Balancing Redox Reactions in Acidic and Basic Conditions
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- Опубликовано: 17 июл 2024
- We know that redox reactions are ones that involve electron transfer. Something is oxidized, and something else is reduced. But these reactions can be tricky to balance when surrounding water molecules are involved in the reaction. Let's go through the algorithm for balancing redox reactions in both acidic and basic conditions.
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I had been searching for a good video to understand this for hours and finally came across this and understood it straight away thank you so much
So.. I'm in 11th grade! and we have this topic for our finals. My chem teacher sorta makes everything more confusing.. for my test, I ended up spending like 2 weeks just to end up memorizing this! So grateful I found this video before my finals!! I can finally solve the reactions on my own. Thank you, professor Dave!
ive been coming to this same video for years now, every time I forget how to do these. This is the absolute BEST explanation on yt on how to do this.
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You will not believe this but I have been practicing Redox rxn for 2 years and if a gap occurs of two-three months I forget half-redox method. But with this easy explanation I will never forget it and for that you have my highest gratitude.
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I was looking for the difference between acidic and basic solution and couldn't find why it even exists. Very nice instructions. Thank you
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always struggled with balancing complex redox rxn, this video rlly helped me out. THANKS!
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literally teaching me the whole course, thank u!
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Thank u sir my school teacher takes test of these reactions tommkrow it help me lot and for final exam it's so imp....
Thanku sir
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I rewatched this video over and over for my homework, it’s helped me so much in class, thank you so much 😭😭
very clear, I got the check comprehension right just by watching the method under each condition once
This was extremely helpful! Thank you so much!!
Oh my god thank u . Its really the easiest way to balance in case of basic medium . I love it .
That was a wonderful explanation! ..thanks
Dude this is literally the perfect video for explaining this
How Cr lost 6 electrons?
It doesn't, it looses 3 so 2 of them loose 6
Your explanation is perfect prof
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Thank you so much 💖 for teaching them to me the first time
Came back here to review too 😂❤
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What a relief when you solve an equation and the answer is right !!
C2O4-2 + Mno4 _ co2 +Mn+2
Can you balance this equation using this rules in the video ?
Yes, you can. Just did this.
Thank very much I have been trying to balance redox reactions for days you didn’t show us how to combine to to reaction after multiplying the electrons pls do a video I would be grateful
This was good but the step where you add electrons could use a bit more clarification. I get it, but only after rewriting the half reactions as one long equation. Maybe annotate that part of the video to eliminate ambiguity as to what left and right actually mean. Again, I got it, but not at first until I stared at it for a little.
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This really helped
Can someone explain how the dichromate ion was reduced to Cr^3+ and how the Fe^2+ was oxidized to Fe^3+ cause I did understand that k ions and the sulfate ions are spectator ions and they are neglected to see what happened in the reaction.
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Super explanation sir
As a college student, part of me really wishes I took chemistry while I was in highschool… and precalc/trig… college doesn’t always take into consideration…
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YOU ARE STUDYING THIS IN COLLEGE WE ARE STUDYING THESE ALL IN 11 GRADE
@harshavardhan.69 it's taught in chemistry. Chemistry is taken both in high-school and college.
@@alexawermuth1219 yeah but balancing is not in high school am I right?
@@harshavardhan.69 I can't remember
hey can u pls tell how to identify wether the rxn took place in acidic or basic medium?? if u hv alreasy uploaded any video regarding that can u pls give me the link for it...
Wow...it s all coming back to me!
Nice explanation
After this video now I created a rule to balance these redox reactions half equation -> balance moles ratio -> H2O -> H+ -> e-(balance charges)
Thanks for this ❤
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This one really helped me
My Text book failed to explain it clearly. 👍
How did you get +6 in the first example for the dichromate?
oxygen is -2, times 7 is -14, the ion has a formal charge of -2, so that's a total of +12 shared between two chromium atoms, so +6 each.
Thankyou . Nicely explained 👌
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