Redox Reaction Simplified...

Added: 2026-05-12

[00:00:00]Um hello guys oxidation oxidation I mean redu reaction reduction and oxidation reaction to want to balance half reaction are we together so now I have few questions here written down here so the first one is zn plus ag+ to give us what zn 2+ plus what plus ag now we check the the the charge of zinc here is zero here is 2+ that means zinc increase right increase in oxidation number that's oxidation if you check um silver here Agentium and here is reduce so silver under go reduction why zinc under go what oxidation so zinc oxidation is loss of electron to make it Z2 plus it has to lose it has to lose two more electron I get it has to lose two more electron to give us what zn N2 plus. So here we can turn into Z N to now give us what? Z N2 plus. If this one comes to the other side become plus 3 minus. So whenever you have plus electron on the other side. Why are we making this electron?

[00:01:16]Because the charges is the charge is true. Whenever you have plus electron on the right side is loss of electron because initially it was on the left by subtraction. But whenever you have this plus on the left is gain. If you have it on the right is loss which is oxidation.

[00:01:30]If you have it on the left is gain which is reduction. So now let's write the half reaction for silver. So here we have Ag+ because Ag is reduced here from this to this that is gain of electron gain of electron E minus to give us what? Ag whenever you there's a reduction is oxidation number like that's reduction. Reduction is gain of electron. So it's going to gain E minus.

[00:01:56]So you can see this we have the electron on the left side here that's gain we have it on the right side here that's lost. So how can we balance this two half reaction is by multiplying equation one by one. If you multiply this by one you use the coefficient of the electron.

[00:02:11]The quotient of the electron is two.

[00:02:13]Here is one. So use the quotient of electron to multiply the first equation.

[00:02:17]Use the quotient of electron to multiply the second equation. You multiply this by one. We still get the same. Now this times 2 we are going to get 2 ag + plus plus 2 a minus to give us what 2 ag right? So you can see that this two plus can now cancel this two plus yes it can if you bind the two equation together if you gather this and this together it does it's not necessary this if it is minus it cannot cancel. Yeah if you gather these two equation together and we take this one to the other side to come and m this one it will turn to minus. So it will just cancel. So now since it has been cancelled, let's write what we have left here. We have Zn on this side. What do we have on this side? Plus 2 Ag+ to give us what do we have on this side? Zn2+ plus what? What do we have on this side?

[00:03:09]2 Ag. On this side we have what? 2 Ag.

[00:03:16]After you've balanced it like that, after you've written your half reaction and you check the number of electron, if they are not equal, you balance the electron out. Forget about the quotient of all this. You are checking the quotient of electron. Since this has two electron, multiply equation 2 by two.

[00:03:30]Since this have one electron, multiply equation one by one. So it's going to give you this will remain this because I'm multiplying by one. This one will turn to this because I'm multiplying by two. Then the electron will now be balanced. It will cancel out. Then what you have left is Z N on this side. What do you have on this side? 2 Ag+. What do you have on this side? Z N2 plus. What do you have on this side? 2 Ag+ do you have there? Now you can see that the two equations now they are not balanced. So let's let's check if they truly balance.

[00:04:00]How many charges do we have here? This plus one* 2 plus. How many do we have?

[00:04:05]This also two plus. So equation they are balanced. We have two silver. We have two silver. We have one zinc. We have one zinc. The number of atoms are balanced. The number of charges are also balanced. Now let's move to the second question.

[00:04:22]Now the second question we have Mg + Fe3+ to give us Mg2+ plus what? Fe. Now looking at this equation for us to write the half reaction. Let's first check which one under oxidation which one under go reduction. can see the um charges on ion on the left side 3 plus on the right side is just zero which means ion is reduced that's reduction right so you can see the charge on magnesium on the left side that's zero the charge on magnesium on the right side that's two plus so you can see that here mag magnesium is increased which is oxidation so magnesium under go oxidation how do you write the reaction for oxidation I told you whenever you have electron on the left on the right side in addition format That's that's loss of electron.

[00:05:10]Oxidation is loss of electron. Reduction is gain of electron. So in the half reaction loss of electron is when you have plus electron on the right. It was initially minus electron on the left. Or you can take it this way. When you have minus electron on the left, that's oxidation. Loss of electron. When you have plus electron on the left, that's reduction, gain of electron. But that since you can't leave subtraction of electron like in half reaction, it has to be plus+. So you have to bring the one from the left to the right. So we say magnesium lose two electron to give us what? Mg2+ right. So this half reaction turns to Mg Mg equals to what? Mg2+ plus what? 2 E minus. This is loss of electron now because that plus E minus is on the right side. But assuming this plus is on the left side that's gain of electron.

[00:06:03]Now for for reduction is always gain of electron don't forget about that oxidation is loss of electron. Now for ion for ferium um we have Fe 3+ is going to gain three electron to give us what Fe let's say this is our equation one now and this our what equation two so now you can see that the the number of electron here is three the number of electron here is two so how do we balance the two equation is by multiplying this one by two and multiplying this one by three we want to balance electron that's the main idea Yeah. Then at the end of the everything will definitely be balanced. Now mg * 3 here we have what? 3 mg to give us what? Mg2 plus * 3 we have 3 mg2+. Then this * 3 we have what? 6 E minus. Isn't it? Fe * 2 we have what? 2 Fe 3+ plus this * 2 we have 6 E minus to give us what? Fe * 2 we have what? 2 Fe.

