Titration of strong acid with weak base

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SUMMARY

The discussion focuses on the titration of a strong acid with a weak base, specifically using the Henderson-Hasselbalch Equation to determine the concentration of HCl. The user calculated 0.00160 mol of H+ resulting in a concentration of 0.0181 M, but received feedback indicating the solution was incorrect. The conversation emphasizes the importance of clearly presenting the work involved in the calculations to facilitate effective assistance from peers.

PREREQUISITES
  • Understanding of the Henderson-Hasselbalch Equation
  • Knowledge of ICE (Initial, Change, Equilibrium) tables
  • Basic algebra skills for solving equations
  • Familiarity with acid-base titration concepts
NEXT STEPS
  • Review the Henderson-Hasselbalch Equation applications in titration scenarios
  • Practice constructing and interpreting ICE tables for various acid-base reactions
  • Explore common mistakes in titration calculations and how to avoid them
  • Study the properties of strong acids and weak bases in titration contexts
USEFUL FOR

Chemistry students, educators, and anyone involved in laboratory work related to acid-base titrations will benefit from this discussion.

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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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