40daysofCHEM 9.4.4 = Part 18

9.4.3 HS Questions Feedback

THE BIG ADVICE:

You need to get in the mindset and be hyperaware that that you need to distinguish yourself. No matter how much you know if you don’t include detail, address the verb, define terms etc, there is no way of distinguishing you from someone who knows nothing. Ask yourself – could someone who was trying to ‘wing it’ write my answer? What have I added that cannot be ‘winged’ that makes me stand out?

2001

Q13) Note – Barium sulphate ppt forms almost immediately – waiting will not make more precipitate

26a) Make your data points stand out. Not just tiny dots (but not huge blobs either)

Q15) The solubility rules are very simple and we have used them since yr 11. I am disappointed that anyone got this question wrong. And considering that our flowchart test for lead is to add chloride ions those who put A and D really need t ask if they are taking ownership of their learning in this subject.

2002

Q24) If asked to assess the impact of AAS always give an illustrative example/case study. Also note that it was more accurate than previous methods and say ‘eg gravimetric analysis’ thus could determine previously unknown roles of trace elements. Also always define key terms in questions. In this Q you had to define ‘trace element’. – NB because lead has NO biological function it is NOT a trace element. Being an assess you should have also had a judgement.

2003

27b) DEFINE KEY TERMS – Reliability – repeat with consistent results – was it repeated?... THEN go on to talk about other errors – excess Ba added?, acid dissolution?, washed and dried?. EVALUATE NEEDS A JUDGEMENT! If you don’t talk about reliability/repetition and just talk about error you are assessing validity/accuracy. Also – sulfates will ppt in all pH’s, it is only carbonates and phosphates that don’t ppt at low pH – hence low pH is idea if you only want to ppt sulfates.

28) Use a ruler to draw ONE straight line of best fit. And USE your graph to calculate concentrations. The whole point of AAS is accuracy. You don’t buy and multi million S AAS machine, go through the process of making an accurate calibration curve and testing your samples only to use your eye and make a rough guess about he concentration “About 5ppm”… To prove it was Sewage you have to state what the Cd was upstream and downstream of it and somehow show it cant be from the industrial plant.

2004

20) This  is a critical Q testing your understanding of AAS. The light source contains the metal being tested to produce the exact wavelength of light that will be absorbed by the sample (to increase accuracy and NB% absorbance proportional to conc). The flame atomises the sample o the atoms CAN absorb those unique wavelengths of its absorption spectrum (remember element only absorb emit their unique spectra when atomised).

20b) Again – define validity and reliability. Is testing from one sample (even if it is tested 5 time) really a reliable way of analysing a whole industrial site? Did they calculate the absorbance in a valid manner? Is AS itself a valid and reliable and accurate technique?

20c) If you write NH3 for the phosphate test give yourself a facepalm then go back and check our flowchart an flowchart equations VERY carefully. IF you used Ba io ns for both phosphate and sulphate without distinguishing them give yourself a facepalm (other hand). The whole point of ppt tests is to be unambiguous you can have a white Ba ppt signifying both sulfate ad phosphate unless you sy that the phosphate dissolves in acid but the sulphate ppt does not.

2005

Q25b) A chemical test  = a precipitation test (AAS is a physical test as it involves no chemical reactions). And while Cl- is OK a better one would be to add I- as it gives the distinctive ‘canary yellow’ ppt.

Q25c) The statement said ‘concentrations’ so your answer should have given an example concentration. And you justify the need to monitor BY showing how bad it is if it is in the body – ie it needs to be monitored to avoid these problems.

2006

Q25) You had to make estimates of concentration from the graph AND concentrations need units – ie ppm! Also – don’t say ‘approximately’ unless you know the data is very unreliable– it is AAS data – ay your results with conviction!

Q26b) To explain the order you should also say what would happen if the correct order was not used eg add Ag first and get a white ppt which could mean….?

2007

Q14) When electrons ‘fall back’ they EMIT light not absorb light and this is absorption spectroscopy. The light is NOT white light, it is the light from the spectral lamp.

17a) No matter how far you are through the course ALWAYS use the cross method to make sure your ionic formulae are correct. States DO matter. If they are solutions the reactants must be aqueous. In a one mark ‘write the equation’ question you will get ZERO if one state is wrong.

19b) Not much working was shown for this Q – very suspicious. If not showing mathematical working you need to show your explanation – ie X mg/L but the tablet was only in 100ml. Thus the mass would have been 1/10^th this value = 0.X mg in the tablet.

