Consider the example of dissolution of Na(s) in H2O(l) represented by the following equation:
\(Na(s) + H_2O(l) \rightleftharpoons NaOH(s) + H^+\). Now, In this case, which is conjugate acid and which is conjugate base?
Bronsted-Lowry acids and bases
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- Dhamnekar Winod
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Bronsted-Lowry acids and bases
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- ChenBeier
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Re: Bronsted-Lowry acids and bases
Its not working like this. The equation is not balanced according the charge.
2 Na + 2 H2O => 2 NaOH + H2 !!!!! No H+,
NaOH => Na+ + OH-
2 Na + 2 H2O => 2 NaOH + H2 !!!!! No H+,
NaOH => Na+ + OH-