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True False Hydroxide, carbonate, and phosphate are always spectator ions.
True False Ammonium, sodium, and nitrate are all spectator ions.
True False In 1M ammonium hydroxide solution, hydroxide can react with some cations to form precipitates.
True False Ammonium nitrate will react with sodium carbonate to form sodium nitrate (a precipitate).
True False If you mix potassium iodide and silver nitrate the precipitate that forms will be potassium nitrate.

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Trinidad Tremblay
Trinidad TremblayLv2
17 Dec 2019

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Related questions

The lab is for CHEM II and it is taken out of a lab paq. Beloware the materials used.


Classify your ions according to the following three groups.

Several of the cations belong to more

than one group.

Group 1: Anions that WILL NOT PRECIPITATE in the presence of

silver nitrate.

Group 2: Anions that WILL PRECIPITATE in the presence ofsilver

nitrate and the resulting

precipitates WILL DISSOLVE upon acidification with nitric

acid.

Group 3: Anions that WILL PRECIPITATE in the presence ofsilver

nitrate and the resulting

precipitates WILL NOT DISSOLVE upon acidification withnitric

acid.

A. Write a net ionic equation for any reaction that producesa

precipitate.

B. Identify the anions that produce gas upon addition of

HCl.

C. Identify the anions that do not precipitate with silver

nitrate.

D. Identify the anions that react with silver nitrate toform

precipitates that dissolve when

acidified with nitric acid.

E. Identify the anions that react with silver nitrate toform

precipitates that do not dissolve when

acidified with nitric acid.

F. What simple test (other than a specific confirmationtest)

would distinguish between CO3 2-

and NO3 - ?


Here are the materials we used


1 Ammonium Molybdate, 0.2 M - 2 mL in Pipet

1 Aqueous Ammonia, 6 M, NH4OH - 4 mL in Pipet

1 Barium Chloride, 0.3 M - 2 mL in Pipet

1 Hydrochloric Acid, 6 M - 8 mL in Dropper Bottle

1 Nitric Acid, 6 M - 2.5 mL in Pipet

1 Organic Reagent - 1.5 mL in Vial

2 Pipet, Empty Short Stem

1 Silver Nitrate, 0.1 N - 6 mL in White Dropper

Bottle

1 Sodium Bromide, 0.1 M - 2.5 mL in Pipet

1 Sodium Carbonate, 0.25 M - 2.5 mL in Pipet

1 Sodium Chloride, 0.1 M - 2.5 mL in Pipet

1 Sodium Iodide, 0.1 M - 2.5 mL in Pipet

1 Sodium Phosphate, 0.1 M - 2.5 mL in Pipet

1 Sodium Sulfate, 0.1 M - 2.5 mL in Pipet

1 Sodium Sulfide, 0.1 M - 2.5 mL in Pipet

1 Unknown - 5 mL in Pipet

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

I tried posting this question before, but I didn't get a greatanswer. ÃPlease this is for the ANION test lab NOT the CATIONtest. Thank you!

The lab is for CHEM II and it is taken out of a lab paq. Below arethe materials used.


Classify your ions according to the following three groups.

Several of the cations belong to more

than one group.

Group 1: Anions that WILL NOT PRECIPITATE in the presence of

silver nitrate.

Group 2: Anions that WILL PRECIPITATE in the presence of silver

nitrate and the resulting

precipitates WILL DISSOLVE upon acidification with nitric

acid.

Group 3: Anions that WILL PRECIPITATE in the presence of silver

nitrate and the resulting

precipitates WILL NOT DISSOLVE upon acidification with nitric

acid.

A. Write a net ionic equation for any reaction that produces a

precipitate.

B. Identify the anions that produce gas upon addition of

HCl.

C. Identify the anions that do not precipitate with silver

nitrate.

D. Identify the anions that react with silver nitrate to form

precipitates that dissolve when

acidified with nitric acid.

E. Identify the anions that react with silver nitrate to form

precipitates that do not dissolve when

acidified with nitric acid.

F. What simple test (other than a specific confirmation test)

would distinguish between CO3 2-

and NO3 - ?


Here are the materials we used


1 Ammonium Molybdate, 0.2 M - 2 mL in Pipet

1 Aqueous Ammonia, 6 M, NH4OH - 4 mL in Pipet

1 Barium Chloride, 0.3 M - 2 mL in Pipet

1 Hydrochloric Acid, 6 M - 8 mL in Dropper Bottle

1 Nitric Acid, 6 M - 2.5 mL in Pipet

1 Organic Reagent - 1.5 mL in Vial

2 Pipet, Empty Short Stem

1 Silver Nitrate, 0.1 N - 6 mL in White Dropper

Bottle

1 Sodium Bromide, 0.1 M - 2.5 mL in Pipet

1 Sodium Carbonate, 0.25 M - 2.5 mL in Pipet

1 Sodium Chloride, 0.1 M - 2.5 mL in Pipet

1 Sodium Iodide, 0.1 M - 2.5 mL in Pipet

1 Sodium Phosphate, 0.1 M - 2.5 mL in Pipet

1 Sodium Sulfate, 0.1 M - 2.5 mL in Pipet

1 Sodium Sulfide, 0.1 M - 2.5 mL in Pipet

1 Unknown - 5 mL in Pipet

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