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29 Nov 2019

Lead ions can be removed from solution by precipitation withsulfate ions. Suppose that a solution contains lead(II)nitrate.

1.

Write complete ionic equation to show the reaction of aqueouslead(II) nitrate with aqueous potassium sulfate to form solidlead(II) sulfate and aqueous potassium nitrate.

Express your answer as a chemical equation. Identify all of thephases in your answer.

2.

Write net ionic equation to show the reaction of aqueouslead(II) nitrate with aqueous potassium sulfate to form solidlead(II) sulfate and aqueous potassium nitrate.

Express your answer as a chemical equation. Identify all of thephases in your answer.

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Keith Leannon
Keith LeannonLv2
17 Dec 2019

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Related questions

Fill the questions according to Data Table 7-2

5. balanced formula equation: for each combination of solutions that produced new product. write correct chemical formulas for the new compounds that could form from the ions present. Indicate which of the new compunds is a precipitate. If no reaction occurs, write NR.

6. complete ionic equation: write complete ionic equations for the precipitation reactions that you observed. show the reactants as ions, the precipitate as a solid, and the spectator ions as unchanged. balance each equation for mass and change. the total charge should be zero on each side of the equation.

7. net ionic equation: write the net ionic equations for each reaction in the preceding question.


1. Write the net ionic equation for the precipitation of aluminum carbonate from aqueous solution:

2. Write the net ionic equation for the precipitation of aluminum sulfide from aqueous solution:

3. Consider the reaction when aqueous solutions of silver(I) nitrate and chromium(II) bromide are combined.

The net ionic equation for this reaction is:

4. Consider the reaction when aqueous solutions of aluminum chloride and iron(III) nitrate are combined.

The net ionic equation for this reaction is:

5. Consider the reaction when aqueous solutions of barium chloride and chromium(III) sulfate are combined.

The net ionic equation for this reaction is:

6. Consider the reaction when aqueous solutions of copper(II) sulfate and sodium nitrate are combined.

The net ionic equation for this reaction is:

7. Consider the reaction when aqueous solutions of silver(I) nitrate and potassium hydroxide are combined.

The net ionic equation for this reaction is:

8. Consider the reaction when aqueous solutions of potassium hydroxide and sodium nitrate are combined.

The net ionic equation for this reaction is:

9. Consider the reaction when aqueous solutions of iron(II) sulfate and ammonium phosphate are combined.

The net ionic equation for this reaction is:

10. Consider the reaction when aqueous solutions of potassium carbonate and sodium iodide are combined.

The net ionic equation for this reaction is:

11. Consider the reaction when aqueous solutions of aluminum sulfate and ammonium sulfide are combined.

The net ionic equation for this reaction is:

12. Consider the reaction when aqueous solutions of sodium sulfide and potassium nitrate are combined.

The net ionic equation for this reaction is:

13. Consider the reaction when aqueous solutions of silver(I) nitrate and potassium hydroxide are combined.

The net ionic equation for this reaction is:

14. Consider the reaction when aqueous solutions of ammonium sulfide and silver(I) sulfate are combined.

The net ionic equation for this reaction is:

15. In the laboratory you are given the task of separating Ag+ and Ba2+ ions in aqueous solution.

For each reagent listed below indicate if it can be used to separate the ions. Type "Y" for yes or "N" for no. If the reagent CAN be used to separate the ions, give the formula of the precipitate. If it cannot, type "No"

Y or N Reagent Formula of Precipitate if YES
1. KBr
2. Na2CO3
3. K2SO4

16. In the laboratory you are given the task of separating Ba2+ and Co2+ ions in aqueous solution.

For each reagent listed below indicate if it can be used to separate the ions. Type "Y" for yes or "N" for no. If the reagent CAN be used to separate the ions, give the formula of the precipitate. If it cannot, type "No"

Y or N Reagent Formula of Precipitate if YES
1. K2S
2. HBr
3. KOH

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