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So I don't know how to calculate the pH after .010 mol gaseous HCl is added to 250.0 mL of a buffered solution of .050 M NH3/.15 M of NH4Cl.
Can someone explain how to do this?
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I would really love to answer that question, and I actually know how to now! But I just spent about 30 minutes writing it out on here to post for you and my computer randomly cleared it!!!! grrr...well, if you want some help PM me,K?
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If you still need help with this problem then the answer is:
First write this equation (NH3 + H+ ---> NH4) then under each reactant and product write the number or moles that are initially present. Next, assume H+ is the limiting reactant and subtract its moles from the reactant side and add it to the product side. Then recalulate the molarity of NH3 and NH4. After that use this equation (NH3 + H2O ----> NH4 + OH-) and write in the molarity and solve for the pH using the ICE chart or the Henderson-Hasselbalch equation.
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