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Consider the titration of a 25.0?mL sample of 0.175M CH3NH2 with 0.145M HBr. Determine each of...

Consider the titration of a 25.0?mL sample of 0.175M CH3NH2 with 0.145M HBr. Determine each of the following.

the pH at 6.0mL of added acid

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Answer #1

chemical equation :
                            CH3NH2        +      HBr   -------------- >       CH3NH3Br
   Before rxn     0.025 L *0.175 M   0.145 M * 0.006L                         0
                          = 0.004375 mols         =0.00087 mols
   Afterrxn        0.004375 mols -0.00087 mols      0                        0.00087mols
                                            = 0.003505 mols
                                            = 0.003505 mols /( 0.025 + 0.005 ) L
                                      C   = 0.116 M
                               
CH3NH2   is a weakbase with Kb = 4.38*10 ^ - 4 .
                                         [OH-]      = ? Kb * C
                                                        = ? 4.38*10 ^ - 4 . * 0.116 M
                                                        = 0.7127 * 10 ^ -2 M
                                                pOH = - log ( 0.7127 * 10 ^ -2 )
                                                         = 2.14
                                                pH    = 14 - 2.14
                                                         = 11. 85 ==>11.9

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