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Question 6A.11

Posted: Tue Nov 12, 2019 12:49 pm
by Ayush Ray 1I
Write the chemical equations of the two proton transfer
equilibria that demonstrate the amphiprotic character of (a) HCO3-; (b) HPO4 2-
Identify the conjugate acid–base pairs in each case.

Re: Question 6A.11

Posted: Fri Nov 15, 2019 10:15 pm
by AGulati_4A
H2CO3 and H3PO4, the compounds in the questions are the conjugate bases and the other would be the acid

Re: Question 6A.11

Posted: Wed Nov 27, 2019 10:37 am
by ALegala_2I
HCO3- and HPO4 2- can both accept and donate protons. In this way, they are considered amphiprotic and can be used as an acid or a base in the reaction. If they are an acid, they lose the hydrogen in the reaction. If they are basic, they gain a hydrogen in the reaction.

Re: Question 6A.11

Posted: Wed Nov 27, 2019 11:58 am
by ishaa Diwakar 4E
H2CO3 and H2SO4 are considered diprotic, meaning they usually lose two protons as anions. So, when they lose only one, they are able to lose one more and act as an acid, even with a negative charge.

Re: Question 6A.11

Posted: Wed Nov 27, 2019 2:08 pm
by Laura WM 3I
ishaa Diwakar 4E wrote:H2CO3 and H2SO4 are considered diprotic, meaning they usually lose two protons as anions. So, when they lose only one, they are able to lose one more and act as an acid, even with a negative charge.


What characteristics of these compounds shows that they are diprotic?

Re: Question 6A.11

Posted: Fri Nov 29, 2019 6:56 pm
by ishaa Diwakar 4E
The main characteristic is that they have the potential to donate two protons (H+) since there are two H atoms per molecule. For example, with H2SO4, the first equation would be: H2SO4 + H2O --> HSO4- + H3O+ , and the second equation would be: HSO4- + H2O --> SO4 2- + H3O+