Solving Equilibrium Question: Calculate Acetate Ion Concentration

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SUMMARY

The discussion focuses on calculating the acetate ion concentration in a solution containing 1.00×10-3 mol of HCl dissolved in 1.00 L of 1.90 M acetic acid, with a dissociation constant (Ka) of 1.7E-5. The initial concentrations of acetic acid (CH3COOH) and the changes due to dissociation are outlined, leading to an equilibrium expression. The participant initially calculated x as 5.68E-3 but failed to incorporate the fully dissociated HCl into their calculations, which is crucial for determining the correct acetate ion concentration.

PREREQUISITES
  • Understanding of acid-base chemistry and dissociation reactions
  • Familiarity with equilibrium expressions and the ICE (Initial, Change, Equilibrium) table method
  • Knowledge of the dissociation constant (Ka) and its application in calculations
  • Basic skills in algebra for solving equations
NEXT STEPS
  • Review the concept of acid-base equilibrium and how to set up ICE tables
  • Learn how to incorporate strong acids like HCl into equilibrium calculations
  • Study the relationship between pH, pKa, and concentration of ions in solution
  • Practice similar problems involving weak acids and their conjugate bases
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Chemistry students, educators, and anyone involved in analytical chemistry or acid-base equilibrium calculations will benefit from this discussion.

Jules18
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Hey guys, I've tried this question a couple different ways. Please help!

Homework Statement



Calculate the concentration of the acetate ion (M) in a solution prepared by dissolving 1.00×10-3 mol of HCl(g) in 1.00 L of 1.90 M aqueous acetic acid. Ka = 1.7E-5

And at that point I'm not sure what to do.


Homework Equations



... CH3COOH --> CH3COO- + H+
initial: 1.90 M 0 0
change: - x +x +x
equlbm: ~1.9 x x

The Attempt at a Solution



I did some calculations and found that x = 5.68E-3 . I that didn't take the HCl into consideration, though - I really have no idea what to do with that. i
 
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As you were already told at CF - concentration of H+ should account for the HCl. It is fully dissociated.

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