Titration of strong acid with weak base

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The discussion focuses on a titration problem involving a strong acid and a weak base, specifically using the Henderson-Hasselbalch equation. The user presents their calculations, indicating a concentration of 0.0181 M for HCl, but receives feedback that their solution is incorrect. The importance of clearly showing work for effective assistance is emphasized, as well as the complexity of the problem requiring multiple equations and algebraic steps. The user believes they have identified the solution but acknowledges the forum's rules against providing direct answers. Clarity in problem-solving steps is crucial for receiving helpful feedback in chemistry discussions.
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Please post readable solutions to your problems, not shaky images impossible to read.

Homework Statement


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Homework Equations


Henderson-Hasselbalch Equation

The Attempt at a Solution


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Sorry for the huge picture, but the number says 0.007558 mol. Is my ICE table correct?
Equation:
7.42 = 6.85 + log((0.007558-x)/x)
(0.007558-x)/x = 3.715
x = 0.00160 mol H+/(0.07483 L + 0.01339 L) = 0.0181 M = [HCl]
It says it is incorrect, though.
 
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This one is not difficult, but still requires a couple of equations and several algebraic steps. You do need to show the work more clearly for the helper to be able to give good feedback. I think I figured out the solution, but the Physics Forum rules do not allow the helper to simply furnish the solution.
 

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