1.When completing net ionic equation problems (when one aqueous solution reacts

Question

1.When completing net ionic equation problems (when one aqueous solution reacts with another aqueous solution), explain why you do not further split up H2O (l) into H+ (aq) and OH- (aq). Note: only mentioning that it is a liquid is not good enough of an explanation.
1.When completing net ionic equation problems (when one aqueous solution reacts with another aqueous solution), explain why you do not further split up H2O (l) into H+ (aq) and OH- (aq). Note: only mentioning that it is a liquid is not good enough of an explanation.
Note: only mentioning that it is a liquid is not good enough of an explanation.

Explanation / Answer

H2O has very weak electrolyte because its dissociation constant is 1.0*10^-14 which is very small.

This can be seen as an equilibrium process:

H2O (l) <—> H+ (aq) + OH- (aq)

Kw = [H+][OH-] = 10^-14

so,

concentration of H+ and OH- is very less in H2O

So, H2O is assumed non ionisable and we dont dissociate and write it as H+ and OH-

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