[00:07:08]So you can see now this electron 6 E minus 6 6 E minus what can cancel out.

[00:07:14]So that's one of the idea to cancel out the electron. Now that we've cancel out now what is left here is 3 mg.

[00:07:22]What do we have left here? Plus 2 Fe3+ to give us what do we have left here? 3 Mg 2 plus what do we have left here?

[00:07:33]Plus what? 2 Fe plus 2 Fe.

[00:07:38]So now let's check now here is the charge is balanced. The charge we have here on this one we have zero charge.

[00:07:44]Here we have 3 + * 2 that's six charges.

[00:07:48]Here we have 2 plus * 3 that's also six.

[00:07:50]Here we have zero. So 6 + 0 we have 6 in total. 6 + 0 we have six in total. So the charges are balanced. Now let's check the atom. Here we have three magnesium. Here we have three magnesium.

[00:08:01]This is charge. This is not number of atom. Three magnesium is balanced. We have two ion we have two ion. So it's balanced. So that's that for that. Now let's before we move to the acidic medium. Now let's check the last one under this basic analogy. Now let's let's try um well let's move to acidic medium. That's so that we won't waste much of our time.

[00:08:27]Okay. Now let's just solve that.

[00:08:31]So now the next one we have um Al plus Cu2+ to give us Al 3+ plus Cu aluminium and copper. Now we can see that the the charge on aluminium here is zero. Here the charge is 3 plus. So that is oxidation. Here is 2 plus here is zero.

[00:08:52]That's reduction. So that means aluminium undergo oxidation. And what is oxidation? That's loss of electron.

[00:08:58]Don't forget. Maybe you should use this code. Um, okay. Okay. Leave that one.

[00:09:04]Yeah. Yeah. Leave that one. So, oxidation is loss. Yeah. Use this one.

[00:09:10]Oxidation is loss. Reduction is gain.

[00:09:13]Oil rig.

[00:09:16]Oil rig. You can use this code.

[00:09:19]Oxidation is loss of electron. Reduction is gain of electron. Don't forget that.

[00:09:25]So now aluminum is oxidized from 0 to 3+. So oxidation is loss of electron and because it becomes 3+ that means we are going to subtract three electrons right to give us what? Al3+ isn't it?

[00:09:42]Why is this thing f like this?

[00:09:46]So here now we have Al to give us what?

[00:09:48]Al3+. If this comes to the other side we have what? Plus 3 E minus. Isn't it? So at the end of the day, this our first equation. Now the second equation now copper is reduced. That's gain of electron. Cu2 plus plus what? 2 minus to give us what?

[00:10:07]To give us Cu. This one gain two electron. This one lost three electron.

[00:10:11]That's equation two. Now how do we balance the electron? How do we balance electron? Is by the quotient of electron here is three. The quotient here is two.

[00:10:19]So multiply this one by two. Multiply this guy by three. 2 * A we have 2 Al to give us 2 * this we have 2 A L3 plus 2 multiply by this we have we have 6 E minus 3 * copper we have 3 C2 plus 3 * this we have 6 E minus to give us 3 * CU we have 3 CU so 6 E minus cancel 6 C minus now let's write the final equation so on this left side we have 2 L and 3 C2 plus. So here we have 2 2 A L plus what? 3 Cu2+ isn't it to give us on the right side we have 2 A3 plus 2 A L3+ plus what plus 3 CU we count the number of charges they are balanced if you count the number of atom they also balanced now without wasting much of our time let's move to um acidic condition so balancing um reaction half reaction using acidic media AC.

[00:11:32]Now one thing you need to know in both acidic medium and basic medium you can add water. But in acidic medium you can add um hydrogenion as well. But in basic medium you can only add hydroxideion. You can add water in both. But for acidic you can add hydrogenion as well. In basic you can add hydroion not hydrogen. Now the first question we'll be dealing with here are broine and zinc when we have Br3 - plus zn to give us what br -1 plus what zn2 plus now now one thing one thing you need to know quick quick is that regardless of the number regardless of the charge on this broine regardless of the charge regardless of what is on it since this guy contain two elements And this is just one element. So it is it is always reduction. Take note of that from two or from more than one element to a single element. It is reduction. Are we together? And like removal of um what's it called? Removal of oxygen. Removal of oxygen. That's reduction. So oxygen was here before oxygen is no longer here. So automatically this broine here broine broine under go reduction to give us broine alone. Now and this should be the oxidation.

[00:12:59]So here we have zen from 0 to 2 plus zed then oxidize to give z 2 plus plus plus what 2 e minus this plus 3 minus was initially minus 3 minus on the left side. So but because we can't leave that subtraction on the left side we have to bring it to the right side.

[00:13:20]>> So we have to bring it to the right side. So let's say this equation one.

