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Write an equilibrium reaction for a buffer system made of the weak base, B, and its conjugate acid. If the buffer contains 1.05 M of B and 0.750M conjugate acid and has a pH of 9.50, what is the pH after 0.0050 mol HCl is added to 0.500 L of this solution?

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    B + H^+ ==> BH^+

    In 500 mL of the buffer we have millimols of
    B = 500 x 1.05 = 525
    BH^+ = 500 x 0.750 = 375
    add 0.005 = 5 millimols HCl.

    ...........B + H^+ ==> BH^+
    initial...525.........375
    add............5..............
    change.....-5...-5....5
    equil.....520.....0....380

    Plug into the Henderson-Hasselbalch equation and solve for pH.

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