Very good video good content but I have a question that if I take NaOH in beaker(analyte) and HCl in burette(titrant) what will happen to the graph will it reverse
Even then, you will get the same curve because both are strong electrolytes. In the beginning the conducatance will decrease due to decrease in the concentration of fast moving OH- (high ionic conductivity) ion till the equivalence point and then it will increase due to accumulation of fast moving H+ ions (high ionic conductivity).
I think the shape of the graph is not quite right. The hydronium ion is a better conductor than the hydroxide ion. The slope after the end point should at a lesser angle than before the end point.
It may need was you say, but we draw two straight lines using a scale with maximum number of points on it. The point of intersection will be considered as the end point for calculation purpose.
In this case all are strong electrolytes and get easily ionised immediately. But acetic acid is a weak acid, which dissociates sparingly and slowly. That is why it will have common ion effect which further suppresses it's ionisation.
When hydrochlorice acid (HCl(aq)) as a source of chloride ions, the conductance of the solution will be so high due to the presence of highly mobile H+ that it will mask any changes in conductivity due to the precipitation reaction. So solutions such as NaCl, KCl is used as a source of Cl- ions.
The corrected conductance can be calculated by multiplying the observed conductance either by total volume (V+V´) or by the factor (V+ V´)/V, where V is the initial volume of solution and V´ is the total volume of the reagent added.
Clearly introduced the topic and also a detailed information about the type of titration....was very helpful mam
Thank you.
Thank you so much it's really helpful for me 👍
Most welcome.
Very good video good content but I have a question that if I take NaOH in beaker(analyte) and HCl in burette(titrant) what will happen to the graph will it reverse
Even then, you will get the same curve because both are strong electrolytes. In the beginning the conducatance will decrease due to decrease in the concentration of fast moving OH- (high ionic conductivity) ion till the equivalence point and then it will increase due to accumulation of fast moving H+ ions (high ionic conductivity).
Very useful ,keep doing more viedos like this mam .
Sure. Thank you.
Very informative mam... really helpful for students.
Thank you sir.
Thank you for clearing this important concept 👍
Most welcome.
I think the shape of the graph is not quite right. The hydronium ion is a better conductor than the hydroxide ion. The slope after the end point should at a lesser angle than before the end point.
It may need was you say, but we draw two straight lines using a scale with maximum number of points on it. The point of intersection will be considered as the end point for calculation purpose.
your videos are useful ma....try to make a video on electrochemical machining
Thank you very much. Sure
wat is the name of the graph
Conductometric titration curves
why their is no common ion effect as Na on both side in Nacl and in NaoH?
In this case all are strong electrolytes and get easily ionised immediately. But acetic acid is a weak acid, which dissociates sparingly and slowly. That is why it will have common ion effect which further suppresses it's ionisation.
@@RevathiPurushothaman got it common ion only suppress the dissociation of weak electrolyte ..
Only in the beginning, it suppresses further. As such, weak electrolytes do not ionise easily.
Im from iraq but i can't understand because I m not good in English and I'm studying this experiment and I'm need understand the calculation
Awesome explaination mam😊
Thank you so much.
Can u please tell the plot of hcl vs agno3 conductometric ppt titration
When hydrochlorice acid (HCl(aq)) as a source of chloride ions, the conductance of the solution will be so high due to the presence of highly mobile H+ that it will mask any changes in conductivity due to the precipitation reaction. So solutions such as NaCl, KCl is used as a source of Cl- ions.
@@RevathiPurushothaman
Thank you...
Thank you maam really helpful for olympiad prep
Thank you very much. Its my pleasure.
Strong acid with weak base
thanks for this video. it was so helpful
Thank you very much 🙏🙏
Most welcome.
Tq madam 👍👍 it is very helpful
Glad that it helped you.
Understood clearly, brilliant explanation!
It's my pleasure. Thank you.
Very nice
Thank you.
Please give the above material in form of pdf in description link
Why equivalent point is arrived at pH4.
Thank you mam.. Very informative
Thank you. Glad that you liked it.
Very helpful video ❣️
Thank you.
Superb 🥰
Thank you.
Nice video and helpful..👌
Thank you. Nice that it helped you.
Thanks you soo much 🎉
You are most welcome.
Thankyou so much
Great efforts
Thank you.
thank u soo much mam.
You are most welcome.
Can I received this ppt
Thank you ma'am
Most welcome.
Thanks mam or maa
You are most welcome.
Thanks a loooought........................................................
You are most welcome
conductometric titration of hcl vs naoh, the end point refers to what -- maximum, minium or infinite ??? Plz reply
Complete neutralisation of HCl.
@@RevathiPurushothaman it means end point refers to minimum or infinite conductance ?
How to calculate corrected conductance plz explain mam
The corrected conductance can be calculated by multiplying the observed conductance either by total volume (V+V´) or by the factor (V+ V´)/V, where V is the initial volume of solution and V´ is the total volume of the reagent added.
Tysm mam❤️❤️
You are most welcome.
Darun mam ❤️
Best ever
Thank you very much.
wat is shape of the graph
We will not define the shapes.
Thankyou ♥
It's my pleasure.