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

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Answer 1 · 2016-02-09T19:32:16

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

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

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.