2009

Q24) This was a big Q for 5 marks, You needed to briefly intro the fact the elements have unique spectra, you needed to BRIEFLY outline the AAS process lamp, furnace, monochromator, detector, (WITH A DIAGRAM) CRITICAL to note that the % of light absorbed is proportional to conc. outline the calibration curve  then ID the fact that it is accurate then give an example of environmental monitoring – and NB the trace element ones are OK for environmental monitoring but ‘environmental monitoring’ in the HSC context usually means pollution – ie lead. If I was doing the HSC this is one of those Q that I would practise a few times as it covers the whole range of AAs concepts in one question.

2010

29a) Broken record time – DEFINE VALIDITY FIRST. All the SULFATE in the fertiliser was dissolved (NB they filter out the solids before adding Ba so clearly not all the fertilizer dissolved – but we only care that the sulphate dissolved). All the sulphate was ppt by excess Ba ions. All the ppt remained in the filter paper. The ppt and paper was fully rinsed. The ppt and paper was dried to constant mass. That no carbonate or phosphate ppts formed with Ba. Also – regardless of *that* years marking scheme – for three marks they could expect three validity issues.

2012

Q32) This is an excellent test of your data analysis and calculations skills. A LOT of solutions matched the Success One book very closely. THIS IS FINE as long as you are learning. This is another question that I would come back to a number o times to make sure I understood how to answer this type of question. Ie come back to it and try again without looking at your previous answer.

9.4.2 HSC Q Feedback

2001

Q9) Hmm a bad start. LCP ONLY relates to “position of equilibrium” ie the %conversion of reactants into products (ie yield). LCP DOES NOT EXPLAIN RATES OF REACTION. Rate of reaction is explained by referring to EA – the greater the proportion of particles with E > EA the greater the rate.

Q10) Look carefully. The second reaction is NOT equilibrium. It goes to completion regardless of what chemicals are added. Adding sodium sulfate will not changethe reactions (ie LCP does not apply). Also –sodium sulphate is a neutral salt. It will not change the acidity of the solution

Q24a) Ammonia is used as a cleaning agent and as a fertilizer (and was used as a refrigerant). Ammonia is used to make urea/fertilizer. Ammonia is used to make nitric acid which in turn is used to make explosives. This is picky but:

·        Nitric acid is not used IN explosives

·        Ammonia is not used IN explosives

·        Technically Ammonia is not used to make explosives

·        Nitric acid is used to manufacture explosives

Q24c) The most logical way to approach all Haber Q is to (once the equation and LCP etc definitions are done) is i) high P (for high yield AND rate), but P limits, ii) High temp for high rate (explain with EA), iii) Low temp for high yield(LCP) , iv) Compromise needed aided by a CATALYST (always mention!), v) Catalyst temp monitored, vi) Then condensing, recycling, gs monitoring (3:1 and O2, CO). This questions was asking you to go through i-iv

2002

Q14) Don’t forget that higher temperatures decrease yield (lower conc of NH3 at equilibrium) but increase rate (equilibrium conc reached sooner = steeper line at thestart).

2003

Q29) This is exactly the same as 2001 Q24c) above but you need to go i-vi including LCP and EA et all the way. It is important to note that

·        You CANNOT answer a Haber/LCP question without an equation. You SHOULD NOT answer any 3+ mark question without writing an equation.

·        high pressure will NOT ‘cause an explosion in the reaction vessel’. An explosion in the vessel would mean that a rapid exothermic reaction initiated (an explosion). Instead high pressure can burst/rupture the reaction vessel.

·        LCP DOES NOT explain rates of reaction

·        ALWAYS name the catalyst as iron, iron oxide or magnetite

·        Remember that the gas stream must be monitored for 1:3 N2:H2 ratio, O2 and CO

·        It is an EVALUTE – thus you need to conclude with a judgement – is it important to monitor….

2005

Q27b) Decreasing volume of the vessel increases the pressure on gases = increases concentration of gases. Each gas conc must jump by the same PERCENTAGE. So if hydrogen conc increases by half its value (1/2H on the pic below), then nitrogen and ammonia must jump by half their original value.

Once the equilibrium shifts, each gas must change according to their mole ratio in the equation Ie for every 1x change in mitogen there will be a 2x change in ammonia and 3x change in hydrogen.

When the Q asks you to explain CHANGES you need to explain ALL the changes ie why the initial spike of all three (increase P = increase conc.), why did ammonia rise and N and H fall (LCP) an why did they come back to  point where their conc. does not change (LCP, ie new equilibrium established).