[00:13:24]Now we also have Br3 minus to give us Br minus one. Now in this case of acidic medium don't balance the electron first balance the atom that there is oxygen here we don't have oxygen here. So now how many oxygen the way three then add three molecules of water to the right side 3 H2O.

[00:13:49]If you have five here you have five molecules of water. That's how it's been done. But there we also have exception.

[00:13:55]It depends. There are some cases that we may only add one H2O. It depends on what we have on ground. But as far as all these are concerned this base case, we still get to question that probably may not add the number of oxygen in terms of water molecule. So we have three oxygen had three molecules of water. Now the right side now oxygen is still oxygen is still balanced. But let's see how many hydrogen do we have now? Six. So we have to balance this side too. How do we balance it? Add what? Six hydrogen.

[00:14:26]So now we have balanced the atom. Now it's left for us to balance what the the charges. Are we together? So how many charge do we have on the right side?

[00:14:34]Just minus one. Minus one. How many charge do we have on the left side?

[00:14:39]That's just that's six plus six. So how do we make them to be equal? How do you make them to be equal?

[00:14:48]So you you you what you do is that that that side with H+ is what you will make to be equal to this one.

[00:14:58]Do you get what I'm saying? Like this this you are adding the you are adding the charges to be balanced to that side with H+ not this side. So you are trying to make this to be equal to this. So what to make um what to make 6 plus to be equals to minus one that's by adding what? Let's say 6 6 um I'm coming -1 = to 7. Yeah 6 - -1 = 7 is subtraction actually. So on this side you are adding six electron.

[00:15:36]I'm using left hand there. Six sorry I'm using left hand there 6 A minus yeah see the the side with H+ you that's the side you are no you may feel like since this is 6 plus then let's make this one 6 plus then you add um whatever do we get since electron is negative okay it's not even it's not even that condition it's not even that condition of the side H+ no it's not even that condition Yeah, because if you should add 6 E minus here or whatever there is no there is no if you add electron here there is no day there is no life there is no year how many year that you can make this guy to be equal to 6 plus so this is negative if you add one this one will become minus2 if you add two this will become minus3 if you add three this will become minus4 there's nothing you want to add since the charge on electron is negative this place can never be positive so we can never make these two to be balanced no matter what we do. So that's why the electron is must be added to this side. So it's not maybe about.

[00:16:43]So just take it that way. That last expression though the first thing I said is not bad. So had the 6 E+ here 6 C minus rather plus 6 C minus. Now here we have it should be seven. Sorry it should be seven. Yeah 6 - one. Assuming we have minus here. It will be 6 - 2. Then that will be eight. So it should be seven.

[00:17:05]You can just do your mathematics there.

[00:17:07]There's no problem. So here we have 7 - 7, right?

[00:17:12]And + 6 - 7 + 6. So here will be minus one. Here we also have minus one. So what happened that way? The electrons are also what? Balanced, isn't it? Now what are we going to do? Here we have 7 A minus. Here we have 2 E minus. How do we balance it? Multiply this by 7.

[00:17:32]Multiply this by what? By two. 7 * Z N we have what? 7 Z N to give us 7 * this we have 7 Z and 2 + 7 * this we have 14 E minus 2 * 7 E minus we have 14 E minus 2 * this plus 12 H+ to give us 2 * Br this we have sorry this plus what 2 Br3 minus to give Plus 2 * this we have 2 B R -1 2 * this we have what plus what 6 H2O now you can see that this this one now where's that zinc this is that for the zinc this for this second one now this 14 E minus we cancel this 14 minus isn't it let me clean the upper part so that you can see what you're doing very well now what do we have on the left side Here we have 7 Z. Then what do we have on the left side here?

[00:18:41]We have 12 H+. What do we have here?

[00:18:45]Plus what? 2 B R O3 minus to give us what do we have on this left side here?

[00:18:52]Z 7 Z N2 plus. What do we have here? 2 B R -1 plus 6 H2O.

[00:19:03]Now let's check that. Now let's check if everything is balanced. Here we have seven zinc, seven zinc. Let's check the atom first. Here we have 12 hydrogen. We have 12 hydrogen balanced. Here we have two broine, two broine. Here we have six oxygen. 6 * 3 2 * 3 rather six oxygen.

[00:19:22]Well, here we also have six oxygen. So the atoms are balanced. Now let's check the charge. Here we have + 1 * 12. We have 12 charge. Here we have -1. This is -1 * 2. Here we have 12 - 2. So the total this is + 12 - 2. The total this one is zero. So the total charge on the left side is + 10. Now let's check the right side. Here we have two. Here we have 2 * 7 that's 14.

[00:19:52]So here we have -2.

[00:19:54]Okay. The charges are not balanced. Now let's check. There's a miss up somewhere.

[00:20:02]I can't really figure where the mistake.

[00:20:03]Here we have 10.

[00:20:07]Here we have 12. It's not balanced. It has to be. I can't figure it. Maybe the question I don't want to waste much time on that.

