The discussion revolves around determining the proton concentration in a mixed solution involving sulfuric acid (H2SO4) and sodium hydroxide (NaOH). Participants explore the stoichiometry of the reactions, the effects of mixing these solutions, and the implications for calculating hydronium ion (H3O+) concentration. The conversation includes theoretical considerations, reaction equations, and equilibrium concepts.
Participants do not reach a consensus on the correct approach to calculate the proton concentration. There are multiple competing views regarding the stoichiometry of the reactions, the interpretation of equilibrium constants, and the calculations involved.
Limitations include unresolved assumptions about the initial concentrations and volumes, as well as the dependence on the definitions of formal and molar concentrations. The discussion also reflects varying levels of understanding of acid-base equilibria and stoichiometry.
This discussion may be useful for students and individuals interested in chemistry, particularly those studying acid-base reactions, stoichiometry, and equilibrium concepts.
(I did not solve it. I only wrote it.)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.
Study basic algebra: Algebra 1 and Algebra 2;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##