Awesome vid! I'd just like to point out something to any student reading this. By using HCl or NHO3 (Nitric Acid) this removes ions,specifically carbonate ions. This is very important since *BaCO3* (Barium Carbonate) is *also a white ppt*, so its indistinguishable from BaSo4 (Barium Sulfate). So by acidifying it first it removes the carbonate ions so you know the white ppt formed is 100% BaSo4. :)
Thank you for your comment. But I still have a question CaCO3 + 2HCl -------) CaCl2 + H2O +CO2, so although the hydrochloric acid is removing the carbonate there is still Calcium chloride left. Does that not matter, and if not do you mind explaining why? Thank you :)
@@MrERintoul Thank you foryour video I still have a question if you don't mind answering ? CaCO3 + 2HCl -------) CaCl2 + H2O +CO2, so although the hydrochloric acid is removing the carbonate there is still Calcium chloride left. Does that not matter, and if not do you mind explaining why? Thank you :)
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I was getting grade Cs and Ds in Chemistry before I found your videos, now I'm getting As!! Thank you so much for taking the time to make them, they are helpful beyond belief! If I pass this A level it will be because of you!
Thank you, I like how you summed it up in such a short amount of time with everything we needed to know. I learnt more in those 15 minutes, than I did in like 3 hours of class and 2 hours of reading :) x
thanks you so much for all the videos, they make life lot easier only if teachers in college could make it so simple. thanks for all the effort in putting these together so close up to the exam, I'm sure every body will appreciate them.
Can you add what happens with magnesium and the extraction of titanium and CaO/CaCO3 in removing SO2 from flue gases? Thanks! Btw great vid really helpful for revision
I liked this video, will help many however there is one piece missing. I think you should've added the flame test of each element i.e. Magnesium turns white, Calcium turns brick-red, Strontium gives scarlet/ red colour and Barium gives an apple-green colour. Also, I think you've missed some part of the syllabus including reactions of group 2 with dilute acids, nitrates and carbonates and thermal decomposition of nitrates and carbonates.
Yash Verma Thanks for your comments - but I have a few of my own... Strictly speaking, I'm not sure that the white colour you see when burning a magnesium strip is classed as a flame test. My understanding is that magnesium ions in some sort of ionic compound will not actually give a colour when placed into a flame. Also, there is no requirement for flame testing in the AQA specification hence the reason that I didn't cover it... Again, those latter points are not required as per the AQA specification... I don't mind you leaving comments, and I'm always open to corrections when mistakes have been made, but it's really important that you are sure that there are mistakes before you try to point them out.
Could you go through the testing SO4 part again? Do you add the HCL first or the same time as the BaCl2? The equations does't make quite make sense to me either. The second one does about the formation of Barium Sulfate I understand that.
abdi hussein You would add the HCl first as it says in the video. The reason for the HCl is to remove anything that may interfere with the test, particularly something that would give a false positive. With regard to the equations, whilst I will try and help, you've been far too vague. What is it you don't understand?
hi would we need to know why Mg reacts differently with steam as opposed to liquid water? so for example could an exam ask "mg reacts with water differently when water is gas or liquid, why is this?" thanks for another great video :D
you havent mentioned about the use of magnesium in the extraction of titanium and that the use of calcium oxide and calcium carbonate to remove so2 from flu gases
On a resource given to me by my teacher it says that Magnesium does not react with cold water and only reacts with steam to form MgO but at 3:26 it's show to react with water to form Mg(OH)2, anyone know which is correct, or which AQA treats as correct, thanks for the video :)
Harry Daley I promise you that magnesium does react with cold water - although not a fast reaction, you can watch it occur in a lab! As far as the products that you mentioned, the hydroxide is formed when magnesium reacts with water yet the oxide is formed when it reacts with steam!
Didn't really like the layout of this vid. Quite unorganised. Would be better if you focused on Oxides, sulphates and carbonates separately and also trends would have been nice to go over
