She explains and breaks down the problems very clearly. With the emotion she puts into it - her facial expressions and voice inflections - she communicates so much more than you could get from just reading a textbook. Her videos would also be good for a non-native English speaker wanting to improve her English and learn chemistry at the same time.
Watching you from Iraq☺️ thank you so much for explaining this so clearly, our teacher hadn’t explained this but it came in one of the exams❤️ but I have one question, if it asks what does Hso4- act as? Can we say it can be a strong base, weak acid, and amphoteric?
Hi Clipstw! Thank you for watching. H2SO4 is a strong acid so it 100% ionizes. On the other hand H2SO3 is a weak acid and only partially ionizes. The HSO3- species is amphoteric. It is produced in the first deprotonation (loses 1st H+) which is a conjugate base, and is a reactant in the second deprotonation (loses the 2nd H+) which is an acid. I hope that helps!
Hello! I'm very confused by the acid/base theories. I have a few questions, if amphoteric species means a chemical that can behave both as an acid or a base then why can't that be everything? We can force the strong acid HCl to act as a base if we react it with a stronger acid making the HCl accept the H+ proton, doesn't that make HCl amphoteric? If this is true, then what is the point of saying something is amphoteric if literally, anything can be amphoteric? Does the definition of amphoteric apply and extend to Lewis acids too? And Arrhenius? or is it only defined using the Bronsted Lowry theory? Help!
An acid donates a H+ and a base accepts a H+. If a species can both accept and donate a H+ then it is amphoteric. Not all species can do both. I hope that helps! You do not see H2Cl in nature. Thanks!
@@OldSchoolChemistry But isn’t accepting an H+ or donating an H+ relative to the other chemical in the reaction? For example ammonia a base because it’s more basic than water; however, it’s perfectly possible (if very unusual) for ammonia to act as an acid. Are these definitions meant to be in relation to water?
@@Hassan-ow1qu You are correct that ammonia can donate a H+ to produce an amine. So, yes it can be classified as amphoteric. Not all chemical species can both donate and accept a H+. I would ask your professor how they expect you to answer on a test. Thanks!
@@OldSchoolChemistry Ah! Sorry Ma’am for asking so many questions. I’m new to acid/base theories and I find it very confusing due to it having more than one definition. To make things clear Ma’am, are we using Bronsted’s definition when talking about amphoteric species? And is donating H+ and accepting H+ here meant in normal conditions, right? So I might be talking about exceptions when I say everything can act as an acid/base depending on the reaction, hence everything can be amphoteric in certain specific conditions, but in standard conditions only few are considered amphoteric species and those are addressed in this video? Am I right? So these definitions are meant to be in relation with water because you can find water everywhere and it’s the most common solvent. Am I right? Correct me If I’m wrong. And I’m so sorry for disturbing, this question is stuck in my head and I need an answer. 😭
@@Hassan-ow1qu You are correct except in the statement that the definitions only apply to a chemical species reacting with water. Here is a Khan Academy summary that may help you. Your next step is to visit your chemistry teacher for further clarification. I hope that helps. Thanks! www.khanacademy.org/science/chemistry/acids-and-bases-topic/acids-and-bases/a/bronsted-lowry-acid-base-theory
what if only one product is formed? which is the conjugate acid and base? the example I'm talking about is Al(OH)3 + OH- ===> [ Al(OH)4 ]- great video btw, you're amazing at explaining things!!!
Hi Jimmy, identify if the reactant is accepting or donating electrons (acid or base). (It looks like you are dealing with Lewis acids/bases so the viewpoint is just slightly different.) The related species on the product side will then be the conjugate. Good luck!
She explains and breaks down the problems very clearly. With the emotion she puts into it - her facial expressions and voice inflections - she communicates so much more than you could get from just reading a textbook.
Her videos would also be good for a non-native English speaker wanting to improve her English and learn chemistry at the same time.
Wow! What a kind comment. Thank you for the positive feedback Keith. I appreciate you:)
Nice hair and face !
tf
Watching you from Iraq☺️ thank you so much for explaining this so clearly, our teacher hadn’t explained this but it came in one of the exams❤️ but I have one question, if it asks what does Hso4- act as? Can we say it can be a strong base, weak acid, and amphoteric?
Hi Clipstw! Thank you for watching. H2SO4 is a strong acid so it 100% ionizes. On the other hand H2SO3 is a weak acid and only partially ionizes. The HSO3- species is amphoteric. It is produced in the first deprotonation (loses 1st H+) which is a conjugate base, and is a reactant in the second deprotonation (loses the 2nd H+) which is an acid. I hope that helps!
God bless you in beautiful Iraq!
@@OldSchoolChemistry thank you so much❤️
@@AnonymousGUY554 Iraqian bro i am from iraq too
@@James189hshwh oh hello dear!!!
Can i consider CAH as an acid or base i mean this CA^+2H2^-1
When its in here
CAH2+H20----->CA(OH)2+2H2
?
