what is the net ionic equation for the reaction of aqueous sodium chloride with aqueous silver nitrate.
Write out the general equation:
NaCl(aq) + AgNO3(aq) ---> AgCl(s) + NaNO3(aq)
Write out the total ionic equation. If it's a strong electrolyte, it is written as ions. If not, it's written as a molecule. NaCl, AgNO3, and NaNO3 are strong electrolytes, so they're written as ions. AgCl is a nonelectrolyte, so it's written as a molecule.
Na+(aq) + Cl-(aq) + Ag+(aq) + NO3-(aq) ---> AgCl(s) + Na+(aq) + NO3(aq)
Remove spectator ions and write the net ionic equation.
Ag+(aq) + Cl-(aq) ---> AgCl(s)
Oh, I'm ready for this one! Brace yourself for some clown-level chemistry humor. Here's the net ionic equation for the reaction:
NaCl(aq) + AgNO3(aq) → AgCl(s) + NaNO3(aq)
And the clown twist, "Looks like Na and Ag had a little party, but things got salty when Cl joined! Silver chloride, the life of the party, formed, while sodium nitrate played it safe in the aqua zone. Better be careful with sodium chloride, it tends to make things a bit Agg or Clowned!"
To determine the net ionic equation for the reaction between aqueous sodium chloride (NaCl) and aqueous silver nitrate (AgNO3), we first need to write the balanced equation for the reaction.
The balanced equation for the reaction between NaCl and AgNO3 is:
NaCl(aq) + AgNO3(aq) → AgCl(s) + NaNO3(aq)
Now, let's write the ionic equation by representing the soluble compounds as separate ions:
Na+(aq) + Cl-(aq) + Ag+(aq) + NO3-(aq) → AgCl(s) + Na+(aq) + NO3-(aq)
In this reaction, the Ag+ and Cl- ions form a precipitate (AgCl), which means they are involved in the net ionic equation. The Na+ and NO3- ions remain as spectator ions and do not participate in the net ionic equation.
The net ionic equation for the reaction is:
Ag+(aq) + Cl-(aq) → AgCl(s)
Finally, the net ionic equation represents only the species that are directly involved in the chemical reaction, in this case, the formation of AgCl.
To determine the net ionic equation for the reaction between aqueous sodium chloride (NaCl) and aqueous silver nitrate (AgNO3), we need to first write the complete ionic equation and then cancel out the spectator ions.
Step 1: Write the balanced molecular equation:
NaCl(aq) + AgNO3(aq) → AgCl(s) + NaNO3(aq)
Step 2: Write the ionic equation by separating the soluble compounds into their respective ions:
Na+(aq) + Cl-(aq) + Ag+(aq) + NO3-(aq) → AgCl(s) + Na+(aq) + NO3-(aq)
Step 3: Identify the spectator ions, which are the ions that appear on both sides of the equation without undergoing any change. In this case, Na+ and NO3- are present on both sides and do not participate in the reaction.
Step 4: Write the net ionic equation by canceling out the spectator ions:
Ag+(aq) + Cl-(aq) → AgCl(s)
The net ionic equation of the reaction between aqueous sodium chloride and aqueous silver nitrate is Ag+(aq) + Cl-(aq) → AgCl(s).