Enter the net ionic equation for the reaction of aqueous sodium chloride with aqueous silver nitrate.
I know the equation is AgNO3(aq)+NaCl(aq)---->NaNO3(aq)+AgCl(s)
Is Ag^+(aq)+ Cl^-(aq)--->AgCl(s) right?
That looks good to me.
NO3 is always soluble though. It doesn't mix with Na (which is also always soluble).
Yes, Ag^+(aq) + Cl^-(aq) → AgCl(s) is the correct net ionic equation for the reaction of aqueous sodium chloride with aqueous silver nitrate.
To obtain the net ionic equation, you need to first write the balanced molecular equation for the reaction and then identify the ions that are actively participating in the reaction.
The balanced molecular equation for the reaction of aqueous sodium chloride with aqueous silver nitrate is:
AgNO3(aq) + NaCl(aq) → NaNO3(aq) + AgCl(s)
Next, you break down the aqueous species (those that are soluble in water) into their individual ions:
Ag^+(aq) + NO3^-(aq) + Na^+(aq) + Cl^-(aq) → Na^+(aq) + NO3^-(aq) + AgCl(s)
From the above equation, you can see that the sodium ion (Na^+) and the nitrate ion (NO3^-) appear on the left side and right side of the equation, so they are spectator ions and can be removed from the equation.
Hence, the net ionic equation is:
Ag^+(aq) + Cl^-(aq) → AgCl(s)