Write the net ionic equation for silver nitrate and sodium chloride.
I only know how to do it when it deals with elements, not compound.
Ag+ (aq) 3NO3- (aq) 3Na+ (aq)3Cl- (aq) -> AgCl3 (s) 3Na+ 3NO3- (aq)
Net: Ag+ (aq) + 3Cl (aq) -> AgCl3 (s)
Most of the above is garbage. For solution.
AgNO3(aq) + NaCl(aq) ==> AgCl(s) + NaNO3
Then rewrite the molecular equation as ions if the molecules are ionic and soluble. If a solid, write it as the molecule. Add (aq) after each except AgCl.
Ag^+ + NO3^- + Na^+ + Cl^- ==>AgCl(s) + Na^+ + NO3^-
Now cancel the ions on each side that are common, in this case that will be NO3^- and Na^+.
And what is left is the net ionic equation.
Ag^+(aq) + Cl^-(aq) ==> AgCl(s)
My DAD is a scientist
To write the net ionic equation for the reaction between silver nitrate and sodium chloride, you first need to know the chemical formulas for each compound.
Silver nitrate has the chemical formula AgNO3, where Ag denotes silver and NO3 denotes the nitrate ion. Sodium chloride, on the other hand, has the chemical formula NaCl, where Na denotes sodium and Cl denotes chloride.
Now, let's break down the chemical equation into its ions. Silver nitrate dissociates in water into silver ions (Ag+) and nitrate ions (NO3-), while sodium chloride dissociates into sodium ions (Na+) and chloride ions (Cl-).
So, when silver nitrate and sodium chloride are mixed together in water, the net ionic equation can be written as follows:
Ag+(aq) + Cl-(aq) -> AgCl(s)
In this equation, (aq) represents the ions in an aqueous or dissolved state, and (s) represents the solid silver chloride precipitate formed.
It's important to note that the sodium ions and nitrate ions do not participate in any chemical reaction and remain as spectator ions in solution. This is why they are not included in the net ionic equation.