How do you approach the task?
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Most likely, you should assume that the solubility of the CO2 depends proportionally on the partial pressure. (Cf.
)
In addition, you should probably start from constant temperatures (at higher temperatures gases dissolve significantly worse).
Furthermore, you should also assume that the concentration of carbonic acid is proportional to the CO2 content and that the degree of dissociation of carbonic acid remains constant (also the 2nd dissociation stage).
(a)
A pH of 5.4 means 10^(-5,4) H3 O^+ ions per H2 O molecule.
In the past, it would have been less by a factor of 315/375 after the above assumptions. From this, the proportion of ions can be calculated and the pH value therefrom.
(b)
Here I’d look in a table. It is impossible to calculate the degree of dissociation of carbonic acid with schools.
The task is a bit more complicated than I thought. It can’t be solved without tools.
So what happens quickly when you create a task at night by half three (e.g. to have something with current reference) and fails to pass through the clear head itself or/and let a colleague pass through.
I had to ask my then US professor again. To give me a reason to think.
We had a similar task then in Environmental Chemistry;)
The carbonic acid becomes carbonate or carbonate in water. Hydrogen carbonate and oxonium ions react. These are logically responsible for the pH value.
Then you have to reset 375 ppm to the amount or concentration.
(Edit: need to change my calculations)
at 375 atm CO2 would be the pCO2
To calculate, you need to apply the law of Henry
the constant would be K(H)=3.4*10^(-2 ) mol/(l*atm)
it results from:
Lastly, you need the GGW constant for the reaction H2CO3 <-> H+ and HCO3
This is 4.5 x 10^(-7)
The MGW for the reaction is therefore
In the dissociated state, the concentration in the denominator is the same, thereby simplifying the whole somewhat
Let’s dissolve this after x and take the SINNVOLLE solution
Finally, the pH value is 5.66 🙂
Hope you can help.