In a 1.0× 10–4 M solution of HClO(aq), identify the relative molar amounts of these species. (most to least)
H2O
HClO
H3O
OH-
OCl-
Is that how you have them arranged? How did you arrive at that sequence?
To determine the relative molar amounts of the species in a 1.0× 10–4 M solution of HClO(aq) - H2O, HClO, H3O, OH-, and OCl-, we need to understand the ionization of HClO in water. HClO is a weak acid that partially dissociates in aqueous solution.
The ionization equation for HClO is as follows:
HClO(aq) ⇌ H+(aq) + ClO-(aq)
In this equation, HClO dissociates to form H+ (hydronium ion) and ClO- (hypochlorite ion).
Since HClO is a weak acid, it does not dissociate completely. Instead, it establishes an equilibrium between the unionized form and the dissociated form. The concentration of HClO in the solution is given as 1.0× 10–4 M, so we can assume that the concentrations of H+ and ClO- are negligible compared to the initial concentration of HClO.
Now, to determine the relative molar amounts of the species, we need to consider the concentration of each species present after the ionization. Since the concentrations of H+ and ClO- are negligible, the main species present are H2O, HClO, and H3O+ (hydronium ion).
So, here is the order of the relative molar amounts from most to least:
1. HClO - since it is only partially dissociated and the initial concentration is given as 1.0× 10–4 M.
2. H2O - it is the solvent and is present in high excess, so its concentration is much higher than the concentration of HClO or H3O+.
3. H3O+ - it is formed as a result of the partial ionization of HClO and is present in lesser amounts compared to H2O.
As for OH- and OCl-, we don't expect significant amounts of these species to be present in an acid solution of HClO.
It is important to note that the relative molar amounts depend on the specific conditions and concentration of the solution. The explanation provided here assumes ideal conditions and a given concentration of HClO.