Now he is twisting it as if I was the one who picked these numbers from wiki....which are indeed for water without any CaCO3 buffer in it. Now he admits it has nothing to do with sea water and talks as if it wasn't him eho copied and pasted the numbers from that wiki-page.
All I did was showing how way off the mark his claim was.
I specifically stated in my first calcs that they had nothing to do with seawater. I specifically said exactly what my calcs were for, to show that very small concentrations of CO2 can change pH significantly, and specifically added the caveats that the oceans are very different. I misrepresented nothing, while you're wildly misrepresenting what I said.
So "mamooth" show me were in your post you addressed the partial pressure for CO2.
It's on the tables, so why do I need to address it more? I could run the numbers, but since the table already did so, what's the point? A good engineer knows when to use the tools given him.
If you had any idea whatsoever how to do the math then why did you not do it for the pH range of 8.25 to 8.14 ?
Because I'm not sure of the carbonate and bicarbonate buffer concentrations, the calcium ions that in turn react with the buffers, or the equilibrium constants of all associated reactions. And even if I did know all that, it's still a very difficult thing to do. Two buffers and a 3rd substance also reacting with the buffers? That's going beyond the basic water chemistry I learned. It's more than I can handle, and I've always said so.
If I wanted to I could and I would not be confined to the numbers of that wiki-page which don`t go above pH7.
I detect a very strong aroma of bullshit coming from that claim.
Go on, run those numbers for seawater, including the effects of the buffers and the calcium ions. That is, if you're not bullshitting us.
44 times 3.36 ^(-8) = 0.00000014784 grams or ~ 1.5 E-7 grams per liter not 1.5 E-6
Nope. Multiplication fail on your part. I'm correct, and you're wrong.
So before you start lecturing us about pH and chemistry you should first learn how to use exponents and how to convert ppm correctly to percent.
Given I got it right and you botched the exponents, the irony is amusing. Before you lecture me again, double-check your work. I double-check my work, which is why I don't botch it like you do.
And after you did then come back here and tell us what the pH would be if you got a solution of 1.5 ^(-7) grams of CO2 gas in water.
Solubility isn't expressed in grams. Again, I recommend double-checking your work.
The number you copied from the table [CO2](mol/L) was 3.36E-8 moles/liter
That's definitely the correct column/number to use, since the concept being discussed is how much CO2 was absorbed by the oceans. Since the equilibrium constant is so small, that means 99+% of the CO2 does not disassociate, so we can quickly estimate [CO2] as CO2 absorbed divided by volume (or mass, depending how you look at it). There's no need to mess with disassociation constants, because the table does that calculation.
Since you have zero knowledge about chemistry you don`t know the difference between [CO2] and [CO3]2- and took that number as dissociated [CO3]2- which is the anion of carbonic acid.
You're really confused about this. Since everyone is discussing how much CO2 in the atmosphere is absorbed by the ocean, the number to use is CO2 absorbed by the ocean. That is, [CO2]. You're off in left field when you say we should take the value of [CO2] and then declare [CO3]2- must be the same. That's just wacky, and would have earned you a failing grade in freshman chemistry.