How to Determine Proton Concentration in a Mixed Solution?

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SUMMARY

The discussion focuses on determining the proton concentration in a mixed solution involving sulfuric acid (H2SO4) and sodium hydroxide (NaOH). Participants clarify that the molarity of hydronium ions (H3O+) is derived from the dissociation of bisulfate ions (HSO4-) after the reaction. The equilibrium constant (Ka) for HSO4- is noted as 1.02 x 10^-2, which is essential for calculating the concentration of H3O+. The final consensus indicates that the formal concentration of HSO4- is 0.5 M, but the actual molarity of H3O+ must account for dissociation.

PREREQUISITES
  • Understanding of acid-base reactions, specifically H2SO4 and NaOH interactions.
  • Knowledge of molarity and formal concentration concepts.
  • Familiarity with equilibrium constants and their applications in weak acid dissociation.
  • Basic algebra skills for solving quadratic equations.
NEXT STEPS
  • Study the dissociation of weak acids, focusing on HSO4- and its equilibrium constant.
  • Learn how to derive and solve quadratic equations in the context of chemical equilibria.
  • Explore the concept of formality versus molarity in chemical solutions.
  • Review stoichiometry principles related to acid-base neutralization reactions.
USEFUL FOR

Chemistry students, educators, and professionals involved in analytical chemistry, particularly those focusing on acid-base equilibria and solution chemistry.

  • #31
mjc123 said:
x is the concentration of H3O+, which is equal to the concentration of SO42-. 0.5-x is the concentration of HSO4-. We ignore the concentration of water as it is effectively constant.
Your solution to the quadratic equation is incorrect.
(I did not solve it. I only wrote it.)
 
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  • #32
Lifeforbetter said:
I don't know where this come from.. 0.5 - x and x refers to what concentration..
But i calculate
x = 0.01 +- 0.05##\sqrt2##
Study basic algebra: Algebra 1 and Algebra 2;
then study Elementary Chemistry, and the first or the first AND second semesters of General Chemistry; only then may you understand these topics.
 

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