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Write a balanced equation for the double-replacement precipitation reaction described, using the smallest possible integer coefficients. A precipitate forms when aqueous solutions of lead (II) nitrate and sodium hydroxide are combined. Be sure to include states such as (s) or (aq). + +

Write a balanced equation for the double-replacement precipitation reaction described, using the smallest possible integer coefficients. A precipitate forms when aqueous solutions of lead (II) nitrate and sodium hydroxide are combined. Be sure to include states such as (s) or (aq). + +

Chemistry
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
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**Double-Replacement Precipitation Reaction** --- **Objective:** Write a balanced equation for the double-replacement precipitation reaction described, using the smallest possible integer coefficients. --- **Description:** A precipitate forms when aqueous solutions of lead(II) nitrate and sodium hydroxide are combined. --- **Instructions:** **Be sure to include states such as (s) or (aq).** --- **Diagram:** Below is a visual representation of the double-replacement reaction: \[ \text{Pb(NO}_3\text{)}_2 \, (\text{aq}) + 2 \, \text{NaOH} \, (\text{aq}) \rightarrow \text{Pb(OH)}_2 \, (\text{s}) + 2 \, \text{NaNO}_3 \, (\text{aq}) \] In this reaction, lead(II) nitrate reacts with sodium hydroxide to form lead(II) hydroxide, a solid precipitate, and sodium nitrate in aqueous form. The states of each compound are indicated in parentheses. ---
Transcribed Image Text:**Double-Replacement Precipitation Reaction** --- **Objective:** Write a balanced equation for the double-replacement precipitation reaction described, using the smallest possible integer coefficients. --- **Description:** A precipitate forms when aqueous solutions of lead(II) nitrate and sodium hydroxide are combined. --- **Instructions:** **Be sure to include states such as (s) or (aq).** --- **Diagram:** Below is a visual representation of the double-replacement reaction: \[ \text{Pb(NO}_3\text{)}_2 \, (\text{aq}) + 2 \, \text{NaOH} \, (\text{aq}) \rightarrow \text{Pb(OH)}_2 \, (\text{s}) + 2 \, \text{NaNO}_3 \, (\text{aq}) \] In this reaction, lead(II) nitrate reacts with sodium hydroxide to form lead(II) hydroxide, a solid precipitate, and sodium nitrate in aqueous form. The states of each compound are indicated in parentheses. ---
### Writing Net Ionic Equations for Reactions #### Instructions: 1. **Specifying States:** - Be sure to specify states such as (aq) for aqueous or (s) for solid. 2. **Leaving Boxes Blank:** - If a box is not needed, leave it blank. 3. **No Reaction:** - If no reaction occurs, leave all boxes blank and click on "submit". #### Example Problem: **Consider the reaction when aqueous solutions of lead(II) nitrate and sodium sulfide are combined. The net ionic equation for this reaction is:** [ ] + [ ] → [ ] + [ ] --- This prompt requires you to determine the net ionic equation for the reaction between lead(II) nitrate and sodium sulfide. When these solutions mix, lead(II) ions will react with sulfide ions to form a precipitate of lead(II) sulfide, while sodium and nitrate ions will remain in solution. The net ionic equation focuses only on the species that undergo a change. Remember: - Include the physical states (aq) or (s). - Use appropriate chemical notation to fill in the boxes. For example: \[ \text{Pb}^{2+} (\text{aq}) + \text{S}^{2-} (\text{aq}) \rightarrow \text{PbS} (\text{s}) \] Where: - Pb²⁺(aq) represents aqueous lead(II) ions, - S²⁻(aq) represents aqueous sulfide ions, and - PbS(s) represents solid lead(II) sulfide.
Transcribed Image Text:### Writing Net Ionic Equations for Reactions #### Instructions: 1. **Specifying States:** - Be sure to specify states such as (aq) for aqueous or (s) for solid. 2. **Leaving Boxes Blank:** - If a box is not needed, leave it blank. 3. **No Reaction:** - If no reaction occurs, leave all boxes blank and click on "submit". #### Example Problem: **Consider the reaction when aqueous solutions of lead(II) nitrate and sodium sulfide are combined. The net ionic equation for this reaction is:** [ ] + [ ] → [ ] + [ ] --- This prompt requires you to determine the net ionic equation for the reaction between lead(II) nitrate and sodium sulfide. When these solutions mix, lead(II) ions will react with sulfide ions to form a precipitate of lead(II) sulfide, while sodium and nitrate ions will remain in solution. The net ionic equation focuses only on the species that undergo a change. Remember: - Include the physical states (aq) or (s). - Use appropriate chemical notation to fill in the boxes. For example: \[ \text{Pb}^{2+} (\text{aq}) + \text{S}^{2-} (\text{aq}) \rightarrow \text{PbS} (\text{s}) \] Where: - Pb²⁺(aq) represents aqueous lead(II) ions, - S²⁻(aq) represents aqueous sulfide ions, and - PbS(s) represents solid lead(II) sulfide.
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