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    The Kstab for this reaction is 1.70*10^7 mol^-4 dm^12
    [Ag(H2O)6]+ + 2NH3 ---> [Ag(NH3)2(H2O)4]+ + 2H2O

    Given the concentrations of the reactions used were
    [Ag(H2O)6]+ = 5*10^-3 mol dm^-3
    [NH3] = 2.5*10^-3 mol dm ^-3

    Calculate the conc. of the complex ion, [Ag(NH3)2(H2O)4]+.

    My answer = 0.531mol dm^-3

    If that is not correct, can you explain please? Thank you.
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    (Original post by ILoveUSA)
    The Kstab for this reaction is 1.70*10^7 mol^-4 dm^12
    [Ag(H2O)6]+ + 2NH3 ---> [Ag(NH3)2(H2O)4]+ + 2H2O

    Given the concentrations of the reactions used were
    [Ag(H2O)6]+ = 5*10^-3 mol dm^-3
    [NH3] = 2.5*10^-3 mol dm ^-3

    Calculate the conc. of the complex ion, [Ag(NH3)2(H2O)4]+.

    My answer = 0.531mol dm^-3

    If that is not correct, can you explain please? Thank you.
    Don't you want to try showing your method?

    I'm assuming the two concentrations you've listed are initial concentrations. If so then you should come out with an answer of 0.005 moldm-3. At least that's what I got. This comes from working out the change in concentration for your original complex ion.
 
 
 
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