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Self-test6A.2B

Posted: Mon Dec 02, 2019 12:25 pm
by AnvitaaAnandkumar_1B
(a)Identify the Brønsted acids and bases in both reactants and products in the proton transfer equilibrium HCO3-(aq) + NH4+(aq) ---> H2CO3(aq) + NH3(aq).
(b) Which species (not necessarily shown explicitly) are Lewis acids and which are Lewis bases?

Re: Self-test6A.2B

Posted: Mon Dec 02, 2019 12:37 pm
by 805394719
Because Bronsted acids are defined to be the molecules to that donate a proton (H atom), NH4+ would be the Bronsted acid here as it is the one that donated a proton to HCO3- and became NH3. Lewis acids are defined to be the lone pair acceptors so NH4+ would be considered a Lewis acid since it is positively charged which makes it more likely to accept a lone pair of electrons. Therefore, the Bronsted and Lewis base would be HCO3-.

Re: Self-test6A.2B

Posted: Mon Dec 02, 2019 12:41 pm
by MAC 4G
805394719 wrote:Because Bronsted acids are defined to be the molecules to that donate a proton (H atom), NH4+ would be the Bronsted acid here as it is the one that donated a proton to HCO3- and became NH3. Lewis acids are defined to be the lone pair acceptors so NH4+ would be considered a Lewis acid since it is positively charged which makes it more likely to accept a lone pair of electrons. Therefore, the Bronsted and Lewis base would be HCO3-.


Thank you, this was really helpful.

Are Bronsted acids and bases the same as Lewish acids and bases?

Re: Self-test6A.2B

Posted: Tue Dec 03, 2019 9:48 pm
by AnvitaaAnandkumar_1B
805394719 wrote:Because Bronsted acids are defined to be the molecules to that donate a proton (H atom), NH4+ would be the Bronsted acid here as it is the one that donated a proton to HCO3- and became NH3. Lewis acids are defined to be the lone pair acceptors so NH4+ would be considered a Lewis acid since it is positively charged which makes it more likely to accept a lone pair of electrons. Therefore, the Bronsted and Lewis base would be HCO3-.


Would NH4+ be considered the Lewis acid or would it simply be H+?