pH of an Amphiprotic Species  [ENDORSED]

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Isa Samad 1L
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pH of an Amphiprotic Species

Postby Isa Samad 1L » Sat Dec 02, 2017 5:27 pm

How would you calculate the pH of a amphiprotic species, as it has the ability to both accept and donate hydrogen protons?
For example, how could you calculate the pH of 0.010 M NaHCO3. I understand that the sodium ion would be a spectator and thus, the HCO3 ion would contribute to the pH of the system. However in this case, how would you be able to tell whether it will accept or donate protons (ie: whether it will be a base or acid).

HCO3- (aq) + H2O(l) ⇌ H2CO3 (aq) + OH- (aq)


HCO3- (aq) + H2O(l) ⇌ CO3 2- (aq) + H3O+ (aq)

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Re: pH of an Amphiprotic Species  [ENDORSED]

Postby Chem_Mod » Sun Dec 03, 2017 1:56 pm

Great question.

You would need to calculate both equilibria using the equilibrium constants for each reaction.

Introduce yourself at the end of class.

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