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AP chemistry

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1). In a titration 20 mL of 0.100 M of HCl is added to 50.0 mL of 0.150 M of ammonia.
A). What is the pH of NH3?

B). What is the pH of the resulting solution?

HELP :(

  • AP chemistry - ,

    1) Makes no sense to me. Is that before the HCl is added or after. If after it's the pH of the solution, not NH3.

    2)
    HCl + NH3 ==> NH4Cl
    mols HCl = M x L = 0.002
    mols NH3 = M x L = 0.0075.
    So you have how much NH3 that doesn't react? That's 0.0075 - 0.002 = 0.0055 mols NH3 excess. That's in how much volume? That's 50 mL + 20 mL = 70 mL = 0.07L so the excess NH3 concn is
    mols/L = 0.0055/0.07 = 0.786M.
    .......NH3 + H2O ==> NH4^+ + OH^-
    I.....0.0786..........0........0
    C......-x.............x........x
    E.....0.0786-x........x........x

    Substitute the E line into Kb expression for NH3 and solve for x = (OH^-), convert to pH.
    Round to the correct number of significant figures.

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