[00:20:18]Let's let's do the next one. We do that very well. But take note that charge is not balanced. So that's reaction is not yet balanced. That one is not yet balanced. But I don't want to waste time on that. Let's just move to the next question. So we deal with it very very well in the next question. Plus CL O minus to give us what? Cl minus to give us Al3+ plus what? CL minus. Now let's do this guy very well. Let's come so that we not make mistake. Sorry for the previous one but at least you learned something from that. So which are going to apply as well. Now aluminum here increase in um charge. So that's oxidation. So Al to give us Al3+ plus what? 3 E minus right.

[00:21:07]Now for Cl minus plus okay to give us what? Cl minus this one don't don't add electron yet first balance the atom. No this place now the atom is balanced that's why we are moving to the electron aspect already. But when you see that the balance first balance the atom before adding electron one oxygen right one oxygen rather so here add one molecules of water just add H2 to this side so oxygen chlorine is one one oxygen is one but here we have two hydrogen so add plus add 2 H+ to this side do we get that so now hydrogen is balanced. Oxygen is balanced. Chlorine is also balanced. Now let's balance electron. Now so how many electron do we have? Here we have two plus minus one. Two minus two plus minus one that's one plus one. Here we have minus one. If you continue adding electron to this side there's no it can turns to positive because electron itself is negative. This side become negative. So we only have to add electron to this side. So how many electron do we need to add to plus one that will make it minus one? It is two electron right? So let's say 2 E minus plus. So if you add 2 E minus to + one it will become minus one. So the charges are now what? Balance. So now now but the next thing here now how many electron do we have? Three. Here we have what? Two. Our here is two. Here is three. So multiply this one by three.

[00:22:49]Multiply this by what? By two.

[00:22:52]So now 2 * A we have 2 A L to give us 2 * this we have 2 A L 3+ 2 * this we have what 6 E minus 3 * this we have what 6 E minus plus 3 * this we have 6 H+ 3 * this we have 3 C minus to give us 3 * this we have 3 CL minus 3 * this plus 3 H2 what? H2O. So this 6 C minus can cancel this 6 C minus. So what do we have left on this left side? We have 2 A L. What do you have left here?

[00:23:32]+ 6 H+ + 3 Cl minus to give us what do you have on this side? Cl minus.

[00:23:45]What do you have here?

[00:23:49]Oh, sorry, sorry, sorry. What do you have on this side? 2 A and this. Right now, what do we have on? Yeah, this. We have Al3+.

[00:24:02]2 A L3+.

[00:24:04]This is the one we have canceled this.

[00:24:06]The one we have on the left here is this. On the left is this. The one we have on the right here is 2 Al3+.

[00:24:12]2 A L 3+. The one we have on the right here is what? 3 CL minus plus what? 3 H2O. Now let's check if they are balanced. Now we have two. Let's check the atom before the charges. We have two aluminium. Two aluminium is balanced. We have six hydrogen. 3 * 2 here we have six hydrogen as well is balanced. We have three oxygen.

[00:24:40]So here also 3 O. So here we have 3 * 1.

[00:24:45]We have three oxygen balanced. We have three chlorine. We have three chlorine.

[00:24:49]So all the atoms are balanced. Now let's check the charge. Now for the charges here. Here we have 6 * + one. Here we have + 6. 3 * -1 we have minus3. So here we have + 3 in total. We have + three in total there.

[00:25:06]But for the right side 2 * 3 we have + 6. 3 * - 1 we have minus3 also what? Plus three in total.

[00:25:14]So both charges and the atoms are balanced. So this is our balance reaction, balance equation. So that's how to do it in acidic medium. You add molecules of water. Then you check if I had water here. What happened to the other side? The other side is lacking hydrogen. Then add hydrogen atom there.

[00:25:35]Hydrogen.

[00:25:37]So that's it. But for for basic medium when you add water whatever the other side is lacking you add hydroxide not hydrogen. Now let's do one more under acidic medium before we move to basic medium.

[00:25:50]Now manganate and ion this is a single element. This is two elements. So it's reduction already. So this one is oxidation. So here we have Fe oxidize to give us Fe3+. Right? So that's loss of electron. That's minus 3 E minus. But let's take it to the other side to become what? + 3 E minus. So for MO4 for magnate um don't don't add electron yet. First balance the atom. You see this one has oxygen. This one does not have. So balance the atom. We have Mn2+. How many molecules of oxygen do we have? Four.

[00:26:29]How many atom rather?

[00:26:33]We have four atoms of four atoms of oxygen cuz it's just a single element do we get? So we have four atoms of oxygen.

[00:26:41]So that means we are going to add what?

[00:26:43]Four molecules of water. So we have four what? H2O. So oxygen is now balanced.

[00:26:50]Now let's check hydrogen. Here we already have eight hydrogen. That means you're going to add what? 8 H+ to the other side. Right? Now the atoms are now balanced. Now let's check the charges.

[00:27:02]How many charge do we have here? We have 8 plus and we not using this to it's only the coefficient of the molecules that use this one is just so this just minus one here. So here we have eight 8 minus one. So here become seven. I mean do we have two plus 7 and 2 plus? So what are we going to how can we make how can we make + 7 to become 2 plus?

