Write an equation in which H2PO3 acts as an acid. (Use the lowest possible coefficients. Be sure to to specify states such as (aq) or (s). If a box is not needed, leave it blank.) H;PO3 (ag) + OH (ag) + Write an equation in which H2PO3 acts as an base. (Use the lowest possible coefficients. Be sure to to specify states such as (aq) or (s). If a box is not needed, leave it blank.) H,PO3 (ag) + H30* (ag) =

According to Bronsted Lowry concept, an acid is a substance that donates proton in solution while base is one that accepts a proton. After an acid loses a proton in aqueous medium, it furnishes hydronium ion and conjugate base of the acid. So, an acid and conjugate base differ by a proton. Answer a) When H2PO3- is an acid, it can donate proton in solution. In presence of hydroxide ion, the proton reacts with hydroxide to form water. After donating a proton, the conjugate base of H2PO3- is formed which is HPO3 2-. The reaction involved is as shown below: H2PO3 - (aq) + OH-aq ↔HPO3 2- (aq) + H2O l Hence, the answers are HPO3 2- (aq) + H2O l.Answer b) When H2PO3- is a base, it can accept protons from solution. In presence of hydronium ion, the proton from hydronium reacts with H2PO3- to form the conjugate acid i.e. H3PO3 and water. The reaction involved as shown below: H2PO3 - (aq) + H3O+aq ↔H3PO3 (aq) + H2O l Hence, the answers are H3PO3 (aq) + H2O l.