hello friends this video on electrochemistry part 22 is brought to you by exam flare calm no more fear from exam it has been seen that as I already told the conductivity varies made the conductivity of a solution vary based on concentration so normal understand the pattern of the variation of the conductivity of a electrolyte we'll talk about the normal conductivity variation and we'll also talk about the molar conductivity variation the novel conductivity was we just saw as k and this is lambda for electrolytes both for weak and strong electorate you'll see a will see there they have little different behavior we will talk about the variation of molar conductivity of electrolyte and we'll talk about normal conductivity of look like the variation of both this conductivity first let's talk about the electrolyte normal conductivity variation so here we are talking about the normal conductivity nanoscale so if we see the definition of conductivity conductivity of a material is nothing but its conductance where it is 1 meter long and its cross sectional area is 1 meter square that is my conductivity of this solution right in this please note I'm talking about the electrolyte a conductivity variation so in this case my current carriers ions they are my current career now if we increase the concentration of ions obviously what will happen if you increase the concentration of ions I encounter per unit volume then the conductivity increases I forgiving it suppose I have one glass of water you add some 1 teaspoon of NaCl you measure the conductivity you are two more teaspoon of NaCl you measure the conductivity you see that the more you add NaCl that is nice once all the more conductive is the solution why because you have more ions it's pretty straightforward answer right but the Z can say that the conductivity is directly proportional to concentration but there is a catcher so if you talk about the strong electrolyte and the weak electrolyte this is a variation you see the strong electrolyte for example NaCl is this case and weak electrolyte example ch3cooh so if you increase the concentration of strong electrolyte the conductivity increase at a higher rate but if you increase the concentration of a weak electrolyte the conductivity increases with a lower rate the question is going see this is the what the picture actually this is my ch3cooh and this is my ch3coo minus ions hi this is my h+ ions here I have my n ECM this is my ne plus until my lines not just understand that items on the left that is my NaCl or ch3cooh they don't conduct current current carriers are my ions in this case ch3coo minus h plus na plus CL minus they carry current that is a very very basic concept right now in case of a strong electrolyte you increase the concentration of NaCl let's suppose NaCl we know the moing you say n is if you see there's a single arrow here that means the moment you add NSEL to a water almost 99% NaCl will dissociate into na+ and cl- ions thus the more you increase NaCl concentration in a electrolyte you will get more and more na+ and cl- ions more na plus and Cl minus sign implies more conductivity like this is pretty ok the catch is the V collector light so the electrolytes you see we have cs3 see us - ions they are in equilibrium with CSC CO - an h+ does if you see there is a equilibrium sign what it means is if you have a dilute solution if you have a dilute solution in the percentage dissociation is more maybe in case of dilute it is 80% districted or it's supposed 80 percent is too much what 3% let me take 10% in case of concentrated it will be not even 1% there is a difference right so if you take a dilute or maybe it will be more in let us say 40 possible yeah just to understand these figures may be wrong just to understand I am taking these figures if you make very very dilute may be hundred percent also like the max is hundred percent let suppose but if you make it very very concentrated it is then solution will shift on the right if you make a very dilute solution the concentration will ship on the the solvation exam the equation the reaction will move on the by rate so if you make a concentrated solution the reaction moves on the left values originally the reaction moves on the right so what is happening in this case of weak electrolytes you are increasing the concentration the of concentration of the ch3cooh or the weak electrolyte the concentration of the ions are not increasing at that right because the moment you increase the concentration the equation is the reaction is also moving a little bit on the right side correct so thus the effective number of ions here doesn't increase that much so let's take one sinner let's give some better area let's take this to be on dilute it let this be hundred percent and I'm constantly this beer can right so if I make a dilute in one liter let suppose in one liter have a one liter job and in that I just put one moles of ch3cooh right if I put 1 mole of CSD coh let me see if I put 1 mole of CSD cos I put 1 more of cscc which I get let's suppose 100% it dissociate so I get 1 mole of CSC co - one more of CSC cos correct now if I make it more concentrated let me make it 10 volts if I make it 10 moles so in 10 verse instead of 100 percent dissociation let's suppose this situation is 50% 50% of this is you get 5 moles of this you get five words of this let me make it 100 moles in honored most let's suppose the discussion is 20 percent because the more you'd make it concentrated the this efficient person this decrease becomes 20 and this become great let me make it now $1,000 and 1001 that we assume this 5% so this becomes 50 and this become put now you see you are increasing the concentration from 1 to 1,000 but actually if you see the ion concentration is only increasing from 1 to 50 and that