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
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