What is the pH after adding a base?

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The discussion revolves around calculating the pH of a solution after titrating a nitrous acid solution with barium hydroxide. The initial moles of nitrous acid and barium hydroxide are provided, with the user expressing confusion about how to proceed after determining these values. Key points include the importance of assuming complete neutralization and using the Henderson-Hasselbalch equation to find the concentrations of the remaining acid and the produced conjugate base. The conversation emphasizes the need to treat this as a limiting reagent problem, where the final concentrations can be calculated based on the amounts of acid and base used, along with the final volume of the solution. Additionally, it highlights the relevance of molarity in determining concentrations and suggests using calculators for pH and stoichiometry to aid in the calculations.
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This is my question:
When a 17.9 mL sample of a 0.493 M aqueous nitrous acid solution is titrated with a 0.476 M aqueous barium hydroxide solution, what is the pH after 13.9 mL of barium hydroxide have been added?
I'm not really sure how to start it?
I have the moles of the acids and the base.
[acid]=8.8247E-3
[base]=6.6164E-3
but after that I'm lost! Help would be greatly appreciated!
 
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Classic buffer question. Assume neutralization went to completion, calculate concentrations of acid and conjugate base, use Henderson-Hasselbalch equation.

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Stoichiometry. You start with some amount of nitrous acid. You add some base. If neutralization went to completion, you are able to easily calculate amount of the acid left, and amount of conjugate base (product of the reaction) - this is just a limiting reagent question. You know amounts, you know the final volume - just plug and chug.

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methods
 
The molarity of your acid/base is given. Molarity = Moles/Liter IS your concentration.
 
Note: in case base is in excess all acid was neutralized, and it is just a limiting reagent question.

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