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Rank the solutions in order of decreasing [H30+].
Rank solutions from largest to smallest hydronium ion concentration. To rank items as equivalent, overlap them.
0.10 M HC2H3O2 0.10 M HCN 0.10 M HBr 0.10 M HClO2
♦ Relevant knowledge
The Bronsted acid species that dissociates in a reverse manner at minimum the covalent “H-X” bonds in an aqueous solution. If the proton that is released is then transferred into water, the hydronium ion and conjugate base products are created. The equilibrium state of reaction is represented by the acid dissociation constant, Ka. This kind of equilibrium constant connects to different constant molarity values for aqueous solutions. The size of its value is directly linked with the power of acidic substances that is, how effective it is in increasing the hydronium Ion molecularity.
This is why we need Ka values to deal with weak acids.
HBr is the strongest acid among all of the acids. So [H 3O +] is the highest of all four.
Ka for HC2H3O2 = 1.8 × 10 -5
Ka for HCN = 6.22 × 10 10
Ka for HClO = 1.1 × 10 -2
Ka is the acid-dissociation constant for a weak acid. The Ka value is a measure of acid strength. Therefore, the conc. H3O+
Therefore, Hydronium ion concentrations are ordered
0.1 M HBr > 0.1 M HClO2 > 0.1 M HC2H3O2 > 0.1 M HCN