Since most acetic acid molecules do not dissociate when a sample is dissolved in water, acetic acid and water molecule interactions are what determine how soluble a substance is. In its liquid state, water forms a network of hydrogen bonds among its molecules; when a material dissolves in water, this network of hydrogen bonds is broken.
<h3>What is acetic acid such a poor electrolyte?</h3>
Since acetic acid is a weak acid, only a small portion of the acetic acid molecules react to produce ethanoate and hydronium ions, shifting the equilibrium position substantially to the left. Aqueous acetic acid is a weak electrolyte as a result of the existence of these few ions.
<h3>Why does acetic acid have a low conductivity?</h3>
The majority ($> 99%) of the acetic acid molecules remain after dissolution, with only a very tiny portion deprotonating to form acetate anions. Only the latter are charged compounds, and as a result, only these increase the conductivity of the solution. They are few, and conductivity is low.
<h3>What makes acetic acid more potent than water?</h3>
The equilibrium shifts to the left and the concentration of hydrogen ions decreases when a strong acid is added to the buffer solution. A strong base is also added, which causes the equilibrium to move to the left and results in a smaller pH increase. Because of this, acetic acid is a better buffer than water.
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