chemistry

A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. Determine the pH of the solution before
the addition of any KOH. The Kb of NH3 is 1.8 × 10-5.
I thought that I would need a second volume to find the moles of NH3?

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asked by Sydney
  1. Something is wrong with the post. You're titrating NH3 with HNO3 but you want the pH before any KOH is added. Where did the KOH come from? I assume you want the pH of a solution of 0.1M NH3.
    At the beginning, before any HNO3 has been added
    ...........NH3 + HOH ==> NH4^+ + OH^-
    I..........0.1............0.......0
    C...........-x............x.......x
    E..........0.1-x..........x.......x

    Substitute the E line into the Kb expression and solve for x = (OH^-), then convert that to pH.

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    posted by DrBob222

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