2006

Q23b) Explain means ‘give reasons’, specifically ‘give chemical reasons’ – so you must use LCP to explain what happens to the OCl- ions, the position of equilibrium, the OH- conc. and thus what happens to the pH

Q24a) THE HABER PROCESS IS AN EQUILIBRIUM REACTION!!!!!!!!!!

Q24b) You should know that Germany was sourcing their nitrates from South America. You should note that the ammonia from the Haber process can be used to manufacture nitrates. Thus, it is important that you mention that ammonia is a raw material for the production of explosives and fertilizers. Also note that it did prolong the war (but not wi it for Germany = lots of death = bad) but in the immediate post war era the fertiizers allowed for increased nutrition and increase in would population.

2008

Q7) This is a strange one. But if you apply your Sherlock Holmes style multiple choice reasoning “When you have eliminated the impossible, whatever remains, however improbable must be the truth” We KNOW that catalysts do not effect equilibrium so it must be B-D, but which of those two are wrong?...

Q23) Again i) Increasing Pressure DOES increase rate of reaction (it increases the concentration of particles with E > EA thus leads to more successful collisions), ii) Even if the Q only said T and P, the fact that a magnetite CATALYST is used allows the temperature compromise – relatively low temp to keep yield acceptable while maintaining a high rate.

2009

Q23) Don’t forget that LCP states that if the conditions of equilibrium are changed the reaction shifts to counteract the change AND A NEW EQUILIBRIUM IS ESTABLISHED. Thus it is vital that you note a new equilibrium is established after each change (ie at 8, 12 and 16 min).The change at 14mi is a increase in volume (decrease in pressure). The drop in all their concentrations just reflects their sudden drop in concentration. THEN the LCP applies showing a small shift to the right before new equilibrium at 16 min.

2010

Q9) this was an interesting Q – just like Sherlock you have to go through each possibility and eliminate the impossible

Q18) This linked LCP and BL acid theory – i) to increase chromate conc do you want to add acid or base and then – which salt do you add?

2011

Q30) This reaction was supposed to be one you have never seen before. You need to apply your understanding of LCP and industrial chemistry (from the Haber topic) to solve it. Some tips: i) look at each equation separately as they are separate steps so each can be done under different conditions, ii) The first reaction, the900oC says that it must be done at 900oC (suggesting a very high activation energy) – so you have no choice on temperature – but what canyou do to pressure, removal of species?, ii) This is just like Haber – don’t forget to consider T, P and catalyst, removal? (but don’t have to know which catalyst), iii) what is different about this reaction. What is the one thing we have to maximise?

2012

Q16) Just like in2005Q27b) you have to be very careful with the relative size of changes in equilibrium graphs. These relative sizes relate to the mole ratio and thus you can determine which species is which.

 Q24) You had to go a couple of steps deep here. i) ammonia to urea/fertilizer to greater crop production nutrition and growth of world population. Ii) ammonia to nitric acid to explosives – used in mining and construction industries allowing for building projects and supplying raw materials for industries/modern world.

Experiment #19

The Method (s)

Determine the wt% sulfate in a fertilizer

PLAN 1

1)      Wear PPE – gloves and goggles.

2)      Wash beaker with distilled water to remove impurities, dry & weigh.

3)      Weigh crystals of fertilizer in the pre-weighed beaker.

4)      Weigh a filter paper.

5)      Dissolve some fertilizer crystals in some water.

6)      Add BaCl₂ solution to precipitate the sulfate as BaSO_{4 (s)}

7)      Use a filter funnel and the weighed filter paper to filter out the precipitate.

8)      Wash all precipitate from the beaker into the funnel with a wash bottle & distilled water

9)      Place the filter paper on a tray and place in an oven to dry.

10)   Weigh the dry precipitate and filter paper and subtract the original mass of filter paper to find the mass of precipitate

11)   Calculate the moles of precipitate and sulfate, the mass of sulfate and the wt% sulfate in the fertilizer via wt%_sulfate = m_sulfate/m_fertilzser x 100

12)   Repeat the experiment for reliability

PLAN 2

bold = adjustments to the plan. The changes made to minimise error are numbered. You need to explain the error that each is designed to overcome as part of Q2 of your discussion.

1)      Wear PPE – gloves and goggles.

2)      Wash beaker with distilled water to remove impurities, dry & weigh.

3)      Weigh three pre dried⁽¹⁾ filter papers on a watch glass⁽²⁾.

4)      Weigh 10g of fertilizer crystals into a clean dry beaker.

5)      Make a 250ml standard solution* of this fertilizer in nitric acid⁽³⁾.

6)      Use a volumetric pipette to transfer 10ml of the solution to a clean test tube.

