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A buffer solution contains 0.227 M ammonium bromide and 0.427 M ammonia. If 0.0488 moles of...

A buffer solution contains 0.227 M ammonium bromide and 0.427 M ammonia.

If 0.0488 moles of nitric acid are added to 225 mL of this buffer, what is the pH of the resulting solution?
(Assume that the volume does not change upon adding nitric acid.)

pH =

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Expert Solution

no of moles of NH4Br   = molarity * volume in L

                                      = 0.227*0.225   = 0.051 moles

no of moles of NH3       = molarity * volume in L

                                       = 0.427*0.225   = 0.096 moles

0.0488 moles of HNO3 is added

no of moles of NH4Br after addition of HNO3 = 0.051+0.0488   = 0.0998 moles

no of moles of NH3 after addition of HNO3     = 0.096-0.0488    = 0.0472 moles

POH   = Pkb + log[NH4Br]/[NH3]

           = 4.75 + log0.0998/0.0472

          = 4.75+0.325   = 5.075

PH    = 14-POH

        = 14-5.075    = 8.925 >>>>>answer

queen_honey_blossom answered 2 years ago
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