In the table at 6:40, it says that Calcium Sulfate is "fairly soluble" but isn't it an exception as Calcium Sulfate is actually insoluble in water. Amazing explanation though! Thanks.
Yes im also not sure on this? Do you perhaps have an answer for this yet, because if barium sulfate is soluble in water then it wouldnt produce a precitpitate
After research, it seems that the solubility of Group 2 sulphates depends on whether they are hydrated or not i.e. CaSO4 is insoluble but CaSO4.5H2O is soluble. However, for our exams this is irrelevant information, all you need to know is that as you go down Group 2 the solubility of sulphates decreases (and increases for hydroxides). Hope this helps!
@@THE_LAST_STYLEBENDER We know Barium sulphate is insoluble, that's why it's used as a positive result in the sulphate test. You would add HCl and BaCl2 to a solution with sulphate ions in, and then a (solid) white precipitate is formed which is BaSO4, which won't dissolve. Hope this answers your question!
Can someone answer my question? So I wanted to ask: Why would they use calcium carbonate to neutralise the sulphur dioxide when they can use calcium oxide because the second reaction doesn't produce carbon dioxide (which is also a pollutant)? I'd also think calcium oxide is easier and cheaper to create than calcium carbonate.
I like your video and I also have a question. Why’s is there 2 moles of H2O when calcium oxide reacts with sulfur dioxide and water when the equation is balanced with only one H2O on both sides. I just want to know if it needs to be there or it doesn’t really matter. Thnx
One question please as you said “as we go down the group the size of the metal ion increases but the number of delocalised electron remains same”....but barium has more number of electrons than magnesium innit?? Or its talking about the electron in outer shell...can you please explain that. Thanks!
7 years later and these videos are Still golden thanks man
Saving my A levels with this one
Love this! Please keep them coming for the rest of the topics with As and A2 . Thanks so much
The rest to be uploaded tonight for AQA. Have not got round to A2 will be done next year I'm afraid as I only do this part time.
Hi, quick question, do you think these revision videos go into enough detail or should I watch the subtopic videos for more depth of knowledge?
did you ever find out?
In the table at 6:40, it says that Calcium Sulfate is "fairly soluble" but isn't it an exception as Calcium Sulfate is actually insoluble in water.
Amazing explanation though! Thanks.
Yes im also not sure on this? Do you perhaps have an answer for this yet, because if barium sulfate is soluble in water then it wouldnt produce a precitpitate
After research, it seems that the solubility of Group 2 sulphates depends on whether they are hydrated or not i.e. CaSO4 is insoluble but CaSO4.5H2O is soluble.
However, for our exams this is irrelevant information, all you need to know is that as you go down Group 2 the solubility of sulphates decreases (and increases for hydroxides).
Hope this helps!
@@THE_LAST_STYLEBENDER We know Barium sulphate is insoluble, that's why it's used as a positive result in the sulphate test. You would add HCl and BaCl2 to a solution with sulphate ions in, and then a (solid) white precipitate is formed which is BaSO4, which won't dissolve.
Hope this answers your question!
You're an absolute legend!
wish i could hug this man for saving my grade
Heh. Pleased you found them helpful!
Have you got summarised videos like these for A2? They're so helpful honestly you've done a great job
why is chemistry so hard
Imo learning the content is hard but the exam questions aren't too hard if u memorise everything
Honest to god you have saved my a level you absolute legend
So helpful! The way you explain things just clicks and thanks for the exam tips
Happy to help!
Thank you so much these are the most useful resources I've come across!
Will you be doing powerpoint videos like these for Year 2 AQA?
at 15:45, what is the point of H2O in the first reaction if it isn't going to react, and could you write that reaction without water?
the CaCO3 and CaO needs to be dissolved in water
Can someone answer my question? So I wanted to ask:
Why would they use calcium carbonate to neutralise the sulphur dioxide when they can use calcium oxide because the second reaction doesn't produce carbon dioxide (which is also a pollutant)? I'd also think calcium oxide is easier and cheaper to create than calcium carbonate.
Will you also be uploading videos on some A2 topics?
Have not done slides for A2 will have to be done next year as I don't do this full time.
These are great. Will there be any organic/second year?
Organic uploaded tonight. A2 will have to be next year as I have not made anything for them. Only do this part time.
Do we need to know the equation for the removal of sulfur dioxide?
Thank you sir............................SO GOOD ........ EXCELLENT :D
My guy...grt job....im horrible at chem but with these...chem becomes easier...anxs
Thank you, this so detailed
You're very welcome!
I like your video and I also have a question. Why’s is there 2 moles of H2O when calcium oxide reacts with sulfur dioxide and water when the equation is balanced with only one H2O on both sides. I just want to know if it needs to be there or it doesn’t really matter. Thnx
Thanks you did well .
Amazing video thank you
Any chance of you making A2 versions of these this year? Thanks!
One question please as you said “as we go down the group the size of the metal ion increases but the number of delocalised electron remains same”....but barium has more number of electrons than magnesium innit?? Or its talking about the electron in outer shell...can you please explain that.
Thanks!
electrons in outer shell remains the same, as these are the only electrons that are delocalised
Hey very useful videos next up should be analytical techniques NMR IR etcc
No NMR but AS analytical techniques uploaded tonight.
Thank you for this
No problem 😊
Sir you are a lifesaver
thank you!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!
No problem. Pleased they are helping you!
Will there be anything based just for ocr a
Yes - OCR A will start tomorrow.
Is this edexcel syllabus?
nope this is for AQA bud
@@ironknight3041 i think u replied 4 yrs too late..
God bless you
Paper 1 in 2 days
legend