# 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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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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