Chemistry Question, Help please.

To calculate % error do: (0.5x2/25) x 100

And what does it mean by what piece of apparatus would have reduced this % error?

Tbh I’m not entirely sure I was thinking along the lines of a pipette of sorts as you could measure more accurately. I’m only a student myself so I didn’t wanna give any info I don’t fully know 😂

You still helped tho, Have you completed this Assignment (Unit 22.1 Preparing Substances)

Also I’ve just re-read the Q and have seen you have only used the measuring cylinder for one measurement. Formula for % error is: (error x No. measurements taken divided by the measurement taken) x100. So it’s 0.5/25 x 100, sorry for that haha

Alright thanks a lot Might have different Questions later lol

Ok well I do the IB and this question has some errors in it I feel, it should be saying uncertainty and not error. Assuming this was a mistake. To calculate percentage uncertainty you do the uncertainty divided by the amount measure * 100 so here it will be (0.5/25)*100 = +-2%. To reduce percentage uncertainty, you could either increase the amount of volume used (according to the % uncertainty equation) or use a measuring cylinder with a lower uncertainty. Once again, I am just a student so I may be wrong.

No problem! Ill be happy to help where I can haha

OK last thing i need help with and im Done with this Assignment the rest i have completed

Add a spatula measure of the copper(11) carbonate and stir with a glass rod

Q3. Note down your observations

a) ________________________________________________________________
b) ________________________________________________________________
c) ________________________________________________________________

Keep on adding more solid copper in small amounts with stirring until all the sulphuric acid has reacted

Q4 What observations did you make to decide that the reaction was complete
d) ________________________________________________________________
e) ________________________________________________________________

Using a fluted filter paper, filter the reaction mixture directly into a crystallising dish. Wash the beaker with a little water and rinse the solid with a little water, all washing collected in the crystallising dish.
It is normal to heat this solution to evaporate some of the water the heat is continued until the volume is reduced to about a half the original volume and then crystal are obtained on cooling.


Q5 Why is the solution not heated until all the water has evaporated? ___________________



We are simply going to leave the solution for a week to allow the water to evaporate and the crystals to form.
After a week pour of any excess solution in the evaporating dish and dry the crystals on absorbent paper and the weigh using a watch glass.

Q6 Describe the crystals you have obtained ______________________________________________

Umm are you not meant to acc do the exp & then note down your observations?😂

I know but I wasn’t in when they conducted the experiment .... 😂

Do you have any ppl in ur class you can ask aha?
Ok well for Q4 it’d be that effervescence stops and the solid stops dissolving. And I know that for Q6 the crystals should be blue as Cu2+ forms blue coloured compounds

Alright I’ll see for the results, you’ve helped a lot thanks a lot

Add a spatula measure of the copper(11) carbonate and stir with a glass rod

Q3. Note down your observations

Should have a green powder (CuCO3) reacting with H2SO4 to turn solution from colourless to blue because CuSO4 is formed and that is blue. Should've seen a gas being let off through bubbles (CO2) and fizzing i suppose.(All guesses from equation you gave). Beaker gets hotter because it is exothermic?

Keep on adding more solid copper in small amounts with stirring until all the sulphuric acid has reacted

Q4 What observations did you make to decide that the reaction was complete
No more bubbling, no more fizzing? Temperature began to decrease? Something to do with green powder (CuCO3) just sinking or not reacting idk.

Using a fluted filter paper, filter the reaction mixture directly into a crystallising dish. Wash the beaker with a little water and rinse the solid with a little water, all washing collected in the crystallising dish.
It is normal to heat this solution to evaporate some of the water the heat is continued until the volume is reduced to about a half the original volume and then crystal are obtained on cooling.


Q5 Why is the solution not heated until all the water has evaporated? No clue


We are simply going to leave the solution for a week to allow the water to evaporate and the crystals to form.
After a week pour of any excess solution in the evaporating dish and dry the crystals on absorbent paper and the weigh using a watch glass.

Q6 Describe the crystals you have obtained blue solid? lol