is what I am showing here you are increasing the concentration too much but the ion concentration or the ion concentration is directly proportional to my conductivity is increasing this way do you see the increase is less but in this case of strong electrolyte if I am adding 1 moles I am getting one mores of any classify Mosul miles remaining hundred moles I am getting hundreds of na plus and room also CA miles right in that case since it is very strongly apply the moment you put in water breaks it breaks so it the dissolution is not much dependent on the concentration of this solution but in case of weak electrolytes the moment I am increasing the concentration of the solution the dissociation is decreasing correct and that's way if I were increasing the concentration from 1 to 1000 but actually the conductivity will increase only from one to 50 and that's mine for the week a left right the the slope is not that steep right the rate of increase of conductivity on adding or increasing the concentration is not as high as we have any some strong electrolyte hope you understand this now let's understand the trend for moral conductivity now let's see the variation of molar conductivity we see the molar conductor is nothing but lambda m k by c so variation of K we have seen just now correct conductivity we have seen now if you see C is one concentration now concentration is also one of the parameter which we are changing and that is there in the derivative so overall what will happen the value of lambda M will decrease as we increase the concentration correct because concentration is also on the parameter so we have seen for strong electrolyte and we tillich be a weak electrolyte for strong electrolyte it means draw first this was of the weak a little light in the green color and this was for my strong electrolyte right this was strong and this was B and this was my key and this was my concentration right noise sheet of km docking what K by C and C's also a parameter here now since C was a parameter the moment you increase the value of C the whole value K by C will go down it mathematically and thus instead of getting straight it will be little lesser straight now if we talk about this is for the strong electrolyte example NaCl but if you talk about weak electrolyte it was already less right it was going in this the steep was less now if you dig if you divide that's this value by C and with the see increasing obviously then you will see X Y is equal to constant kind of graph right in the maths you have seen that right so you see this value because this value if you see is almost constant I think this is almost constant constant almost constantly we saw the slope of almost constant and as x and y we are changing this a bit it will give you this kind of graph so this is mathematically you will see lots of textbook has different explanation but if you think from experiment perspective right molar conductivity and connectivity is just the name you have given but actually the mechanism going inside is same like the weak electrolytes the moment you are increased concentration dissociates less but for strong electrolytes even if you increase concentration it dissociates almost completely and that's the reason why we have difference in the graph right for the normal conductivity the strong electrolytes the atom the the the step is pretty high right the increase in concentration leads to very high increase in conductivity but for weak identified increase in concentration leads to away minor increase in conductivity if you talk about the molar conductivity the same value just divided by see mathematical representation there you will see since there was a steep graph the moment divided you get this kind of rap and so almost constant you get X Y is equal to constant ago crap in this case of we correctly correct one thing to note here is now if this concentration is becoming almost zero then this graph goes in this direction something like this because that's the graph for x y is equal to constant now at these values when the concentration concentration almost approach zero then in that case my molar conductivity is given a new name and that is called limit molar conductivity it has a very great importance and that has a special symbol even two dots M naught because at this point you see the conductivity shoots up like in thing the molar conductivity should slap like anything here it becomes very high and at such a dilute well it is very difficult to find that kind of the conductivity conductivity using this kind of setup because see another day what we do is we uses which Stonebridge right we use this for Register's use wheat stone bridge right and then we some voltmeter here and we pass some AC source up correct now if I am being it very very tell you if I make it very very dilute solution very very dilute solution almost zero then in that case this is easy easy bar if everything in a very very dilute solution in that case what happens is this whole electrolyte won't even conduct electricity it will conduct at a very very small level right the resistance the the bulb will glow a very very minor level so at that point at that point it is very very difficult to measure the conductivity because these values are very high so it is very difficult to calculate the values of conductivity at that point and does vini different law orders and we will see that we have called Ross law who has proposed a lot to find the conductivity of strong and B electrolytes at low concentration effect to for weak electrolytes at low concentration correct in fact this thank you visit exam viacom to watch more videos Atem free online tests get three study materials find tutors and mentors and much more trying self again
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