PH of a mixed solution: is this right?

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The discussion focuses on calculating the final pH of a solution created by mixing 200 ml of 0.400 M NH3 with 300 ml of 0.100 M HCl. The initial calculation using an ICE table resulted in a pH of 9.68, prompting questions about the correctness of this approach. Participants suggest that using two ICE tables may be necessary to account for the reactions in both directions, depending on which component is in excess. The hint provided indicates that if HCl is in excess, the pH can be calculated directly using the pH equation, while if NH3 is in excess, the Kb equation should be applied. The discussion emphasizes the importance of correctly identifying the limiting reactant to determine the final pH accurately.
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Homework Statement



What is the final pH of a solution obtained by mixing 200 ml of 0.400 M NH3 with 300 ml of 0.100 M HCl? (Kb = 1.8 x 10^-5)

Homework Equations



The Attempt at a Solution



I used an ICE table and came up with 9.68. Is that correct?

Should I have used two ICE tables instead of one? The first in the one direction and the second going back in the other direction?
 
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hint: the first reactions is that with NH3 and HCl, if you have excess HCl, then you can simply use the pH equation (pH= -log[H3O+]) to find the resulting pH, if the base is the excess, then the Kb equation is going to be used to determine the [OH-] concentration, and eventually the pH.
 
Thank you.
 
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