[00:27:31]There is no you can make this two plus to become plus because it will keep on reducing till it gets to negative but this one can reduce and get to plus. So that means sorry that means we are adding electron to this side. So how many electron are we adding here we are that should be minus minus 2 that's 9. So we adding n electron this side that's 9 e minus plus we're adding n electron.

[00:28:00]Just do your math. Do your math there.

[00:28:02]So this 9 e minus plus what? So here now we have - 9 + 8 - 1. It becomes what?

[00:28:15]And come let me check no no no no.

[00:28:21]This one is + two. Sorry it's not minus2. We are not adding minus 9. What we are adding there? Assuming this is minus. That's when you will be doing 7 - - 2 but it's 2 plus so it will be what 7 just 7 - 2 assuming it's minus it will be 7 - like the one we have been doing can just do your math there it's not hard how can you turn 7 to 2 to + 2 assuming how can we turn seven to minus2 yeah that's by adding plus 9 how can we turn seven to + two just add what do we get? So this one should be five.

[00:28:59]So that should be five. So now we can see that the coefficient of electron here is five. The quotient here is three. So how do we balance it? 5 * what * 3. 5 * F we have 5 F to give us 5 * this we have 5 F3 plus 5 * this we have 15 E minus. 3 * this we have 15 E minus.

[00:29:21]3 * 8 + 24 H+ 3 * this we have 3 MN O4 minus to give us 3 * this we have 3 M2+ plus what 3 * 4 H2 we have 8 H2 H2O so 15 E minus will cancel 15 E minus isn't it so now what do we have on the left side what is left there we have 5 Fe what is left here plus 24 H+ plus what? 3 M O minus to give us what do you have left here?

[00:29:59]5 Fe2+. What do you have left on this right side? On the left side and on the left side here, you gather them together. The right side and the right side here, you gather them together.

[00:30:08]Here we have the right side here is this. The right side there is 3 MN2 plus what? 8 H2O.

[00:30:18]8 H2.

[00:30:21]Now let's check the atom and the charges if they are balanced. Now we have 5 Fe.

[00:30:25]5 Fe is balanced. 24 hydrogen.

[00:30:31]Wait. Hydrogen is not balanced.

[00:30:34]It's balanced. I made a mistake. 3 * 4 is 12. I wrote eight. 3 * 4 is 12. Thank god like that. So it's balanced. So we have 5 Fe.

[00:30:47]5 Fe on the right side balance 24 hydrogen.

[00:30:52]So this is 12 12 * 2 24 24 hydrogen three magnes 3 magnes 3 * 4 12 oxygen 12 oxygen 12 oxygen as well 12 is the coefficient here 12 oxygen can we see that now for the charges are the charges balance here we have 24 * + 1 we have 3 * -1 that's -3 so here we have 24 - 3 we have 21 charges plus 21 charges on the left side. Now let's check the right side. Is it up to or more than 21 charges? 5 * 2 + we have 10.

[00:31:36]3 * 2 plus we have six plus 16. We have to check something is not balanc.

[00:31:47]So what's happening? Here we have 21.

[00:31:49]Here we are 16.

[00:31:52]What's happening? What's happening?

[00:31:59]Okay. Sorry. This is 3 plus Fe3+.

[00:32:04]This is it, not two plus. Please just be very careful in case you are doing your exam. Don't don't mix things together.

[00:32:11]No. The left side there is 5 E, 5 E. The left side there is 24 this this. The right side there is Fe3+ Fe3+.

[00:32:21]The right side there is this, this, and H2. This So this is Fe3+. 5 * 3 that's 15.

[00:32:30]3 * 2 that's 6. 15 + 6 is 21. So the two charges are balanced. So thank God for that. Maybe that's one of the mistake we made in the first question. So please, that's how to. Now let's move to basic medium.

[00:32:44]Don't forget to like and subscribe. If you have any question, just drop it on the comment section. I'm going to answer it. Now, for the basic medium, let's say we have Fe plus C minus to give us Fe2 plus what? CL what? CL minus.

[00:33:12]So that's the question.

[00:33:18]So that's the question. Now Cl is reduced. Obviously the oxygen oxygen is not here. So it's reduced obviously and this one is oxidized. So now we have CL minus to give us CL.

[00:33:35]So in this case reduction we should have added electron already but I told you first balance the atom in cases like this. So how do we balance the atom? We have one oxygen here, right? So what what happen here?

[00:33:50]So here let's add one H2.

[00:33:57]I'm coming.

[00:34:02]Okay, let's add one H2O. Five. So oxygen is balanced right now. Now what of hydrogen out of hydrogen here we have you know I told the basic medium you are not adding hydrogenion what you are adding is what hydroxide so here let's add 2 O minus 2 O minus so now let's see what is happening here we have hydrogen is now this is now three Oh yeah, sorry.

[00:34:40]Sorry. In basic medium. Yeah. Yeah.

[00:34:42]Sorry about that. In basic medium, always add the water to the side that have more hydrogen. Yeah. Yeah. Sorry about that. In acidic medium, we add the water molecule to the side with less hydrogen. But in basic medium, add water to the side with more hydrogen. Add water to the side with more hydrogen. So we are adding the water here. H2O.

