Amphoteric Compounds: Ka of H2PO4 & HS Reaction Explained

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SUMMARY

The reaction between H2PO4 and HS is represented by the formula H2PO4 + HS <--> HPO4 + H2S. The dissociation constant (Ka) values indicate that H2PO4, with a Ka of 6.3 * 10^-8, acts as the acid, donating a proton, while HS, with a Ka of 1.3 * 10^-13, acts as the base, accepting a proton. This conclusion is based on the comparative strength of the acids involved, confirming that H2PO4 is the stronger acid in this amphoteric reaction.

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Homework Statement



The Ka of H2PO4 is 6.3 * 10^-8. The Ka of HS is 1.3 * 10^-13. Write a formula for the reaction of these substances and explain your results. Both are amphoteric.

The Attempt at a Solution



The formula is:

H2PO4 + HS <--> HPO4 + H2S

I figured that the H2PO4 will act more like the acid in this particular situation because it has a higher value of Ka. So, H2PO4 will donate a proton while HS will receive a proton.

Is this the correct train of thought?

Thanks.
 
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Seinfeld4 said:
Is this the correct train of thought?

Yes. Just don't ignore charges - use [noparse]-[/noparse] to get -.
 

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