Select the correct relationship among the concentrations of species present in a 1.0 M aqueous solution of the weak acid represented by HA. Multiple Choice [H2O] > [A–] ~ [H3O+] > [HA] > [OH–] [H2O] > [HA] > [A–] > [H3O+] > [OH–] [HA] > [H2O] > [A–] > [H3O+] > [OH–] [H2O] > [HA] > [A–] ~ [H3O+] > [OH–] [HA] > [H2O] > [A–] ~ [H3O+] > [OH–]

As we know, in solution solute is present in smaller amount than solvent.So the concentration of water will be maximum followed by undissociated weak acid.

[tex][H_2O] > [HA][/tex]

Since, HA is a weak acid it will not completely dissociate in water but dissociation will take place in less extend. And on dissociation Hydronium ion and [tex]A^-[/tex] ions will be produced.

[tex][HA] > [A^-] \sim [H_3O^+][/tex]

And remaining concentration of hydroxide ions will be very small.

The order of ions from maximum concentration to minimum concentration is:

[tex][H_2O] > [HA] > [A^-] \sim [H_3O^+] > [OH^-][/tex]

pstnonsonjoku pstnonsonjoku · Answer 2 · 2022-04-12T14:20:34+02:00

The species present in their relative proportions are [H2O] > [HA] > [A–] ~ [H3O+] > [OH–].

What is a weak acid?

A weak acid is an acid that is not completely dissociated in solution. In other words, there are more undissociated acid molecules than there are the ions that compose the acid.

For a 1.0 M aqueous solution of the weak acid represented by HA, the species present in their relative proportions are [H2O] > [HA] > [A–] ~ [H3O+] > [OH–].

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