polyprotic acids calculating pH

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A large number of acids can give two or more protons on dissociation and these are referred to as polyprotic acids.
A polyprotic acid always dissociates in a stepwise manner, one proton at a time. Note that the acid dissociation constants are labelled ka1 and ka2. The numbers on the constants refer to the particular proton of the acid that is ionizing. Thus, ka1 always refers to the equilibrium involving removal of the first proton of a polyprotic acid.
Most acids have a ka2 that is much smaller than ka1. This can be explained by the fact that the second H+ has to leave from a negatively charged species. For example in HSO3- - electrostatic attraction has to be overcomed – while the first H+ from a neutral compound H2SO3.

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[faykey]

what pen is used in that video? It looks like it writes very well...

[phatsimoleepo]

can we use that experssion to find the concentration of HSO4-? if so, whats the ratio from h2so4?

[phatsimoleepo]

i'm saying this because i'm only given pH and volume of the titration base (burette readings) and i don't know what to do

[tinak]

How do you how what the Ka1 and Ka2 values are?

[MusicMeister]

Wait, why did you cancel out the (1+x) and (1-x) in the expression (1+x)x/(1-x)? They aren't like terms. Can you explain your math please?

[felixmcintyre]

Isn't the concentration of H+ actually 1.012, and therefore pH = -0.005?

[TheMustafa]

This was the greatest video on pH calculation so far! It's way better than those who talk about their 6 years old cat while solving the equation. Please more!

[HarshRajAlwaysfree]

U should have made a case with a weak acid

cuz then it would have been complex and fun to watch people panic

<:)