Which of the following Lewis acid-base reactions are not Bronsted acid-base reactions ?
a) Ag +(aq) + 2NH3(aq) = Ag(NH3)2 +(aq)
b) 2HCl(aq) + Ca(OH)2(aq) --> CaCl2(aq) + 2H2O(l)
c) Al(OH)3(s) + OH-(aq) --> Al(OH)4-(aq)
d) H2SO4(aq) + H2O(l) --> H3O+(aq) + HSO4-(aq)
2006-12-09 04:24:36 · 2 answers · asked by patternpile 1 in Science & Mathematics ➔ Chemistry
According to the Bronsted-Lowry definition, acids are H+ donors and bases are H+ acceptors. Therefore any Lewis acid-base reaction that doesn't invlove the transfer of an H+ is not a Bronsted-Lowry acid base reaction. In the examples above, B and D invlove H+ transfer, so are Bronsted-Lowry reactions, but A and C are not.
2006-12-09 04:28:15 · answer #1 · answered by Amy F 5 · 0⤊ 0⤋
a and c is not bronsted acid base reaction because the product must contain both conjugate acid and its conjugate base but a and c doesn't have the conjugate acid and base.
2006-12-09 04:34:15 · answer #2 · answered by lynn 2 · 0⤊ 0⤋