Chemistry

For the titration of 50.00mL of 0.1000 M ammonia with 0.1000 M HCl, calculate the pH
(a) before the addition of any HCl solution
(b) after 20.00mL of the acid has been added

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  1. At the beginning you have pure NH3 solution.
    ......NH3 + H2O ==> NH4^+ + OH-
    I.....0.1............0.......0
    C......-x............x.......x
    E.....0.1-x...........x......x

    Plug the E line into the Kb expression and solve for x = OH, then convert to pH.

    For part b. You started with how many mols of each.
    mols NH3 = M x L = ? about 0.005
    mols HCl = M x L = ? about 0.002
    So you have 0.003 M NH3 left no HCl in excess and you formed 0.002 mols NH4Cl.

    Use the Henderson-Hasselbalch equation for buffers and calculate the pH.
    pH = pKa + log (base)/(acid)

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  2. take it ez maaaan

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