Answer to Question #140231 in General Chemistry for Sarah

Question

Calculate the pH of a solution that is 0.134 M in benzoic acid (C6H5CO2H) and 0.120 M in hypobromous acid (HBrO).

Answer 1

The acidic and basic nature of the solution is determined by the pH of a solution. The pH range in the pH scale is 0 to 14. The pH below seven indicates that the solution is acidic. The pH above seven indicates that the solution is basic.

the pH of a solution that is 0.134 M in benzoic acid (C6H5CO2H) 

0.120 M in hypobromous acid (HBrO).

Ka = [H⁺][B^-]/[HB]Benzoic acid dissociates to C6H6COO^- and H⁺ -

this is a 1:1 ratio so the concentrations are equal hence [H⁺][B^-] = [H⁺]²6.3x10-5 = [H⁺]²/0.16.3x10-6 = [H⁺]² 

therefore H⁺ concentration is 0.0025MpH = -log([H⁺])

therefore pH = -log(0.0025M) = 2.61