Enter the net ionic equation, including phases, for the reaction of AgNO3(aq) and KCl(aq).

Where is the NO3 and KCl?

To write the net ionic equation for the reaction between AgNO3(aq) and KCl(aq), we need to identify the dissociated ions and write the balanced equation.

The balanced equation for the reaction between AgNO3 and KCl is:

AgNO3(aq) + KCl(aq) -> AgCl(s) + KNO3(aq)

Now, let's break down the equation into ions to get the net ionic equation:

Ag+(aq) + NO3-(aq) + K+(aq) + Cl-(aq) -> AgCl(s) + K+(aq) + NO3-(aq)

In the net ionic equation, the spectator ions (ions that appear on both sides and do not participate in the reaction) are removed. In this case, K+ and NO3- are spectator ions.

Thus, the net ionic equation for the reaction between AgNO3(aq) and KCl(aq) is:

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

To write the net ionic equation for this reaction, we first need to write the balanced equation for the reaction between silver nitrate (AgNO3) and potassium chloride (KCl). Then, we can eliminate any spectator ions from the balanced equation to obtain the net ionic equation.

The balanced equation for the reaction is:

AgNO3(aq) + KCl(aq) -> AgCl(s) + KNO3(aq)

In this reaction, silver nitrate reacts with potassium chloride to form silver chloride (AgCl) and potassium nitrate (KNO3).

Now, let's identify the spectator ions. Spectator ions are ions that do not participate in the reaction and remain unchanged from the reactants to the products. In this case, the spectator ions are the potassium cation (K+) and the nitrate anion (NO3-).

So, we can eliminate the spectator ions from the equation to obtain the net ionic equation. The net ionic equation for this reaction is:

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

In the net ionic equation, we have eliminated the spectator ions (K+ and NO3-) and only included the ions that are actually involved in the reaction (Ag+ and Cl-). The Ag+ ions from AgNO3 and the Cl- ions from KCl combine to form solid silver chloride (AgCl).

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