The equation is N1V1=N2V2 no matter what is in burette and in conical, however generally we fill known compound in burette, but if you need to perform number of titrations then we fill common solution in burette, thanks for watching and your concern
Dear you can calculate by equation N1V1= N2V2, suppose you want to prepare 100 ml solution of N /500 from N/10; V1*(N/10)=100ml *(N/ 500) in this manner you will get V1 = 2 ml that is you have to add 2ml of N/10 solution in 100 ml measuring flask and then make up to 100 ml, but I would suggested you use 10 ml in 500 ml because you can easily measure the volume in less volume more chances of error, I hope this will work for you, thank you
Thanks for watching, you please use the formula wt = (n/44)x molecular weight of sodium thiosulfate x volume in litre; the weight you get from this formulae dissolve that in to the volume you need to prepare e.g you wish to prepare in 100 ml then put (100 ml/1000 ml i.e., 0.1 litre) put 0.1 litre in the formula. Here important point is in case of normality we use equivalent weight (= molecular weight/ oxidation state) in case of sodium thiosulfate vs iodine solution the change in oxidation state= 1, therefore in this case equivalent weight= molecular weight; if you are doing some other titration or for some other purpose then you can write me back the equivalent weight may be changed, if this is helpful to you give me a 👍, thank
Please elaborate your question if it is not discussed in the video, actually for redox titrations we should do the calculation in molarity then we exact results, in case of normality we should know about the n factor for the reactants in the working conditions. Thanks for watching 🙏
Very nice explanation
Thank you
For 100 ml calculation=248*0.01*100÷1000
Then it would be 0.248 g of sodium thiosulphate....am i right?
Yes, after preparation standardization is required, thanks for watching
Mam but burate m to known concertration hoti h or conical m unknown concertration , us according ye normality to k2cr2o7 ki aaygi
The equation is N1V1=N2V2 no matter what is in burette and in conical, however generally we fill known compound in burette, but if you need to perform number of titrations then we fill common solution in burette, thanks for watching and your concern
Mam from n/10 sodium thiosulphate how we wil prepre n/500
Dear you can calculate by equation N1V1= N2V2, suppose you want to prepare 100 ml solution of N /500 from N/10; V1*(N/10)=100ml *(N/ 500) in this manner you will get V1 = 2 ml that is you have to add 2ml of N/10 solution in 100 ml measuring flask and then make up to 100 ml, but I would suggested you use 10 ml in 500 ml because you can easily measure the volume in less volume more chances of error, I hope this will work for you, thank you
Mam how to prepare n/44 sodium thiosulfate solution
Thanks for watching, you please use the formula wt = (n/44)x molecular weight of sodium thiosulfate x volume in litre; the weight you get from this formulae dissolve that in to the volume you need to prepare e.g you wish to prepare in 100 ml then put (100 ml/1000 ml i.e., 0.1 litre) put 0.1 litre in the formula. Here important point is in case of normality we use equivalent weight (= molecular weight/ oxidation state) in case of sodium thiosulfate vs iodine solution the change in oxidation state= 1, therefore in this case equivalent weight= molecular weight; if you are doing some other titration or for some other purpose then you can write me back the equivalent weight may be changed, if this is helpful to you give me a 👍, thank
Mam why we use KI ? Purpose?
Iodine (I2) is insoluble in water therefore KI is used to make it I3- ion which is soluble in water, thanks for watching
I'm not getting correct normality..plz do explain
You'll not get exact N/10 it should ranges between 0.97 N/10 or 1.01N/10
You've to calculate with that, it's not at all problematic
Thank you!!
How much normality
Please elaborate your question if it is not discussed in the video, actually for redox titrations we should do the calculation in molarity then we exact results, in case of normality we should know about the n factor for the reactants in the working conditions. Thanks for watching 🙏
Ki is not use
KI is or KIO3 potassium iodate is an essential part of iodometric titrations