A solution has [c6h5cooh] = 0.100 m and [ca(c6h5coo)2] = 0.200 m. ka = 6.3 × 10−5 for c6h5cooh. the solution volume is 5.00 l. what is the ph of the solution after 10.00 ml of 5.00 m naoh is added?

6.8 is the pH of the solution after 10 ml of 5M NaOH is added.

Explanation:

Data given:

Molarity of C6H5CCOH = 0.100 M

molarity of ca(c6h5coo)2  = 0.2 M

Ka = 6.3 x 10^-5

first pH is calculated of the buffer solution

pH = pKa+ log 10

pKa = -log10[Ka]

pka = -log[6.3 x10^-5]

pKa = 4.200

putting the values to know pH of the buffer

pH = 4.200 + log 10

pH = 4.200 + 0.3

    pH  = 4.5 (when NaOH was not added, this is pH of buffer solution)

now the molarity of the solution is calculated after NaOH i.e Mbuffer is added

MbufferVbuffer = Mbase Vbase

putting the values in above equation:

Mbuffer =

             =

             = 0.01 M

molarity or [ A-] = 5M

pH =   pKa+ log 10

pH = 4.200 + log 10

pH = 4.200+ 2.69

pH = 6.8

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