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Chemistry

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Consider the titration of 50.0 mL of 0.20 M NH3 (Kb = 1.8x10^-5) with 0.20 M HNO3. Calculate the pH after addition of 50.0 mL of the titrant.

  • Chemistry - ,

    The secret to doing titration problems is to recognize what you have in the solution. In this case, the NH3 is exactly neutralized by the HNO3; therefore, you are at the equivalence point and you have NH4NO3 is solution. How much NH4NO3? That will be 50.0 mL x 0.20 M = 10 millimoles in 100 mL = 0.1 M

    Write the hydrolysis equation.
    NH4^+ + HOH ==> NH3 + H3O^+
    Then do the ICE bit.
    Ka = Kw/Kb = (NH3)(H3O^+)/(NH4^+
    Solve for (H3O^+) and convert to pH.

  • Chemistry - ,

    5.13

  • Chemistry - ,

    8.5

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