T&P Analysis Flashcards

1
Q

How is the Rf value in chromatography calculated?

A

dspot / dsolvent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Describe how paper chromatography is carried out.

A
  • 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
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What is thin layer chromatography used to do?

A
  • Separate small quantities of organic compounds
  • Purify them / check their purity
  • Follow the progress of a reaction
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

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.

A
  • Organic compounds have different affinities for a given solvent
  • So are carried through the chromatography (silica / alumina) plate at different rates
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Describe how thin layer chromatography is carried out.

A
  • 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
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What can be used to locate spots in TLC?

A
  • UV lamps
  • Iodine
  • Ninhydrin
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

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.

A
  • 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)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

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.

  1. Why is their teacher disappointed?
  2. How could their method be improved?
A
  1. Large % uncertainty due to small titre (21%)
  2. Use more dilute thiosulfate or more concentrated iodate(V)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What are iodine-thiosulfate titrations used for?

A

Finding the concentration of a strong enough oxidising agent to oxidise I- to I2.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

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-

  1. Balance equations A and B.
  2. 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.
A

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.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

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

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)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

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.

A
  • 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
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

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.

A
  • 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
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

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.
A
  • 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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q
A
  1. 2 x 0.05 x 100 / 24.7 = 0.4%
  2. Student A correct; titre unaffected since mol Sr(OH)2 unaltered
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q
  • What 2 instruments can be used to determine the concentration of a coloured solution?
  • Distinguish between the two.
A
  • Colorimeter (gives data for restricted wavelengths of light due to specific filters)
  • Visible spectrophotometer (gives data for any visible wavelength)
17
Q

Describe how a colorimeter would be used to measure the concentration of a sample.

A
  • Select filter of complementary colour to sample
  • Zero colorimeter with tube of pure solvent (usually water)
  • Prepare range of 5+ standard test solutions, with concentrations above and below that of sample
  • Measure absorbance of standard solutions + sample of unknown concentration
  • Plot calibration curve of concentration against absorbance for samples of known concentration
  • Read off unknown concentration
18
Q

A student has test tubes containing solutions of 0.010 mol dm-3, 0.020 mol dm-3, 0.030 mol dm-3, and 0.040 mol dm-3 of MnO4- ions.

How could they use a colorimeter to measure the concentration of a solution containing approximately 0.025 mol dm-3 MnO4- ions?

A
  • MnO4-(aq) is purple so select yellow (complementary colour) filter
  • Zero colorimeter with tube of pure water
  • Use colorimeter to measure absorbance of all MnO4- solutions, including sample of unknown concentration
  • Plot calibration curve of concentration against absorbance for samples of known concentration
  • Read off unknown concentration
19
Q

The standard electrode potential of a half-cell may be measured by connecting it to which two types of half-cell?

A
  • Standard hydrogen half-cell
  • Calibrated reference half-cell (calibrated with H2 half-cell)
20
Q

Draw a diagram of the apparatus used to determine the standard electrode potential of a Zn(s)/Zn2+(aq) half-cell.

A

Also: H2 half-cell electrode should be labelled as Pt(s) or graphite

21
Q

Describe a technique which could be used to determine the standard potential of a Fe3+(aq)/Fe2+(aq) half-cell.

A
  • Set up Fe3+/Fe2+ half-cell:
    • Use platinum / graphite electrode
    • Fe3+ and Fe2+ in solution
  • Set up standard hydrogen half-cell:
    • Use platinum / graphite electrode
    • H+ in solution
    • Feed H2(g) at 100 kPa into solution using porous glass tube covering electrode
  • Concentrations of solutions all 1 mol dm-3
  • Temperature of solutions and H2(g) 298 K
  • Connect solutions with salt bridge
  • Connect electrodes with high-resistance voltmeter
  • Record voltmeter reading (switch connections if negative)
  • This gives Ecell and therefore Eo (since Eo for H2 half-cell = 0 V)
22
Q
A

Advantage: portable / no gas involved

Disadvantage: mercury is toxic / poisonous

Ignore references to cost. Mercury being “harmful” is too vague

23
Q

Before using a pH probe (pH electrode), it must be calibrated for which two quantities?

