Question

part: 1 / 2
part 2 of 2
write the net ionic equation for the precipitation reaction in part 1. remember to include the proper physical states and charges of ions.

Explanation:

To solve this, we need the precipitation reaction from Part 1 (which isn't provided here). However, a general example of writing a net ionic equation for a precipitation reaction (e.g., reaction between silver nitrate and sodium chloride) is as follows:

Step 1: Write the balanced molecular equation

For example, if Part 1 was $\ce{AgNO3(aq) + NaCl(aq) -> AgCl(s) + NaNO3(aq)}$

Step 2: Write the total ionic equation

Break soluble ionic compounds into ions:
$\ce{Ag^+(aq) + NO3^-(aq) + Na^+(aq) + Cl^-(aq) -> AgCl(s) + Na^+(aq) + NO3^-(aq)}$

Step 3: Cancel spectator ions (ions present on both sides)

Spectator ions here are $\ce{Na^+}$ and $\ce{NO3^-}$.

Step 4: Write the net ionic equation

$\ce{Ag^+(aq) + Cl^-(aq) -> AgCl(s)}$

Since the specific reaction from Part 1 is not given, you would follow these steps with the reactants/products from Part 1:

1. Identify the precipitate (insoluble solid) from the reaction.
2. Write the total ionic equation by dissociating soluble compounds.
3. Eliminate spectator ions.
4. Write the net ionic equation with correct states ($\ce{(aq)}$ for ions in solution, $\ce{(s)}$ for the precipitate) and charges.

If you provide the reaction from Part 1, I can help write the exact net ionic equation.

Answer:

To solve this, we need the precipitation reaction from Part 1 (which isn't provided here). However, a general example of writing a net ionic equation for a precipitation reaction (e.g., reaction between silver nitrate and sodium chloride) is as follows:

Step 1: Write the balanced molecular equation

For example, if Part 1 was $\ce{AgNO3(aq) + NaCl(aq) -> AgCl(s) + NaNO3(aq)}$

Step 2: Write the total ionic equation

Break soluble ionic compounds into ions:
$\ce{Ag^+(aq) + NO3^-(aq) + Na^+(aq) + Cl^-(aq) -> AgCl(s) + Na^+(aq) + NO3^-(aq)}$

Step 3: Cancel spectator ions (ions present on both sides)

Spectator ions here are $\ce{Na^+}$ and $\ce{NO3^-}$.

Step 4: Write the net ionic equation

$\ce{Ag^+(aq) + Cl^-(aq) -> AgCl(s)}$

Since the specific reaction from Part 1 is not given, you would follow these steps with the reactants/products from Part 1:

1. Identify the precipitate (insoluble solid) from the reaction.
2. Write the total ionic equation by dissociating soluble compounds.
3. Eliminate spectator ions.
4. Write the net ionic equation with correct states ($\ce{(aq)}$ for ions in solution, $\ce{(s)}$ for the precipitate) and charges.

If you provide the reaction from Part 1, I can help write the exact net ionic equation.