A buffer solution is made that is 0469 M in HCIO and 0469 M

A buffer solution is made that is 0.469 M in HCIO and 0.469 M in KCIO If Ka for HCIO is 3.50 × 10-8, what is the pH of the buffer solution? pH= Write the net ionic equation for the reaction that occurs when 0.101 mol HI is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H3O instead of Ht)

Solution

PKa    = -logka

          = -log3.5*10^-8

         = 7.4559

[HClO]   = 0.469M

[KClO]   = 0.469M

PH   = Pka + log[KClO]/[HClO]

          = 7.4559 + log0.469/0.469

          = 7.4559+0

       = 7.4559 >>>>answer

molarity of HI   = no of moles/volume in L

                         = 0.101/1 = 0.101M

     HI + H2O ---------------> I^- + H3O^+

0.101M                             0.101M