WHAT ARE THE MAJOR SPECIES PRESENT IN A AQUEOUS SOLUTION OF 1.0M CH3C00H?

I) CH3COOH
II) H20
III) H30+
IV) CH3COO-
VI) OH-

all of the above. Of course, one wonders what "Major" means. In a 1M solution, the major species will be water.

1M= is about 60 grams acid in almost 1000 grams solution, or about six percent, meaning 94 percent of the solution is water.

H2O

In an aqueous solution of 1.0M CH3COOH, the major species present are:

I) CH3COOH (acetic acid): This is the main component of the solution.

II) H2O (water): Water is the solvent in the solution.

III) H3O+ (hydronium ion): Acetic acid donates a proton to water, leading to the presence of hydronium ions in the solution.

IV) CH3COO- (acetate ion): Acetic acid also ionizes to some extent, producing acetate ions.

VI) OH- (hydroxide ion): Although not specifically mentioned, hydroxide ions can exist in aqueous solutions due to the autoprotolysis of water.

To determine the major species present in an aqueous solution of 1.0M CH3COOH, we need to consider its dissociation in water. CH3COOH is a weak acid that partially ionizes in water. The dissociation reaction for CH3COOH is as follows:

CH3COOH + H2O ⇌ CH3COO- + H3O+

The major species present in the solution can be identified based on the extent of ionization. Let's break down each species:

I) CH3COOH: This is the molecular form of acetic acid present in the solution.

II) H2O: Water is always present in an aqueous solution.

III) H3O+: This is the hydronium ion, which is formed when CH3COOH donates a proton to water. It represents the acidic properties of acetic acid.

IV) CH3COO-: This is the acetate ion, derived from the dissociation of acetic acid. It represents the basic properties of acetic acid.

VI) OH-: Hydroxide ions are not produced directly by the dissociation of CH3COOH, so OH- is not a major species in this case.

Therefore, the major species present in an aqueous solution of 1.0M CH3COOH are: I) CH3COOH, II) H2O, III) H3O+, and IV) CH3COO-.