7)      Add 0.25 mol/L BaCl_{2 (aq)} – until no more ppt formation is apparent. Let the precipitate settle 24hr. Add more BaCl_{2 (aq)} and repeat until no more ppt forms⁽⁴⁾.

8)      Use a filter funnel and the three⁽⁵⁾ pre-weighed filter papers to filter out the precipitate.

9)      Wash all precipitate from the beaker into the funnel with a wash bottle & distilled water

10)   Wash the ppt with water ⁽⁶⁾.

11)   Dry the filter papers and precipitate on the watch glass in an oven to constant mass⁽⁷⁾.

12)   Weigh the dry precipitate and filter paper and subtract the original mass of filter paper to find the mass of precipitate.

13)   Calculate the moles of precipitate and sulfate, the mass of sulfate and the wt% sulfate in the fertilizer via wt%_sulfate = m_sulfate/m_fertilzser x 100.

14)   Repeat the experiment for reliability.

* Ensure the correct steps are followed to ensure accuracy of measurement and concentration – see titration and standard solution experiment.

The equipment used

The precipitates in different stages of settling* (most to least settled) 

*sedimenting

RESULTS    

All tests had 10.00 g of fertilizer dissolved into a 250.0 mL standard solution. 10.00 mL of this standard was reacted with excess aqueous barium chloride to produce a barium sulfate precipitate which was weighed.

GROUP	Mass ppt (g)
A	0.25
A	0.23
A	0.26
A	0.11
A	0.16
B	0.26
B	0.39
B	0.08
B	0.24
C	0.43
C	0.62
C	0.65
C	0.51

CHEMICALS

A = Iron (II) Sulfate - hmmm

B = Magnesium Sulfate - hmmm

C = Potassium Sulfate - hooray!  

 

 

Summary Feedback

 

NOTE - AAS can ONLY be used for analysing metal ion conc. It cannot be used to analye sulphate ion conc

 

A) After 19 experiments you should know that you can’t skimp on safety. The danger of each chemical is distinct. Choose 1 Ba compound e.g. BaCl₂ and HNO₃ and specify the dangers (and precautions) for each. Don’t forget about disposal issues. ‘Take care’ is not sufficient instead say ‘wear gloves to avoid contact with skin’ ie say exactly what ‘taking care’ means

 

B) Make sure you look up a proper chemical definition of each term – use textbook? – many definitions given were too specific and thus not thorough. You need a valid, general definition for each term.

C) Detail, detail, detail – don’t just say the precipitate might pass through the filter paper – this is unusual – say why e.g. "The very fine nature of the BaSO₄ ppt means it can pass through the filter paper…this would lead to an underestimate of sulfate content". NB the MOST important issues to discuss are: adding acid, adding excess BaCl₂, filtering, washing, drying – be detailed for each.

 

D) In the conclusion, state the class average and the theoretically calculated value

 E) You must show working for your calculation of the theoretical wt% sulfate in the fertiliser. Make sure you use the results posted to the Blurg (above) for your calculations for the group wt %. Also don’t forget the fertiliser was ammonium sulfate NOT barium sulfate.

 F) This summary can be 2 pages!

 G) Reliability means repeated with consistent results. We repeated but were the results consistent (they were to an extent but were not perfect) – what were the main sources of error? Remember that assess means you need to introduce the concept first – ie DEFINE reliability & ditto when assessing validity

 H) Make sure your calculations are clearly set out. ie don’t just write "n = 3.02 / 2233.37….". Use subscripts "n_BaSO4 = 3.02/233.37…"

 

I) Nitric acid was used as it will dissolve any phosphates in the fertilizer and also any carbonates (which are converted to CO2 and bubble out of solution). Thus the only ions that will precipitate with the Barium ions will be sulfate ions. Thus we know the ppt will be BaSO4 only (ie carbonates and phosphates will NOT ppt in acidic conditions)

But NB sulfates WILL precipitate in acidic, neutral and basic conditions – see Expt #18 results!

J) Because we added nitric acid there will be nitrate ions (and because there might be phosphate, chloride, potassium, magnesium, ammonium etc ions from the fertilizer) in the solution. These ions will be in the water surrounding the wet ppt. Unless we wash them through the filter with extra water they will crystallise when we evaporate the water from the ppt and add to the mass of the ppt … UPDATE-  thank you to those that read this before posting but Don't take shortcuts. nitrate ions will not 'crystallize' upon evaporation. They will crystalise as a salt with some of the cations in the solution - eg excess barium ions, metal ions from the fertilizer etc.

K) There were 4 possible fertilizers to calculate the wt% sulfate for – don’t forget ammonium sulfate