We’re being asked to calculate the equilibrium concentration of HNO2 if the percent dissociation of 2.00 M HNO2 is 0.58%.
Recall that the percent dissociation is given by:
Remember that weak acids partially dissociate in water and that acids donate H+ to the base (water in this case).
The dissociation of HNO2 is as follows:
HNO2(aq) + H2O(l) ⇌ H3O+(aq) + NO2–(aq)
Nitrous acid, HNO2, is a weak acid that is partially dissociated (broken apart) in aqueous solution. What is the equilibrium concentration of HNO2 if the extent of dissociation in 2.00M HNO2 is 0.58%? The equilibrium equation is shown below.
HNO2 (aq) ⇋ H+ (aq) + NO2- (aq)
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