Problem: When KNO2 is dissolved in water, which of the following is the principal acid-base equilibrium?A) NO2- (aq) + H2O(l) ⇌ HNO2(aq) + OH-(aq)B) HNO2(aq) ⇌ H+ (aq) + NO2-(aq)C) K(H2O)6+(aq) ⇌ K(H2O)5OH(aq) + H+ (aq)D) NO2- (aq) + H2O (l) ⇌ HNO3(aq) + H+ (aq)

FREE Expert Solution

We’re being asked to determine principal acid-base equilibrium when KNO2 is dissolved in water.


Ionic salts are made up of positively charged ion (cation) and a negatively charged ion (anion). To determine if the ionic salt would be acidic, basic, or neutral, we need to identify the acidity or basicity of the cation and anion.

For cations:

transition metal

▪ charge of +2 or higheracidic
▪ less than +2 → neutral solution

main group metal

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Problem Details

When KNO2 is dissolved in water, which of the following is the principal acid-base equilibrium?

A) NO2(aq) + H2O(l) ⇌ HNO2(aq) + OH-(aq)

B) HNO2(aq) ⇌ H+ (aq) + NO2-(aq)

C) K(H2O)6+(aq) ⇌ K(H2O)5OH(aq) + H+ (aq)

D) NO2- (aq) + H2O (l) ⇌ HNO3(aq) + H+ (aq)

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Our tutors have indicated that to solve this problem you will need to apply the Bronsted Lowry Acid and Base concept. You can view video lessons to learn Bronsted Lowry Acid and Base. Or if you need more Bronsted Lowry Acid and Base practice, you can also practice Bronsted Lowry Acid and Base practice problems.