Question

Consider the reaction of nitrous acid in water where Ka = 4.0 ✕ 10−4. HNO2(aq) + H2O(l) equilibrium reaction arrow NO2−(aq) + H3O+(aq) (a) Which two bases are competing for the proton? (Select all that apply.) HNO2 H2O NO2− H3O+ (b) Which is the stronger base? HNO2 H2O NO2− H3O+ (c) In light of your answer to (b), why do we classify the nitrite ion (NO2−) as a weak base? The nitrite ion is a (stronger or weaker) base than water and produces (acidic or basic) solutions in water. When the nitrite ion is put into solution as the only major species, the competition is between the nitrite ion and the hydroxide ion for the proton. The resulting equilibrium lies far to the left producing a Kb value of (greater than, less than, or equal to) one. (Hydronium, hydroxide, nitrite, or nitrous acid) is the strongest base possible in water. Species that are classified as weak bases are stronger bases than water but are weaker bases than(Hydronium, hydroxide, nitrite, or nitrous acid) . Use an appropriate reaction to justify your answer. (Include states-of-matter at 25°C and 1 atm in your answer.)

Answer 1