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A solution is prepared by adding 300 mL of 0.500 M NH3 and 100 mL of 0.500 M HCl. Assuming that the volumes are additive, what is the pH of the resulting mixture? Kb for ammonia is 1.8 x10 -5

  • Chemistry -

    You've added a base to an acid; which one is in excess. The equation is
    NH3 + HCl ==> NH4Cl
    mmoles NH3 = 300 mL x 0.500 M = 150
    mmoles HCl = 100 mL x 0.500 M = 50

    It should be obvious that the reaction produces 50 mmoles NH4Cl, all of the HCl is used and there are 100 mmoles NH3 remaining unreacted. This is a solution of a weak base (NH3) and its salt (NH4Cl) and that is a buffered solution. So use the Henderson-Hasselbalch equation.
    pH = pKa + log [(base)/(acid))]
    Post your work if you get stuck.

  • Chemistry -


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