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? (Selectall 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 weclassify the nitrite ion (NO2−) as a weak base? The nitrite ion isa (stronger or weaker) base than water and produces (acidic orbasic) solutions in water. When the nitrite ion is put intosolution as the only major species, the competition is between thenitrite ion and the hydroxide ion for the proton. The resultingequilibrium lies far to the left producing a Kb value of (greaterthan, less than, or equal to) one. (Hydronium, hydroxide, nitrite,or nitrous acid) is the strongest base possible in water. Speciesthat are classified as weak bases are stronger bases than water butare weaker bases than(Hydronium, hydroxide, nitrite, or nitrousacid) . Use an appropriate reaction to justify your answer.(Include states-of-matter at 25°C and 1 atm in your answer.)
