Question

1. what is the net ionic equation for the reaction represented by this equation?

agno₃(aq) + nacl(aq) → agcl(s) + nano₃(aq)
options:
na⁺(aq) + no₃⁻(aq) → na⁺(aq) + no₃⁻(aq)
ag⁺(aq) + no₃⁻(aq) + na⁺(aq) + cl⁻(aq) → agcl(s) + na⁺(aq) + no₃⁻(aq)
agno₃(aq) + nacl(aq) → agcl(s) + nano₃(aq)
ag⁺(aq) + cl⁻(aq) → agcl(s)

Explanation:

Step1: Identify Strong Electrolytes

First, we recognize that \( \text{AgNO}_3 \), \( \text{NaCl} \), and \( \text{NaNO}_3 \) are strong electrolytes and will dissociate completely in aqueous solution. \( \text{AgCl} \) is a precipitate (solid) and does not dissociate.
So, dissociate the strong electrolytes:
\( \text{AgNO}_3(aq)
ightarrow \text{Ag}^+(aq) + \text{NO}_3^-(aq) \)
\( \text{NaCl}(aq)
ightarrow \text{Na}^+(aq) + \text{Cl}^-(aq) \)
\( \text{NaNO}_3(aq)
ightarrow \text{Na}^+(aq) + \text{NO}_3^-(aq) \)
\( \text{AgCl}(s) \) remains as is.

Step2: Write the Total Ionic Equation

Substitute the dissociated forms into the original equation:
\( \text{Ag}^+(aq) + \text{NO}_3^-(aq) + \text{Na}^+(aq) + \text{Cl}^-(aq)
ightarrow \text{AgCl}(s) + \text{Na}^+(aq) + \text{NO}_3^-(aq) \)

Step3: Cancel Spectator Ions

Spectator ions are ions that appear on both sides of the equation. Here, \( \text{Na}^+(aq) \) and \( \text{NO}_3^-(aq) \) are spectator ions. Cancel them:
After canceling, we get: \( \text{Ag}^+(aq) + \text{Cl}^-(aq)
ightarrow \text{AgCl}(s) \)

Answer:

\( \text{Ag}^+_{(aq)} + \text{Cl}^-_{(aq)}
ightarrow \text{AgCl}_{(s)} \) (corresponding to the option: \( \text{Ag}^+_{(aq)} + \text{Cl}^-_{(aq)}
ightarrow \text{AgCl}_{(s)} \))