[00:35:06]So here now oxygen is now two hydrogen is also two. So this one becomes what add two hydroxideion.

[00:35:15]Oxygen is balanced. Now hydrogen is also balanced. Two and two. Two and two.

[00:35:21]For acidic medium you can add water and hydrogen. Add water to the side with less hydrogen. Then hydrogen to the other side because it's going to lack hydrogen after adding water to the side with less hydrogen. But for basic medium, for basic medium you can only add water and hydroxideion. Add for basic medium add water to the side with more more oxygen rather. Initially I mention hydrogen I mean oxygen.

[00:35:44]Let me repeat again acidic medium add water to the side with less oxygen.

[00:35:50]Then you are going to add H+ to the other side. If it's lacking H+ in basic medium add water to the side with more oxygen. Then on the other side you're going to add O minus.

[00:36:03]So the number of O minus will be determined whether will be determined by the amount of O and H that you have on this side. So here now we can see that it's already balanced. This is the only one question I will solve on basic medium but I will explain it very well or I may solution and give some some assignment on it. Now let's see what happens next. Now let's write for Fe. Fe to give us what? F E O H O H 2. Now here we can see that here we have 2 O this one.

[00:36:37]So obviously what are you going to do?

[00:36:40]Add hydroxide to this side. Two molecules of hydroxide.

[00:36:44]Now O is 22. H is also 22. Everything is balanced.

[00:36:50]Everything is balanced. So what's the next thing? Now let's now now how to know when where to add and the amount of electron to add. Now let's check the since the since all the atoms are now balanced. Now let's check all the charges if they are balanced or not. If all the charges are balanced then we can just add the two equation together then that will be the final answer. But if they are not balanced we are going to either add electron to whatever whatever. Now for this one here we have how many how many charge do we have here? We have minus one on this side we have minus3. Right? this 2 minus and 1 minus that's minus 3. So how do we make them to be equal? Now if we keep adding electron here to this side it will keep increasing in negative from minus3 if you add one electron we have minus4. If you add two electron we have minus 5. So it can never be minus one. So for minus1 to be minus3 the electron has to be added here. So if you add two electron here so this place becomes 2 e minus do we get? So -2 and minus1 is now minus3 is balance. Now let's check the other one here. The charge here is zero. There's no charge here. The charge here is minus2. How do we make both of them to be zero? So now if you add now which side are you going to add? This side or this side? Is this side actually? Because there's no how this can be reduced to zero. If you keep on adding electron it become more big in the negative like it become having negative negative. It can't be reduced to zero. But here is by adding what? 2 E minus. So do we get what you are saying now? So what's the next thing to do now?

[00:38:34]So I think since both since the electron we added to both is 2 - 3 minus that means in the first place the equation is balanced. do we get?

[00:38:47]Well, we don't know yet. Always try it by confirming. It's not about, you know, if you had this left to this left and had this right to this right, it may balance. But first check the electron first probably or you can check either way. So this one will cancel back. That means we don't even need them in the first place.

[00:39:05]So you can first check and add this time assuming we are adding three here now.

[00:39:11]Then we have to multiply by three multiply by two. But since this 22 is balanced that means in the first place even before we had this they are balanced. Let's check let's check if they are indeed balanced. Now what are the left side there we have H2O plus what CL minus to give us what are the right side here you have CL minus plus oh sorry sorry the left side there is what? H2O plus C minus. The left side there is what? 2 H minus plus what? Fe to give us the right side there is what?

[00:39:40]CL minus plus what? 2 O minus plus what?

[00:39:45]Fe O what? 2 right or the left side and the right side together. Now let's check if it's not balanced. Now that mean there is a mistake. But since this guy are equal by balancing the two side and the two sides since this one are equal and they can stick that means initially without checking they are also balanced.

[00:40:03]Now we have how many hydrogen do we have here? Let's first check the molecule.

[00:40:06]Here we have two hydrogen plus another two that's four. Here we have two hydrogen plus another two. That's four.

[00:40:13]Let's check oxygen. We have one oxygen, one oxygen. That's two plus two. That's four. Here we have two oxygen, two oxygen. That's also four. Let's check chlorine. One chlorine, one chlorine, that's balanced. Let's check. One ion, one ion, that's balanced. All the atoms are balanced. Now, let's check the charge. Here we have -1 and -2. 2 - 2 * -1. That's -3. Right? Here we have -1 -3.

[00:40:37]So, it's balanced already. So now let's do one more question then I will give you the rest as assignment.

[00:40:48]So now here we have um I - plus CL3 -1 to give us I3 -1 plus CL minus minus there's no need of putting one. So now um now for this one is reduced because there's a loss of oxygen CL3 minus to give us what Cl minus. But we have to balance the atom first. Now this is a basic medium not acidic medium. So you adding water to the side with more oxygen. If it's acidic medium you're adding water to the side with less oxygen. Do you get? So this guy is going to become plus what?

