# Problem: A 0.142 M solution of a monoprotic acid has a percent dissociation of 1.60%. Determine the acid ionization constant (Ka) for the acid.

###### FREE Expert Solution

We’re being asked to calculate the acid ionization constant (Ka) for a monoprotic acid if a 0.142 M solution has a percent dissociation of 1.60%.

Recall that the percent ionization is given by:

(Let HA → monoprotic acid)

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)

84% (215 ratings) ###### Problem Details

A 0.142 M solution of a monoprotic acid has a percent dissociation of 1.60%. Determine the acid ionization constant (Ka) for the acid.

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