Question

1. NaCl(aq)+KNO3(aq)____

1. Then find the overall ionic equation

3. And then the net ionic equation

Answer 1

When solutions of sodium chloride and potassium nitrate are mixed, the equation for the hypothetical double displacement reaction is
NaCl + KNO3  KCl + NaNO3
(The formulas of the products are obtained by switching the ions.) We get the
hypothetical products by simply combining each positive ion with the other negative ion. But has there been a reaction? When we do the experiment we see no evidence of reaction. There is no precipitate formed, no gas evolved, and no obvious temperature change. Thus we must conclude that no reaction occurred. Both hypothetical products are
48
soluble salts, so the ions are still present in solution. We can say that we simply have a solution of the four kinds of ions, Na+, Cl-, K+, and NO3-.
The situation is best expressed by changing the equation to NaCl + KNO3  No reaction
The complete ionic equation for this reaction is:
Na+(aq) + Cl-(aq) + K+(aq) + NO3-(aq)  K+(aq) + Cl-(aq) + Na+(aq) + NO3-(aq) There is no net ionic equation for this reaction. Since all of the ions are spectator ions, they all cancel out.
Source: http://www.laney.edu/wp/cheli-fossum/files/2011/08/9-Double-Displacement-Reactions.pdf

Answer 2

I don't know why it put those symbols in there but click on the link, and example 2 (pg 48) is your exact reaction.