Problem: A 9.0×10−2 M solution of a monoprotic acid has a percent dissociation of 0.60%.Determine the acid ionization constant (Ka) for the acid.

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Establish the percent ionization equation and determine the acid ionization constant (Ka) for a monoprotic acid (9.0x10-2 M) which has a percent dissociation of 0.60%


Recall that the percent ionization is given by:


% ionization=[H3O+][HA]initial×100


Remember that weak acids partially dissociate in water and that acids donate H+ to the base (water in this case). 


The dissociation of HA is as follows:

HA(aq) + H2O(l)  H3O+(aq) + A(aq)


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Problem Details

A 9.0×10−2 M solution of a monoprotic acid has a percent dissociation of 0.60%.

Determine the acid ionization constant (Ka) for the acid.

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Based on our data, we think this problem is relevant for Professor Vassilian's class at RUTGERS.