a. Write the balanced chemical equation for the reversible acid–base reaction that takes place between nitrous acid (HNO 2 ) and water. b. Write the equilibrium constant expression for this reaction....

a. Write the balanced chemical equation for the reversible acid–base reaction that takes place between nitrous acid (HNO 2 ) and water. b. Write the equilibrium constant expression for this reaction. c. Name and draw the Lewis structure of the conjugate base of nitrous acid. d. For nitrous acid, Ka = 4.0 ? 10 -4. What is the value of pKa? e. Which are there more of once the reaction in part a has reached equilibrium, reactants or products? f. For carbonic acid (H2CO3), Ka = 4.4 ? 10 -7 . Which is the stronger acid, nitrous acid or carbonic acid? g. Which is the stronger base, the conjugate base of nitrous acid or the conjugate base of carbonic acid? h. Assuming that the reaction in your answer to part a is at equilibrium, what will happen to restore equilibrium if the pH is lowered by addition of H 3 O + , a net forward reaction or a net reverse reaction? i. Over what pH range would a solution containing nitrous acid and its conjugate base be effective as a buffer?