Question

Write the molecular and net ionic equations, including phases, for the reaction that occurs between aqueous sodium chloride, NaCl , and aqueous silver nitrate, AgNO 3 .

Answer 1

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 2

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)