Aqueous solutions of ammonium iodide and lead (II) nitrate are mixed. Precipitate: Chemical Equation: Complete lonic Equation: Net ionic Equation:
Aqueous solutions of ammonium iodide and lead (II) nitrate are mixed. Precipitate: Chemical Equation: Complete lonic Equation: Net ionic Equation:
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Predict the precipitates formed (if any) from the reactions shown. Then write a balanced chemical
equation, a balanced complete ionic equation, and balanced net ionic equation. If no reaction takes place, write “no reaction.”
Please solve and explain. Thank you.
![### Reaction of Ammonium Iodide and Lead (II) Nitrate
**Aqueous solutions of ammonium iodide and lead (II) nitrate are mixed.**
- **Precipitate:**
The formation of a precipitate can be observed when these solutions are mixed. A solid compound will emerge as a result of the reaction.
- **Chemical Equation:**
The balanced chemical equation for the reaction is:
\[
2 \text{NH}_4\text{I (aq)} + \text{Pb(NO}_3)_2 \text{ (aq)} \rightarrow \text{PbI}_2 \text{ (s)} + 2 \text{NH}_4\text{NO}_3 \text{ (aq)}
\]
- **Complete Ionic Equation:**
The complete ionic equation shows all the soluble ionic compounds dissociated into their respective ions:
\[
2 \text{NH}_4^+ \text{ (aq)} + 2 \text{I}^- \text{ (aq)} + \text{Pb}^{2+} \text{ (aq)} + 2 \text{NO}_3^- \text{ (aq)} \rightarrow \text{PbI}_2 \text{ (s)} + 2 \text{NH}_4^+ \text{ (aq)} + 2 \text{NO}_3^- \text{ (aq)}
\]
- **Net Ionic Equation:**
The net ionic equation removes the spectator ions and shows only the species involved in the formation of the precipitate:
\[
\text{Pb}^{2+} \text{ (aq)} + 2 \text{I}^- \text{ (aq)} \rightarrow \text{PbI}_2 \text{ (s)}
\]
This net ionic equation illustrates the main chemical change: the formation of lead(II) iodide precipitate.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe6119d99-d423-4375-907f-5db89cfc0f1d%2Fcbee2209-58c5-46eb-a94b-73ccb2a309d2%2F4vjgssx_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Reaction of Ammonium Iodide and Lead (II) Nitrate
**Aqueous solutions of ammonium iodide and lead (II) nitrate are mixed.**
- **Precipitate:**
The formation of a precipitate can be observed when these solutions are mixed. A solid compound will emerge as a result of the reaction.
- **Chemical Equation:**
The balanced chemical equation for the reaction is:
\[
2 \text{NH}_4\text{I (aq)} + \text{Pb(NO}_3)_2 \text{ (aq)} \rightarrow \text{PbI}_2 \text{ (s)} + 2 \text{NH}_4\text{NO}_3 \text{ (aq)}
\]
- **Complete Ionic Equation:**
The complete ionic equation shows all the soluble ionic compounds dissociated into their respective ions:
\[
2 \text{NH}_4^+ \text{ (aq)} + 2 \text{I}^- \text{ (aq)} + \text{Pb}^{2+} \text{ (aq)} + 2 \text{NO}_3^- \text{ (aq)} \rightarrow \text{PbI}_2 \text{ (s)} + 2 \text{NH}_4^+ \text{ (aq)} + 2 \text{NO}_3^- \text{ (aq)}
\]
- **Net Ionic Equation:**
The net ionic equation removes the spectator ions and shows only the species involved in the formation of the precipitate:
\[
\text{Pb}^{2+} \text{ (aq)} + 2 \text{I}^- \text{ (aq)} \rightarrow \text{PbI}_2 \text{ (s)}
\]
This net ionic equation illustrates the main chemical change: the formation of lead(II) iodide precipitate.
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