T&P Analysis Flashcards
How is the Rf value in chromatography calculated?
dspot / dsolvent
Describe how paper chromatography is carried out.
- Draw pencil (insoluble) line 1 cm from base of chromatography paper (stationary phase)
- Using capillary tubes, spot test mixture + pure reference samples along line
- Suspend plate in beaker containing solvent reaching max height 5 mm
- Cover with watch glass (prevents evaporation)
- Remove paper when solvent front nears the top; mark point reached + allow to dry
- Measure height of spots + calculate Rf values = dspot/dsolvent
- Match with those of known compounds in this solvent
What is thin layer chromatography used to do?
- Separate small quantities of organic compounds
- Purify them / check their purity
- Follow the progress of a reaction
Thin layer chromatography is used to:
- Separate small quantities of organic compounds
- Purify them / check their purity
- Follow the progress of a reaction
Describe the principle upon which this technique is based.
- Organic compounds have different affinities for a given solvent
- So are carried through the chromatography (silica / alumina) plate at different rates
Describe how thin layer chromatography is carried out.
- Draw pencil (insoluble) line 1 cm from base of silica (SiO2) / alumina (Al2O3) plate (stationary phase)
- Using capillary tubes, spot test mixture + pure reference samples along line
- Suspend plate in beaker containing solvent reaching max height 5 mm
- Cover with watch glass (prevents evaporation)
- Remove plate when solvent front nears the top; mark point reached + allow to dry
- Locate spots with UV lamp
- Measure height of spots + calculate Rf values = dspot/dsolvent
- Match with those of known compounds in this solvent
What can be used to locate spots in TLC?
- UV lamps
- Iodine
- Ninhydrin
Describe how you would carry out a titration to find the concentration of a sodium hydroxide solution, using 0.2 mol dm-3 ethanoic acid.
Describe how you would use the titre to calculate the concentration of the sodium hydroxide solution.
- Rinse + fill burette with CH3COOH(aq)
- Record initial reading to nearest 0.05 cm3
- Rinse + fill graduated pipette with NaOH(aq)
- Use pipette filler to add 25 cm3 to a conical flask
- Add indicator to flask
- Perform rough titration
- Repeat, adding acid dropwise when 1 cm3 below end-point
- Repeat to obtain 3 concordant titres within 0.1 cm3
- Calculate average titre
- [NaOH] = mol / volume = (0.2 x titre x 10-3) / (25 x 10-3)
A student performs a titration of sodium thiosulfate (in the burette) and potassium iodate(V) (in the conical flask) and gets a titre of 0.48 cm3.
- Why is their teacher disappointed?
- How could their method be improved?
- Large % uncertainty due to small titre (21%)
- Use more dilute thiosulfate or more concentrated iodate(V)
What are iodine-thiosulfate titrations used for?
Finding the concentration of a strong enough oxidising agent to oxidise I- to I2.
An iodine-thiosulfate titration can be used to find the concentration of a solution of chlorate(I) ions, which react as follows:
A: ClO- + I- + H+ →I2 + Cl- + H2O
B: S2O32- + I2 → I- + S4O62-
- Balance equations A and B.
- Describe how the titration would be carried out, but do not include details of the procedure. Refer to equations A and B in your answer. Include details of the observations which would be made.
1.
A: ClO- + 2I- + 2H+ →I2 + Cl- + H2O
B: 2S2O32- + I2 → 2I- + S4O62-
2.
- Add excess I-(aq) to ClO-(aq). Forms brown mixture since iodine is formed in A.
- Titrate I2 produced with thiosulfate ions. When mixture turns from brown to pale yellow, add a few drops of starch solution. End-point is when blue-black colour, due to iodine-starch complex, disappears, since all I2 has been reduced, as in B.
An iodine-thiosulfate titration can be used to find the concentration of a solution of chlorate(I) ions, which react as follows:
A: ClO- + 2I- + 2H+ →I2 + Cl- + H2O
B: I2 + 2S2O32- → 2I- + S4O62-
Describe how a titration would be carried out to find the concentration of a solution of chlorate(I) ions, using standard 0.1 mol dm-3 sodium thiosulfate solution. Include details of the observations which would be made.
A: ClO- + 2I- + 2H+ →I2 + Cl- + H2O
- Rinse + fill graduated pipette with ClO-(aq)
- Use pipette filler to transfer 25 cm3 to conical flask
- Add excess KI(aq)
- Add excess H2SO4(aq)
- Mixture turns brown since iodine forms
B: I2 + 2S2O32- → 2I- + S4O62-
- Rinse + fill burette with standard 0.1 mol dm3 S2O32-(aq)
- Run some out to remove bubbles in jet
- Record initial reading to nearest 0.05 cm3
- Place conical flask onto white tile
- Perform rough titration
- When mixture turns pale yellow, add a few drops of starch solution
- End-point is when mixture turns from blue-black, due to iodine-starch complex, to colourless
- Repeat to get accurate titres, adding dropwise when 1 cm3 below rough end-point
- Repeat to obtain 3 concordant titres within 0.1 cm3
- Calculate average titre
- [ClO-] = mol / vol = (0.1 x titre x 10-3 x 1/2) / (25 x 10-3)
The concentration of a solution of Fe2+ ions can be found by titration with a standard potassium manganate(VII) solution. Other than from the uncertainty in burette and mass balance readings, suggest potential sources of error in the prodedure.
- Loss of material during transfer between vessels
- Parallax error in reading burette, volumetric flask + pipette
- Drips inside burette increasing titre
- Random error in judging end-point; titre may be too small or large
A solution of Fe2+ ions is made up by dissolving a certain mass of thyme in water. Some of the solution formed is transferred to a conical flask.
A student wants to determine the iron content of thyme. They do this by finding the concentration of the Fe2+ solution, by titration with standard potassium manganate(VII) solution.
Describe how the percentage uncertainty of the method could be minimised.
- Use a greater mass of thyme, in order to:
- reduce % uncertainty in mass balance reading
- make Fe2+(aq) more concentrated, to achieve a larger titre, to reduce % uncertainty in burette reading
- Use more dilute manganate(VII) solution to achieve a larger titre, to reduce % uncertainty in burette reading
The concentration of a solution of Fe2+ ions can be found by titration with a standard potassium manganate(VII) solution.
- Describe how the titration would be carried out.
- State how the end-point can be recognised and explain why an indicator does not need to be added.
- Rinse + fill burette with standard MnO4-(aq)
- Rinse + fill graduated pipette with Fe2+(aq)
- Use filler to transfer 25 cm3 to conical flask
- Add excess H2SO4 to flask
- Titrate until pink colour remains due to excess MnO4-(aq); no indicator required
- Repeat to obtain 3 concordant results within 0.1 cm3
Don’t use HCl as easily oxidised to toxic Cl2
- 2 x 0.05 x 100 / 24.7 = 0.4%
- Student A correct; titre unaffected since mol Sr(OH)2 unaltered