Question 6A.11

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Ayush Ray 1I
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Joined: Sat Sep 14, 2019 12:15 am

Question 6A.11

Postby Ayush Ray 1I » Tue Nov 12, 2019 12:49 pm

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.

AGulati_4A
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Joined: Sat Sep 07, 2019 12:19 am

Re: Question 6A.11

Postby AGulati_4A » Fri Nov 15, 2019 10:15 pm

H2CO3 and H3PO4, the compounds in the questions are the conjugate bases and the other would be the acid

ALegala_2I
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Joined: Thu Jul 11, 2019 12:17 am

Re: Question 6A.11

Postby ALegala_2I » Wed Nov 27, 2019 10:37 am

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.

ishaa Diwakar 4E
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Joined: Wed Sep 11, 2019 12:17 am

Re: Question 6A.11

Postby ishaa Diwakar 4E » Wed Nov 27, 2019 11:58 am

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.

Laura WM 3I
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Re: Question 6A.11

Postby Laura WM 3I » Wed Nov 27, 2019 2:08 pm

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?

ishaa Diwakar 4E
Posts: 56
Joined: Wed Sep 11, 2019 12:17 am

Re: Question 6A.11

Postby ishaa Diwakar 4E » Fri Nov 29, 2019 6:56 pm

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+


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