6D.11b

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Simon Dionson 4I
Posts: 107
Joined: Sat Sep 14, 2019 12:17 am

6D.11b

Postby Simon Dionson 4I » Mon Dec 02, 2019 5:35 pm

If we were to dissolve Na2CO3 in water, would CO3 2- be completely or partially protonated by the water?

i.e.

CO3 2- + 2H2O -> H2CO3 + 2OH-

vs

CO3 2- + H2O -> HCO3- + OH-

Could the same be said for bases with a negative charge greater than 1? thanks.

Ryan Yee 1J
Posts: 101
Joined: Sat Aug 17, 2019 12:16 am

Re: 6D.11b

Postby Ryan Yee 1J » Mon Dec 02, 2019 7:10 pm

Well, for the purposes of the question, either way that it goes, the concentration of OH- would be high and result in a basic solution, but I would imagine that carbonate would form both of these compounds, since it is a weak acid and not fully dissociated. Because it isn't fully dissociated, HCO3- and H2CO3 are both present within the water.


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