Answer:
Molecular equation: NaCl(aq) + AgNO₃(aq) → NaNO₃(aq) + AgCl(s)↓
Net ionic equation: Cl⁻(aq) + Ag⁺(aq) → AgCl (s)
Explanation:
We determine the reactants for the reaction:
NaCl and AgNO₃
In aqueous solutions, salts from nitrate are soluble (all soluble)
In aqueous solutions, salts from chloride can make precipitate (with Ag⁺, Pb²⁺ Hg²⁺, Cu²⁺)
We dissociate the reactants:
NaCl → Na⁺ + Cl⁻
AgNO₃ → Ag⁺ + NO₃⁻
Molecular equation: NaCl(aq) + AgNO₃(aq) → NaNO₃(aq) + AgCl(s)↓
To build the net ionic equation we pick up the ions:
Na⁺(aq) + Cl⁻(aq) + Ag⁺(aq) + NO₃⁻(aq) → NO₃⁻(aq) + Na⁺(aq) + AgCl (s)
Those who are solid must be written as a compound, the ions are only from aq solutions. As we find NO₃⁻ and Na⁺ in both sides of the reactions we named them, spectators ions because they do not react. We can cancel them, so the net ionic equation is: Cl⁻(aq) + Ag⁺(aq) → AgCl (s)
Answer:
Molecular equation: NaCl(aq) + AgNO3(aq) → AgCl(s) + NaNO3(aq)
net ionic equation: Ag+(aq) + Cl-(aq) → AgCl(s)
Explanation:
Step 1: Data given
aqueous sodium chloride = NaCl(aq)
aqueous silver nitrate = AgNO3(aq)
Step 2: The (un)balanced equation
NaCl(aq) + AgNO3(aq) → AgCl(s) + NaNO3(aq)
This equation is already balanced
Step 3: The net ionic equation
The net ionic equation, for which spectator ions are omitted - remember that spectator ions are those ions located on both sides of the equation - will , after canceling those spectator ions in both side, look like this:
Na+(aq) + Cl-(aq) + Ag+(aq) + NO3-(aq) → AgCl(s) + Na+(aq) + NO3-(aq)
Ag+(aq) + Cl-(aq) → AgCl(s)
