qualitative analysis chemistry 12 ap. what is qualitative chemical analysis? it is a branch of...
TRANSCRIPT
What is Qualitative Chemical Analysis?
• It is a branch of chemistry that deals with the identification of elements or grouping of elements present in a sample.
• There are usually two types: qualitative inorganic analysis and qualitative organic analysis.
Identifying Ions
• We could use these rules to work out if hydroxides or chlorides are present in a solution. (What is one difference between the two ions?)
• To make life easier we could use a flow chart that shows the order that we need to do tests in order to eliminate possible ions
• These two flow charts divide all ions into two groups – anions and cations. Once we have identified one of the ions in a solution we need to identify the other. Can also use flame tests (for soluble metals), or other tests (see next page).
• Chemical tests are used to confirm that some anions (negative ions) or cations (positive ions) are present in an unknown, also to identify unknown gases or liquids.
• If you made a chemical reaction that produces fumes or gases or something you must have a way to identify this produced gas or fumes.
Flame Colours of Solutions
If a flame test produces one of the these colours, that ion is in the solution. Other
colors are possible, but these are the most common.
new sample
precipitate disappearsAl3+, Zn2+, Pb2+
precipitate remainsMg2+, Ba2+
add 2 drops, thenexcess NH3
solution
white precipitate formsAl3+, Zn2+, Pb2+, Mg2+,
Ba2+
add excessNaOH solution
add 2 drops of dilute NaOH
solution.
no precipitateNH4
+, Na+
add NaOH solution, heat, test gas with
red litmus.
litmus stays red Na+
litmus goes blue NH4
+
blue precipitate then deep blue solution
Cu2+
blue precipitate formsCu2+
brown precipitate formsAg+
brown precipitate then colourless solution Ag+
add 2 drops, then excess
NH3 solution
add 2 drops, then excessNH3 solution
orange precipitate formsFe3+
green precipitate formsFe2+
white precipitate formsAl3+, Pb2+
white precipitate forms and disappears, Zn2+
add dilute H2SO4 solution
colourless solutionAl3+
white precipitatePb2+
add dilute H2SO4 solution
colourless solutionMg2+
white precipitateBa2+
add 2 drops KSCN solution
dark red solution confirms Fe3+
Identifying Cations: NH4+, Na+, Mg2+, Ag+, Fe2+, Fe3+, Cu2+, Al3+, Pb2+, Zn2+, Ba2+
new sample
newsample
newsample
newsample
new sample
Identifying Cations I
• Use the cation flowchart to identify the cation used below:
Add NaOH Add KSCN
Identifying Cations II
• Use the cation flowchart to identify the cation used below:
Add NaOH Add NH3
Identifying Anions: CO32, Cl, I, S2, SO4
2, NO3, OH
litmus remains redSO4
2, Cl, I, NO3
add Ba(NO3)2 solution white precipitateSO4
2
add AgNO3 solution
no precipitate
precipitateCl, I
add dilute NH3 solution
precipitate disappearsCl
precipitate remainsI
no precipitateNO3
new sample
START: add red litmus
litmus goes blueOH, CO3
2
add dilute HCl solution
bubbles of gasCO3
2
no bubblesOH
Smelly bubblesS2
Identifying Anions I
• Use the anion flowchart to identify the anion used below:
Add Ba(NO3)2 Add AgNO3 Add NH3Add red litmus
Identifying Anions II
• Use the anion flowchart to identify the anion used below:
Add HClAdd red litmus
Solution Colors
Cations
Ions Symbol Colour
Chromium(II)Copper(II)
Cr2+
Cu2+
Blue
Chromium(III)Copper(I)Iron(II)Nickel(II)
Cr3+
Cu+
Fe2+
Ni2+
Green
Iron(III) Fe3+ Pale yellow
Cobalt(II)Manganese(II)
Co2+
Mn2+
Pink
Anions
Chromate CrO42- Yellow
Dichromate Cr2O72- Orange
Permanganate MnO42- purple
Some Precipitate Colours
Al3+, Mg2+,Ca2+ white
Cu2+ blue/greenFe2+ grey/greenFe3+ red/brown
Precipitated calcium carbonate (CaCO3)
Precipitated copper(II) hydroxide, Cu(OH)2
So How Do I Use Qualitative Analysis?
• Here is an example of a question:A sample of a solution of an unknown was treated with dilute HCl. The white precipitate formed was filtered and washed with hot water. A few drops of KI solution were added to the hot water filtrate and a bright yellow precipitate was produced. The white precipitate remaining on the filter paper was readily soluble in NH3 solution. What two ions could have been present in the unknown?(A) Ag+ and Hg2
2+
(B) Ag+ and Pb2+
(C) Ba2+ and Ag+
(D) Ba2+ and Hg22+
(E) Ba2+ and Pb2+
Ask yourself – what happens at each step?
Solution – Ag+ forms a precipitate with chlorides (AgCl), so what is the other metal? Think of a metal that would likely be insoluble with I- Pb2+ is a good choice because in our labs, it formed mostly yellow/orange precipitates.
Lab Procedures For Qualitative Analysis
Solution containing ions of all cation groups
Solution containing ions of remaining groups
Solution containing ions of remaining groups
Solution containing ions of remaining groups
Solution contains Na+, K+, NH4+ ions
+ HCl Precipitates: AgCl, Hg2Cl2, PbCl2
Precipitates: CuS, CdS, HgS, SnS, Bi2S3
Precipitates: CoS, FeS, MnS, NiS, ZnS, Al(OH)3, Cr(OH)3
+ H2S
+ NaOH
+ Na2CO3
filtration
filtration
filtration
filtration
Solution is now basic, so other S2- will precipitate
Precipitates: BaCO3, CaCO3, SrCO3