A
  • Temperature
  • pH
24
Q

Describe how to calibrate a pH probe.

A
  • Rinse probe with distilled water
  • Immerse in buffer solution of pH 7.00
  • Connect to meter
  • Calibrate for temperature (if not automatic)
  • Set meter pH reading to 7.00
  • Re-rinse probe
  • If intending to measure a wide range of pH values, calibrate with acidic + alkaline buffer solutions too
25
Q

Describe the test for unsaturation. State what would be observed as a positive result.

A
  • Shake sample with bromine water
  • Positive result: brown bromine water decolourises
26
Q

Draw a diagram of the apparatus used to crack a hydrocarbon vapour over a heated catalyst.

A

Also label delivery tube

27
Q

Describe how you would crack an alkane over a heated catalyst.

A
  • Soak mineral wool with alkane + place at end of horizontally mounted boiling tube
  • Add catalyst (porcelain chips) to middle of tube, leaving space for passage of gas
  • Place bung in tube
  • Fill collection trough with water
  • Add several inverted test tubes
  • Connect to boiling tube with delivery tube
  • Use Bunsen flame to heat catalyst
  • Collect gas in tubes, replacing + corking when full. Discard first tube; contains displaced air. Heat throughout - this prevents suck-back
  • Remove delivery tube from trough before stopping heating - this prevents suck-back
28
Q

A student cracked liquid paraffin over a heated catalyst and collected the gaseous product in several test tubes.

Explain how they could test whether they had produced an alkene from an alkane.

A
  • Shake liquid paraffin with bromine water: should remain brown
  • Shake gas in tubes with bromine water: brown solution should decolourise
29
Q

Name 5 methods of analysis which are used to measure rate of reaction.

A
  • Titration (redox / acid-base)
  • Colorimetry
  • pH measurement
  • Volume of gas evolved
  • Mass change
30
Q

How does quenching work?

A
  • Sample isolated from reaction mixture
  • Chemical added which stops reaction (e.g. neutralises a catalyst)
  • Sample titrated to find conc. of a reactant/product
31
Q

Name 3 methods of analysis which are used to determine the value of an equilibrium constant.

A
  • Titration (redox / acid-base)
  • Colorimetry
  • pH measurement
32
Q

Explain how the value of Kc can be found experimentally.

A
  • Record initial reactant concentrations
  • Allow mixture to reach equilibrium
  • Measure eq conc. of a reactant or product
  • Calculate eq conc. of other reactants + products using above + equation
  • Write expression for Kc then calculate value using eq concentrations. State with unit + temperature
33
Q

The reaction below is done at 298 K. The initial reactant concentrations are known.

  1. How would you find the concentration of ethanoic acid in the eq. mixture?
  2. How would you find an expression for Kc?
A
  1. Titrate a known volume of equilibrium mixture with standard NaOH solution

2.

  • Assume [CH3COOH]eq = [CH3CH2OH]eq
  • Let this = x
  • [CH3COOCH2CH3]eq and [H2O]eq must equal initial conc - x
  • Let initial concentrations respectively be y and z
  • Kc = x2 / (y - x)(z - x) at 298 K (no unit)
34
Q

Describe how you would determine the solubility product, Ksp, of a soluble salt.

A

Prepare a saturated solution:

  • Swirl salt into conical flask containing warm distilled water until no more dissolves
  • Cool
  • Check there is undissolved solid at bottom of flask; if not, repeat first step
  • Filter

Measure temperature (Ksp is temperature-dependent)

Find concentration of one of the dissolved ions (method depends: e.g. titration, colorimetry)

Use equation to determine concentration of other ion

Calculate Ksp, giving unit + temperature

35
Q

Describe how you could determine the value of Ksp for calcium hydroxide at 298 K.

A

Prepare a saturated solution:

  • Swirl Ca(OH)2 into conical flask containing warm distilled water until no more dissolves
  • Cool
  • Check there is undissolved solid at bottom of flask; if not, repeat first step
  • Filter

Titrate known volume of filtrate with hydrochloric acid. Calculate [OH-]

[Ca2+] = [OH-] / 2

Ksp = [Ca2+][OH-]2, in mol3 dm-12 at 298 K