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Calculate the [H3O+] concentration (in M) in a 0.1 M aqueous solution of NH3

  1. Jun 14, 2009 #1
    1. The problem statement, all variables and given/known data
    Calculate the [H3O+] concentration (in M) in a 0.1 M aqueous solution of NH3.
    [Kb = 1.8 x 10–5 ]
    (a) 7.5 x 10–12 M (c) 1.8 x 10–6 M
    (b) 3.0 x 10–10 M (d) 1.3 x 10–3 M


    2. Relevant equations
    ΔTb = Kb x m


    3. The attempt at a solution
    So... I'm kind of at a loss here. First of all to do anything useful with the ΔTb = Kb x m equation, they would have to give ΔTb right? And also, because its an aqueous solution, I assume we are dissolving NH3 into water. The Kb of water is 0.512.... why then do they give a Kb value of 1.8 x 10–5?

    Thanks in advance :smile: The answer is a, btw, but why!?
     
  2. jcsd
  3. Jun 15, 2009 #2

    Borek

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    Staff: Mentor

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