THANKS FOR THE VEDIO
I am sorry, I am not familiar with this reaction.
@@OldSchoolChemistry ok no problem thanks
I used to hate chemistry but after watching your lecture you made me fall for chemistry thank you so much ❤️❤️❤️
Hi Yash! That makes me so happy. Enjoy your class😊
Beautiful teacher and beautiful explanation😍
You look so pretty how you can be smart too?!
اسیدسولفوریک نمیتواندبه عنوان اسیدقوی تولیدشود بنابراین Hso4یک امفوترنیست
Thank you for your comment. Sulfuric acid is a strong acid. Thanks! www.britannica.com/science/sulfuric-acid
thanks so much
Hi @sugarcrane7982, you are so welcome. I appreciate the comment:)
Thank you.
Hi Osamu, you are very welcome:) Thank you for your comment.
I sure that you will help me
please contin.. this lot of my problem are solved are bc of you. Your explanation is very well
Hi Kazim, I am so glad! Thank you for your kind comment. Let me know what topics you would like for future videos. Thanks!☺
If it is a reversible reaction does that mean it is amphoteric species? and if it isn't a reversible reaction it isn't amphoteric?
No, an amphoteric species can both donate a hydrogen and accept a hydrogen.
I thank god for finding you
Is OH- can be amphoteric
Please answer me l really need it
Hi Rezdar, no, OH- can only accept a H+ (base). It cannot donate a H+. I hope that helps! Thanks:)
But it became oxide,doesn't it?!
This reaction is wrong?!Ms
2OH->O-2+H2O
Please explain it to me how it is?! Cause I really need it
😿😞😥😢😓😓
You are legendary
I appreciate your comment Rezdar. Thank you:)
😘🦋🌹
You are legendary 👹
Hello, is H2SO4 also amphoteric?
Great question. No, because it is a strong acid and 100% ionizes (breaks apart). I hope that helps!
Cramming for a final right now. Thank you
Hi Trenton, Good luck on your test! :)
Hello!
I'm very confused by the acid/base theories.
I have a few questions, if amphoteric species means a chemical that can behave both as an acid or a base then why can't that be everything? We can force the strong acid HCl to act as a base if we react it with a stronger acid making the HCl accept the H+ proton, doesn't that make HCl amphoteric? If this is true, then what is the point of saying something is amphoteric if literally, anything can be amphoteric?
Does the definition of amphoteric apply and extend to Lewis acids too?
And Arrhenius? or is it only defined using the Bronsted Lowry theory?
Help!
An acid donates a H+ and a base accepts a H+. If a species can both accept and donate a H+ then it is amphoteric. Not all species can do both. I hope that helps! You do not see H2Cl in nature. Thanks!
@@OldSchoolChemistry But isn’t accepting an H+ or donating an H+ relative to the other chemical in the reaction? For example ammonia a base because it’s more basic than water; however, it’s perfectly possible (if very unusual) for ammonia to act as an acid.
Are these definitions meant to be in
relation to water?
@@Hassan-ow1qu You are correct that ammonia can donate a H+ to produce an amine. So, yes it can be classified as amphoteric. Not all chemical species can both donate and accept a H+. I would ask your professor how they expect you to answer on a test. Thanks!
@@OldSchoolChemistry Ah! Sorry Ma’am for asking so many questions.
I’m new to acid/base theories and I find it very confusing due to it having more than one definition. To make things clear Ma’am, are we using Bronsted’s definition when talking about amphoteric species? And is donating H+ and accepting H+ here meant in normal conditions, right? So I might be talking about exceptions when I say everything can act as an acid/base depending on the reaction, hence everything can be amphoteric in certain specific conditions, but in standard conditions only few are considered amphoteric species and those are addressed in this video? Am I right?
So these definitions are meant to be in relation with water because you can find water everywhere and it’s the most common solvent. Am I right? Correct me If I’m wrong.
And I’m so sorry for disturbing, this question is stuck in my head and I need an answer. 😭
@@Hassan-ow1qu You are correct except in the statement that the definitions only apply to a chemical species reacting with water. Here is a Khan Academy summary that may help you. Your next step is to visit your chemistry teacher for further clarification. I hope that helps. Thanks!
www.khanacademy.org/science/chemistry/acids-and-bases-topic/acids-and-bases/a/bronsted-lowry-acid-base-theory
is HI an amphoteric species?
No, it can only donate a H+ so it is only an acid. It cannot accept a H+ to be a base. Thanks!
Thank you so much 😍😍
I hope your class goes well!!😊
Thank you
Hi Mohamad! You’re welcome😉
what if only one product is formed? which is the conjugate acid and base?
the example I'm talking about is Al(OH)3 + OH- ===> [ Al(OH)4 ]-
great video btw, you're amazing at explaining things!!!
Hi Jimmy, identify if the reactant is accepting or donating electrons (acid or base). (It looks like you are dealing with Lewis acids/bases so the viewpoint is just slightly different.) The related species on the product side will then be the conjugate. Good luck!