Reacting OH- with CO2 in a Buffer Solution: Which Molecule Takes Priority?

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When OH- is added to a buffer solution containing CO2, it primarily reacts with CO2 to form HCO3- and H+, rather than directly with H+. This reaction can be represented as CO2 + OH- <-> HCO3- + H+, although balancing issues suggest complexities in the reaction dynamics. The predominant acid in the solution typically dictates the reaction pathway, which can be ambiguous in less clear-cut scenarios. Generally, it is assumed that OH- will react with available H+, influencing the equilibrium of other acid/base dissociations according to LeChatelier's principle. Understanding these interactions is crucial for predicting the behavior of buffer solutions in various chemical contexts.
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Here's the buffer solution H2O + CO2 <=> HCO3- + H+ so the question is why when OH- is added to the solution it reacts with CO2 to get HCO3- and H+ :confused: how do you know which one will OH- react with?Why doesn't the OH- react with the H+ :confused:
 
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Are you telling that reaction that takes place is

CO2 + OH- <-> HCO3- + H+

It can't be balanced (which usually means that such reaction doesn't take place).
 
So what happen when OH- is added to the buffer?
 
It should react with the predominant acid in the solution.
 
ermz...so how do you know which one is the acid?I mean in cases where the acid and base is not so obvious?
 
In general you may safely assume that OH- always reacts with H+. That in turn may move equilibrium of other reactions (acid/base dissociations) according to the LeChatelier's principle.
 
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