[00:41:39]Three molecules of water. Do we get now to how many number of how many oxygen do we have on this side? Now we have three and that's six, right? How many hydrogen? We also have six. So on this side you are going to add what? Six O minus. It's balanced. Now don't make mistake. In acidic medium you're adding water molecule to the side with less oxygen. In basic medium you're adding water molecule to decide with more oxygen. We have few exception in basic medium at times that it depends on the kind of um you know what gives you this. It depends at times we have some exception but just know it that way.

[00:42:21]When we get to those exception side you also understand the way I'm going to explain it. Now we are done with the first one. Now for for I for for iodine the atom are balanced already here we are not talking of number we are not talking of whether this is one this is three but it's hydrogen hydrogen there's no additional whether is this one has oxygen this one does not have there's no problem about that now okay I think we are going to add two I here to make this up to three.

[00:42:59]We are going to know along the way.

[00:43:00]There's no problem to make this up to three. I think we are going to add to high now. Yeah, we balance the atom too.

[00:43:08]Yeah. Yeah. Yeah. We balance the atm.

[00:43:10]Yes. Yes. Add to high. So, we have three iodine and three iodine. Fine. No problem. So, now let's check the charges. Now, the charges here is -1, right? And this side is -1 and -6.

[00:43:26]That's - 7. How do we make -7 here to be equals to minus1? Is by adding six electron here 6 E minus plus. So here is already - 7 and - 7. They are balanced.

[00:43:38]Now always balance the atom. Please take note of that. So I have to add two iod here to make it up to three. Now here we have charges minus1 minus one. The charges are balanced, isn't it? So we don't need to stress we don't need to stress ourself with this one.

[00:43:54]So, but now how do we now balance the electron? How do we balance the electron? So, this is going to be what?

[00:44:02]Times one.

[00:44:04]This is going to be what you are going to multiply this one by six. The number of electron. Wait. I think >> you wait. Electron has to be on this side.

[00:44:22]>> Where?

[00:44:24]something. I'm trying to get what we are going to do here >> and I don't want to waste our time by making the video so long.

[00:44:36]Um, okay. Let's pause on this. It will be part of the assignment. I'll just confirm.

[00:44:45]I will confirm and I will drop the solution. So, let's not waste time on this.

[00:44:52]I need to check something on that. So, let me just do one more. I I want to make sure that we do one more. So, let's just let's have one more. S O 32 minus plus N I O 3 minus to give us N I plus what? SO4 2 minus.

[00:45:20]I hope I'm writing all these. I hope all these equations are correct. But please what we have explained so far they are 100%. Just know those one and be able to apply them. Okay. Let's let's let's check this question as well. Let's check. Let's check.

[00:45:37]So now what's going to happen here this one is reduced because there is loss of oxygen. So it's reduced.

[00:45:51]This one is increased. This is um S for four. This is S for six. This of six.

[00:45:58]This of four. So this one is increased.

[00:46:01]This one. This one increased from four to six. Like this tetra sulfate four.

[00:46:06]This t of six. So this one increased from four to six. That's oxidation. So we are not even balancing we not even balancing the charges yet. So I don't even need I don't even need that for now. So now like I said you going to add water to the side with more oxygen for basic medium. So plus what?

[00:46:30]H2O. Now should we add 4 H2O?

[00:46:34]Now you know I told you the number of oxygen will be the number of water you had. No but because we already have three oxygen here.

[00:46:45]I think we can just add one more water.

[00:46:49]Let's check. Assuming we add one more water. Let's see. It's something that you can just use your Now let's add O here. O minus O minus. Now let's check the number of oxygen. Four. Oxygen here is now five.

[00:47:11]If we had two O minus here, oxygen here is five. oxygen is balanced. So yeah, it's balanced that way. So why do we not need to you know like I said we have some exception such a way that it's not every time you be saying since the number of hydro oxygen is four then add four molecules of water. You don't need to add four molecules of water. The reason for adding molecules of water is to first first of all balance the number of oxygen. Since you already have three oxygen on this side I think for this case you can just add one molecules of water. So number of oxygen Do we do we grab that and just um assuming it's acidic medium now you will understand this this very very well you understand very assuming it's acidic medium because here now it's like we are even increasing oxygen here and this is just three this this is this has become five now it is easy to make this balance now five and we still have two hydrogen two hydrogen so even Even though if you want to say four, there's no problem. You still get your answer. Put four here.

[00:48:17]Yeah. Now we now what? Eight oxygen, right? And eight hydrogen, right?

[00:48:24]How many oxygen we have here? Three.

[00:48:28]Now you can see now in fact this one will not even work because you put five here.

[00:48:33]There will be having five hydrogen.

[00:48:35]There is no there is no day, no, no year, no month. You can make the hydrogen balance. we get just just just think so here we have what two so it's balanced that way it's balanced now let's check for nl here we have n i h3 minus to give us what n i so let's add our water here so here now we can add four molecules three molecules of water 3 H2O plus so now how many hydrogen do we have six how many oxygen six so This just become plus what? Six O minus.

[00:49:16]All the atoms are balanced now. Now let's check the charge. The charges.

[00:49:20]Here we have two minus and another 2 minus. That's what that's four minus.

[00:49:25]Here we have 2 minus. So it has to be balanced.

