(a) Place the following species on order of increasing acid strength. Explain yo
ID: 514028 • Letter: #
Question
(a) Place the following species on order of increasing acid strength. Explain your response. (i) HOCl, HOCIO, HOCIO_2 (ii) H_2O, H_2S, H_2Se (bond energies: H-O, 467 kJ mol^-1: H-Se, 363 kJ mol^-1: H-Se, 276 kJ mol^-1) (iii) NaHCO_3, Na_2CO_3 (iv) HBr HI, HF b. Explain how the Bronsted-Lowry theory of acids and bases is explained by the Lewis acid-base theory. Your response must communicate clear explanations of both theories. Feel free to use illustrations along with words in your response. Your response will be graded on accuracy, completeness and clarity.Explanation / Answer
(2)
(i) HOCl < HClO2 < HClO3
The anions of these acids are stabilised by resonance after the loss of H+ ion. In each of the anion negative charge is present on Oxygen. It is shared by other oxygen atoms through resonance. SInce in ClO3- ion negative charge is shared by 3 oxygen atoms it is more stable followed by ClO2- in which negative charge is shared by 2 oxygen atoms followed by ClO- in which negative charge is shared by only one oxygen, so it is unstable.
Due to the stability of their conjugate bases
(ii) H2O < H2S < H2Se
Due to decrease in bond dissociation enthalpy. Easy the bond dissociated easy the availability of H.
(iii) Na2CO3 < NaHCO3
Due to the prsence of one acidi proton in NaHCO3 it is more acidic.
(iV) HF < HBr < HI
Due to increase of polarising power of conjugate base. More is the polarising power more is the ability to pull the electrons and bear around it self.
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