Calculate the pH of a solution that contains 0.045 M HCl and 0.045 HClO2., HClO2 Ka...

Calculate the pH of a solution that contains 0.045 M HCl and 0.045 HClO2., HClO2 Ka = 1.1x10^-2

Expert Solution

HCl is strong acid while HClO2 is weak acid

HClO2 ionizes as HClO2+ H2O---------->ClO2-+ H3O+

Ka= [ClO2-] [H3O+]/[HClO2]

preparing the ICE table,

x= drop in concentration of HClO2 to reach equilibrium, at equilibrium [ClO2= [H3O+]=x

component HClO2 ClO2- H3O+

initial 0.045 0 0

change -x x x

equilibrium 0.045-x x x

Ka= x²/(0.045-x)= 1.1*10^-2 , when solved using excel x= [H3O+]=0.01742

HCl being strong ionizes completely as HCl+ H2O----------->H3O++Cl-

[H3O+] from HCl ionization =0.045

total of H3O+ =0.01742+0.045=0.06242

pH= -log[H3O+]= -log (0.06242)=1.2047

queen_honey_blossom answered 2 years ago

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