[00:49:29]So here for this side for this side we have to add plus 2 E minus and here will be 4 - 4 minus. Now let's check this one too. Here we have just minus one. Here we have 6 minus.

[00:49:47]How do we make this to be equal? So is by adding 5 E minus here. So this one is now min - 6. This one is zero. There's no charge.

[00:49:58]- 6 and - 6 balance. Now do we balance everything? Multiply this by coicient of this one by five. Multiply this one by two. So this one times 5 and this second one time what? Two * 2. So 5 * this you have 10 O minus plus 5 * this 5 SO3 2 minus or minus2 to give us 5 * this 5 SO4 2 minus 5 * this we have 5 H2O 2 * this we have okay 5 * 2 E minus we are not done 5 * 2 E minus we have + 10 E minus So we are done with the first one. Now the second one 2 * this we have what? 10 E minus 2 * this we have what? Plus what? 6 H2O. 2 * this we have plus what?

[00:50:57]Plus 2 N I O H3 minus plus 2 * this we have what?

[00:51:05]2 N I plus 2 * this 2 * 6 we have 12.

[00:51:13]O minus.

[00:51:15]Do we get that way? So is just multiply all this by two. Multiply all this by two. Multiply this by five. Like the coefficient of electron in equation two.

[00:51:26]Use it to multiply equation one. The coefficient of electron in equation one.

[00:51:29]Use it to multiply equation two. You get this. Now this one cancel this 10 E minus. All right. So now let's now write everything out.

[00:51:42]So writing everything out. So here we have the assignment I want to give. I've clean it. Okay, I will paste it on the comment section. I will paste the assignment on the comment section. So here we have 10 O minus plus what? 5 SO3 2 minus. Now what was the left side here? Plus what? 6 H2O plus what? 2 N I O H 3 minus to give us what's the right side there? 5 SO42 minus plus what? 5 H2O.

[00:52:25]The right side there plus what? 2 N I plus what? 12 O minus. Now let's check everything. Now how many hydro do we have here? And how many oxygen do we have here? 10. Here we have 5 * 3 15 that's 25. Here six.

[00:52:47]That's 31. Here we have 2 that's 33. Now let's check the number of oxygen. If it's also equal to 33 5 * 4 20 + 5 25 + 12 25 + 12 that's what?

[00:53:05]Let's confirm. This is 10 + 15.

[00:53:11]10 + 15 that's 25 + 6 that's 31. Okay.

[00:53:15]Sorry. Sorry. It's not 33. Plus this 10 + 15 25 + 6 that's 31. Here we have 3 * 2. 31 + 6 that's 37. 37. This is 2 * 3 6 hydrogen. 6 oxygen. Right? 6 + 6 + 15 that's 12 + 15 right and that's 27 + 10 that's 37. Now let's check the right side. 5 * 4 20 + 5 25 + 12 that's also 37. So oxygen is balanced. Now let's check hydrogen. 10 hydrogen + 12 that's 22. 3 hydrogen that's 25. Let's check here. We have 10 here. Let's check again. 10 + 12 22 + 3. Now let's check this one. Here we have I'm coming.

[00:54:09]Oxygen is balanced now. Okay, I'm coming back to hydrogen. Let's check the charges. Here we have 10 minus 5 * 2 that's 10 minus that's 20. 2 - 22 charges. We have - 22. We have 22 minus.

[00:54:24]Here we have 5 * 2 10 minus and 12 that's also 22 12 minus. So charges are balanced. Now oxygen are also balanced.

[00:54:34]Now the hydrogen we have 10 we have 12 that's 22. Here we have three that's 25.

[00:54:43]Now here we have 10 and 12 that's 24 and that's 22.

[00:54:49]Three hydrogen is left. What happened?

[00:54:52]Okay, for now let's check for sulfur.

[00:54:55]Sulfur is five here. Sulfur is also five. Sulfur is balanced. Nicar is two.

[00:54:59]Nic is two. Nickel is also balanced.

[00:55:01]The the hydrogen is missing up somewhere. You have to be careful when doing all these things. You have to be very very careful.

[00:55:11]Okay, hydrogen is even six. Hydrogen is even six. It's not even three. Here we have 10 + 12 22 + this 2 * 3 is 6.

[00:55:21]That's 28.

[00:55:22]28. Here we have 10 and that's 22. There is six. There is six hydrogen somewhere.

[00:55:30]Six hydrogen somewhere.

[00:55:32]There are six hydrogen somewhere.

[00:55:38]Six hydrogen somewhere.

[00:55:41]That's just be careful. I've cleaned the question. I would have done it again. So that's that for that. But I think I've explained it enough. just yeah if I see where it's missing I'm going to put it on the comment section and also put the assignment on the comment section. Thanks for watching.

[00:55:58]Don't forget to like and subscribe and drop your drop whatever you want to drop on the comment section. I will surely attend to it. Thank you. But please whenever you are doing something like this check the number of charges the number of atoms. If there are no balance that means you have made a mistake. So you have to trace your step back. But I think the explanation is very clear now.

[00:56:19]So you can apply it and the the main part is that you should be very very very careful.