Using oxidation states - balancing half equations

[@BinhNguyen-vl2dx]

The rules made it a million times clearer. Thank you very much. Here's an extra sub for you!

[@AlleryChemistry]

Awesome, thank you!

[@atiarimi7322]

Wow, once again you managed to explain something so effectively that would have otherwise taken me hours to grasp😂, thank you so much sir.

[@AlleryChemistry]

You're very welcome!

[@g1rlonl1ne]

Thanks sir, I always seem to not comprehend what I'm listening to in my chemistry classes and all your videos are so clear so it's very helpful... :D

[@AlleryChemistry]

You are most welcome

[@itzbigdelly3118]

Forgotten how to do ionic equations and this video helped me regain all that knowledge and be able to do them easily, thank you so much

[@user-lr8op6qx7p]

Thank you so much! I have binged so many of your videos in these last few days and I've honestly found them so helpful! Thank you!!

[@BenjaminHughes-s3z]

the greatest to ever do it

[@fatimahislam792]

I understood in 14 minutes! Wow amazing explanation! Thank you very much!!

[@loodynagy9270]

Can't thank you enough! :')

[@بنتمحمود-ز4ذ]

these videos are very helpful thanks

[@FanFactor]

Thank you for making these videos! They're incredibly helpful! Could you do a video where OH- ions are involved in the half equations because I'm not sure how you can balance the O's if you keep on adding OH- ions. I know that Q8 on the June 2014 F325 OCR paper asked you to do this - perhaps you could do a worked example? Thank you again!

[@AlleryChemistry]

John Lewis Thanks very much! I will take a look at your request and see what I can do. Watch this space.

[@FanFactor]

Life saver! Thanks!

[@noorah.r8411]

I know this is late but to everyone with the same question, you balance the same as you would a redox equilibria in acidic conditions but as you're doing in alkali/basic conditions you need to add OH- to cancel out the H+, so do everything else the same just 1. Add an OH- for every H+ ion to both sides, combine the OH- and H+ to make H2O and then cancel out the H2Os to get your overall equation

[@meowmeow-dw3bi]

thank you for these amazing videos

[@AlleryChemistry]

Glad you like them!

[@l.o3223]

What do you do if there are hydroxyl groups in the equation? In some past paper questions, I have seen them use OH- and H20 instead to balance.

[@saharaiqbal9973]

This is so helpful thank you

[@mariamorais2568]

YOU ARE AMAZING!!

[@amajdalaweyeh1582]

Brilliant despite of the small board... thanks

[@i_dontlikemilk]

redox really had me shook, smh thank you

[@yahiaaa3]

your 800th like, you're welcome sir👍

[@AlleryChemistry]

🎉 Thanks for the like!

[@farwahrehman3684]

LOVE THISS TYSM!!!!!!1 HELPED ME SO MUCHH

[@risandi420]

bless omg i finally get it

[@danielfranklin2433]

Thanks!

[@jodiebodimeade1583]

Thanks so much!!!!

[@victoriaheath6981]

THANK YOU!!!! the biggest help

[@na.1221]

Thanks teacher

[@AlleryChemistry]

No problem 😊

[@jamesmatawa8577]

Amazing 🎉

[@AlleryChemistry]

Thank you! Cheers!

[@ramyagururajan]

hi sir i had a quite challenging question in my textbook which said balance the following equation using oxidation numbers ....cl2 + ....oh^-1 ----> .....cl^-1 +.....clo3^-1 + ....h2o how would you balance that and could you kindly outline the steps you would have to go through as done in this video warm regards.

[@hamzah4656]

no

[@Tsy172]

@@hamzah4656🤣

[@MuhammadUmair-wu3ez]

Thank you ;)

[@georgia.k]

why does having 2cr3+ affect the overall charge. i thought it is just still 3+ and not 6+

[@sheeer4370]

Why didn't u made an ionic equation of that ethanol reaction? :/

[@BenjaminHughes-s3z]

we cannot replace him

[@Wild4lon]

Nice but a little oversimplified method in my opinion, since sometimes you can't add H+ as it's not in acidic conditions

[@splitswinger2041]

you look like my cousin