7-6 This video describes how to calculate the pH for a general polyprotic acid, and carries out a numerical example for a 0.1 M solution of carbonic acid.
I have a final tomorrow and this greatly clears up titrations of polyprotic acids. I was always confused when to use Ka1 or Ka2 and you do a great job telling which one to use.
when writing a diprotic acid reaction of sulfuric acid, H2SO4 + H2O --> SO4 + H3O, there's a missing hydrogen on the product side, so how do you write the correct equation?
This method of yours may be useful. But one should keep in mind that equilibrium concentrations never change . In the second equation the equilibrium concentration of hydronium is greater than that in the first and that's wrong . The true way of solving this problem is by writing proton balance and mass balance equations and then use approximations
I have a final tomorrow and this greatly clears up titrations of polyprotic acids. I was always confused when to use Ka1 or Ka2 and you do a great job telling which one to use.
This was an amazingly helpful and clear video. Thank you!
You are really good at explaining!
Thank you very much! Such a great explanation!
Helped me understand the material very well for my final tomorrow. Thank you.
You're a great teacher. Thank you
Great Video, this helped me a lot! Thanks!
Very helpful video. Thanks!
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extremely helpful lecture. Thanks
great explanation. thank you!
Great video, thank you!
Great explication, thank you
Thank you so much! Help so much!!
extremely helpful
very helpful Thank you
Nice. Thank you.
Thank you!
when writing a diprotic acid reaction of sulfuric acid, H2SO4 + H2O --> SO4 + H3O, there's a missing hydrogen on the product side, so how do you write the correct equation?
this video rocks!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!
very helpful. fyi is the ka1 written incorrectly?
Thank you sir
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Thanks
Why you do t change H2CO3 conc. after HCO3- disociated, why it's not [H2CO3]=0,1-2,1*10^-4 - y
This method of yours may be useful. But one should keep in mind that equilibrium concentrations never change . In the second equation the equilibrium concentration of hydronium is greater than that in the first and that's wrong . The true way of solving this problem is by writing proton balance and mass balance equations and then use approximations
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How do you got pH =3.89
PH =3.68
@@ramavittal3494 You take the negative log of H+ Ion Concentration. -log[H+] = -log[2.1X10^-4] ~= 3.68 ; pH = 3.68
Thank you!