+Cl^(-)(aq)->AgCl(s)+K^(+)(aq)+NO_3^(-)(aq)#

Net ionic equation: #Ag^(+)(aq)+Cl^(-)(aq)->AgCl(s)#

Explanation:

The reaction between silver nitrate #AgNO_3# and potassium chloride #KCl# is the following:

#AgNO_3(aq)+KCl(aq)->AgCl(s)+KNO_3(aq)#

During this reaction, a precipitate will form which is the silver chloride #AgCl#.

The total ionic equation would be:

#Ag^(+)(aq) +NO_3^(-)(aq)+K^(+)(aq)+Cl^(-)(aq)->AgCl(s)+K^(+)(aq)+NO_3^(-)(aq)#

The net ionic equation however, would be:

#Ag^(+)(aq)+Cl^(-)(aq)->AgCl(s)#

Notice, the spectator ions - which are the common ions in both sides - are removed from the net ionic equation.