Problem: 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) 

FREE Expert Solution
96% (12 ratings)
FREE Expert Solution

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:


% dissociation=[H+][HNO2]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 HNO2 is as follows:

HNO2(aq) + H2O(l)  H3O+(aq) + NO2(aq)


96% (12 ratings)
View Complete Written Solution
Problem Details

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)

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Weak Acids concept. If you need more Weak Acids practice, you can also practice Weak Acids practice problems.

What is the difficulty of this problem?

Our tutors rated the difficulty ofNitrous acid, HNO2, is a weak acid that is partially dissoci...as medium difficulty.

How long does this problem take to solve?

Our expert Chemistry tutor, Sabrina took 4 minutes and 3 seconds to solve this problem. You can follow their steps in the video explanation above.

What professor is this problem relevant for?

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