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Paper 5 Tips !! :)

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Thank you very much. It helped a lot but could you please explain in more detail the last bullet point on how to decide when the point of the temperature of the solution is to be taken please
It's not that hard. You simply have to follow the given guidelines. Anyway, I will list down the major points. :)

In this experiment, we are to show how the solubility of K(NO3)2 varies with temperature. From the previous part of the question you must already know that the temperature is the independent variable (since it's in our control), and the solubility is the dependent variable.
  • The first bullet point asks you that you should "ensure a wide range of results suitable for analysis by graph". They're basically asking what range are you going to provide for you independent variable. Basically when we conduct these experiments, we usually start from 0-100 degrees. The ms wants the candidates to give a range of at least 40 degrees.
  • The second bullet point wants to know what mass of K(NO3)2 and volume of what you should use. Remember the independent variable in this experiment is the temperature. So temperature is only variable you're allowed to change. ALL the other variables are to be kept in control (needs to be constant). So you need a constant mass of K(NO3)2 (say 2 g) and a constant volume of water. (around 100 cm^3)
  • The third one wants you to describe how you will "measure the amounts of the two reagents". This is an easy one. Measure the K(NO3)2 using a balance measuring up to 0.02g, and volume of water by a measruing cylinder measruing up to 1 cm^3
  • The fourth point: "heat the apparatus". You could describe how you could use a thermostatically controlled water bath. You also have to mention that you have to stir the solution (they already gave you a wire stirrer- a BIG clue)
  • In the fifth point, you need to describe what you would do. So say you heated the solution to 10 degrees- and after about 2-5 mins you took your boiling tube out, and filtered the solution and dried it (water and propanone), then you reweigh the remaining salt and subtract it from the initial mass. And you'll have your solubility of the solution for that particular temp. Do this for the rest of the values in your temp range.
Hope this helped! :)
 
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For the diagram:
finding-the-formula-of-copper-oxide-194.jpg

Replace the Copper with Lead though! :p

This is how you will heat the Lead oxides, with the excess hydrogen burning at the end of the tube. And instead of pipe to the gas tap, you should attach a syringe. And in another diagram on the same page, you should draw a a test tube, with a rubber bung, attached to the same syringe. In the contents of the tube, mention a gorup II metal (For eg: Mg) + a suitable acid, like HCl. This will liberate H2 gas into the syringe, which you will then attach to the apparatus shown above.
We can replace the test tube in which H2 is liberated with a conical flask right? because i realy don't like to draw apparatus in mid-air;)
 
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Ohh makes sense now. The bullet point in the question is kind of misleading. Anyway i get your point.
Thanks a lot..
Please pray for all of us. Insallah we will all be fine!
The mark scheme has four ways to explain it:


I used "Alternate 2" because I understand it the best. See, let's go back to what hypothesis that we're testing. We're testing the solubility of K(NO3)2 at different temperatures. So the fifth point asks at what point when the temperature be taken. Remember we used a thermostatically controlled water bath? What you could also do is you could heat using a bunsen burner to a certain temperature (say 10 degrees). Also remember that our initial mass of the salt was 2.00 g. So you heated the solution to 10 degrees (while stirring). And after that you filtered the solution, and you reweighed your residue, and say you had 1.80 g left. This means that only 0.20 g of the salt had dissolve. Then you try it again with 20 degrees, and the mass of your residue was 1.50g (0.50 g had dissolved).
 
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The mark scheme has four ways to explain it:


I used "Alternate 2" because I understand it the best. See, let's go back to what hypothesis that we're testing. We're testing the solubility of K(NO3)2 at different temperatures. So the fifth point asks at what point when the temperature be taken. Remember we used a thermostatically controlled water bath? What you could also do is you could heat using a bunsen burner to a certain temperature (say 10 degrees). Also remember that our initial mass of the salt was 2.00 g. So you heated the solution to 10 degrees (while stirring). And after that you filtered the solution, and you reweighed your residue, and say you had 1.80 g left. This means that only 0.20 g of the salt had dissolve. Then you try it again with 20 degrees, and the mass of your residue was 1.50g (0.50 g had dissolved).
How do heat the solution to 10^C? can you please elaborate on that? Nice answers though(y)
 
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and brother Ashique , the diagram u posted above.. it doesnt show the excess H2 is being taken care of... is that what the gas syringe is for?
 
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s11 :51 2c could some please picture or scan the graph for me ?! please thank u
 
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Isn't that wrong? The question asks you to draw a line of best fit. You drew a curve. :unsure:
Yeah.. but look at what the mark scheme says:)
And why is my diagram wrong? Can you please explain what excess gas burnt means?
Thanks.
 
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Friends can you please help me how to calculate solubility and molality. what are the formula to calculate these?
May you all get A's and A*.
 
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Friends can you please help me how to calculate solubility and molality. what are the formula to calculate these?
May you all get A's and A*.
solubility=( mass of solid/ mass of water ) x 100
molality= no of moles of solute dissolved in 1kg of water
 
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