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Ka Question
How would do I work this out:
In a 0.150 mol dm-3 solution of weak acid HX at 25C, 1.80% of the acid molecules are dissociated into ions.
Calculate Ka for the acid HX at this temp and state units.
Ka = [H+][X-] / [HX]
... is as far as I've got.
In a 0.150 mol dm-3 solution of weak acid HX at 25C, 1.80% of the acid molecules are dissociated into ions.
Calculate Ka for the acid HX at this temp and state units.
Ka = [H+][X-] / [HX]
... is as far as I've got.
assume that the volume is 1 litre
work out the moles of all components taking intyo account the fact that 1.8% of 0.15 moles of HX have dissociated = 0.0027 moles leaving only 0.1473 moles of acid
Moles of the other two components = 0.0027
sub into equation
work out the moles of all components taking intyo account the fact that 1.8% of 0.15 moles of HX have dissociated = 0.0027 moles leaving only 0.1473 moles of acid
Moles of the other two components = 0.0027
sub into equation
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