The following chemical reaction takes place in aqueous solution:

Question

AgF(aq) + NaCl(aq) -> AgCI(s) + NaF(aq)
Write the net ionic equation for this reaction.

Answer 1

To write the net ionic equation for the reaction occurring in aqueous solution between AgF and NaCl, let's first break down each compound into its constituent ions:

1. \( \text{AgF (aq)} \) dissociates into \( \text{Ag}^+ (aq) \) and \( \text{F}^- (aq) \).
2. \( \text{NaCl (aq)} \) dissociates into \( \text{Na}^+ (aq) \) and \( \text{Cl}^- (aq) \).

The complete ionic equation, showing all the ions involved, is:

\[ \text{Ag}^+ (aq) + \text{F}^- (aq) + \text{Na}^+ (aq) + \text{Cl}^- (aq) \rightarrow \text{AgCl} (s) + \text{Na}^+ (aq) + \text{F}^- (aq) \]

Now, to find the net ionic equation, we need to remove the spectator ions. Spectator ions are those ions that appear on both sides of the equation and do not participate directly in the reaction. In this case, the spectator ions are \( \text{F}^- \) and \( \text{Na}^+ \).

Removing the spectator ions, we get the net ionic equation as:

\[ \text{Ag}^+ (aq) + \text{Cl}^- (aq) \rightarrow \text{AgCl} (s) \]

This equation represents the actual chemical change occurring in the solution, where silver ions (\( \text{Ag}^+ \)) react with chloride ions (\( \text{Cl}^- \)) to form solid silver chloride (\( \text{AgCl} \)).