Consider the dissociation of hydrocyanic acid in aqueous solution HCN - CN + H* for which K, is 4.9 x 101°. (i) Find the pH of a solution initially 102 M in HCN, and the degree of dissociation of the HCN, a. (ii) To this solution is added more CN' until [CN'] = (0.1 M. What is the new pH of the solution? (ii) Without making a new numerical cakculation, explain qualitatively how the degree of dissociation would change if the solution is diluted.

Consider the dissociation of hydrocyanic acid in aqueous solution HCN - CN + H* for which K, is 4.9 x 101°. (i) Find the pH of a solution initially 102 M in HCN, and the degree of dissociation of the HCN, a. (ii) To this solution is added more CN' until [CN'] = (0.1 M. What is the new pH of the solution? (ii) Without making a new numerical cakculation, explain qualitatively how the degree of dissociation would change if the solution is diluted.

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter16: Principles Of Chemical Reactivity: The Chemistry Of Acids And Bases

Section: Chapter Questions

Problem 116IL: Amino acids are an important group of compounds. At low pH, both the carboxylic acid group (CO2H)...

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