Diagnostic Exam

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sen117
Posts: 8
Joined: Fri Jan 10, 2020 2:51 pm

Diagnostic Exam

Post by sen117 » Mon Mar 09, 2020 1:06 pm

In Bicarbonate buffer system H+ (aq) + HCO3- (aq) ↔ H2CO3 (aq) ↔ H2O (l) + CO2 (g)
If you increase water concentration, wouldn't it stress the side of the product and shift the reaction to left (increase proton/decrease pH)?

I understand water is neutral in pH, but I wanted to understand this in terms of le chatelier's principle. Does water not play a role here, because it is Liquid instead of Aqueous or Gas (similar to calculating Keq)?

Thank you for your help in advance!
NS_Tutor_Mathias
Posts: 543
Joined: Sat Mar 30, 2019 8:39 pm

Re: Diagnostic Exam

Post by NS_Tutor_Mathias » Mon Mar 09, 2020 5:08 pm

You are totally correct: Solids and liquids are not part of our equilibrium expressions.

(You may say that doesn't make perfect sense, and I'm pretty sure in a practical sense, sufficient dilution would the buffer should allow you to dissolve more gaseous CO2 and convert it to carbonic acid. But this isn't true as far as our equilibrium expressions are concerned. Do you have the number this question is from?)
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