Tutorial Titration of Hydrochloric Acid and Sodium Hydroxide
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- čas přidán 21. 08. 2024
- In this tutorial I set up a burette and use a pipette to load 10 cm3 of a 2 Molar solution of Hydrochloric acid into a conical flask. Then I fill a burette with an unknown concentration of Sodium Hydroxide. I then titrate the sodium Hydroxide against the known concentration of Hydrochloric acid, using Phenolphthalein as an indicator.
Finally I go through the calculation to work out the concentration of the unknown Sodium Hydroxide.
Thank you very much, you are so kind for going out of your way to make this video. It helps so much!
Thank you!
thanks Philip
What an explanation! !!
This was really helpful
Thank you this was very helpful. Why did you let a little bit of the sodium hydroxide into the beaker before doing the burette reading?
To make sure the burette was completely filled with Alkali. If I hadn't the reading would have been wrong as the first cc would fill up the burette and not go into the acid and neutralise it.
Thank u sir it's really helpful
Thank you sir
Thanks
Very cool
thanks for the tutorial
You are welcome.
Awesome
Thanks boss
can hydrochloric acid mixed with sodium hydroxide and methyl can it wash away ink
Thanks alot .. what if we add some water to the solution after is added to the buret? Is that correct in titration method?
In a normal titration you would make up the correct concentration first then put it in the Burnett, that way you know the concentration.
@@PhilipRussell I saw some doctors add water to solution ( water in flask after add sol. also water to buret after add solution!!! Why🤕
@@user-xo2mj7ps8l I can tell you that they are diluting the solution but I can't really tell you why. The amount of substance in the burette will stay the same but its concentration will change, this won't make it good for doing calculations..
@@PhilipRussell 👍🌺
So what was the concentration of the acid in %? How do you convert Mole to %?
The mole is the measurement of the amount of substance. So 2M HCl means that there is 2 x 36.5g of HCl in every 1000 cm3. Where did I get 36.5 from? The numbers are from the molecular mass .In this case there is 73 g in every 1000 cm3. The % is 73/1000x100.
Now the problem comes when you work in % that a strength of 7.3% is pretty useless when you want to do chemistry.
@@PhilipRussell So the 73g of HCL is the mass of the liquified HCL gas (without water)? Is that correct?
@@PhilipRussell So 12M HCL would be 43.74% right?
@@Berghiker yes
@@Berghiker yes
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