I'm wondering if you titrate a polyprotic acid, say, HX3POX4, with a strong base, and you successfully pass the first equivalence point and are maybe at the pH=pKa2 point now, how would you find the concentration of HX3POX4?
Is there none left? I don't have a specific homework question, I'm just wondering.
Attempt at a solution:
I thought maybe you would find the equilibrium concentration of HX2POX4X−, find the pH, and use the pH to find OHX−. Then, you could write the equilibrium, HX2POX4X−+HX2O−⇀↽−OHX−+HX3POX4, and without making an ICE table, substitute your equilibrium values into the Ka expression.
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