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WILL GIVE BRAINLIEST! Why does the percent ionization increase when the concentration of a weak acid decreases? How does Le Chatelier's Principle explain this?

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As you add more acid to the solution the amount of dissociation increases to compensate for it. But since the acid is weak, it will never have more ions dissociate than are in the concentrated solution being added. % ionization is the concentration of dissociated H+ ions divided by the initial concentration of the weak acid. 

% ionization = [H+] / [weak acid] x 100% 

As you increase the concentration of the weak acid, the numerator increases more than the denominator so the percentage goes down.

The percent ionization increases when the concentration of a weak acid because the ratio of the equilibrium concentration or ionized concentration to the initial concentration, multiplied by 100%.

What is Percent Ionization ?

Percent ionization is used measure the quantity of number of ions which is present in the weak acid dissolved in a solution.

Percent Ionization = [tex]\frac{\text{Ionized acid concentration}}{\text{Initial concentration of acid}}} \times 100[/tex]

The percent ionization increases when the concentration of a weak acid decreases because the ratio of the equilibrium concentration or ionized concentration to the initial concentration, multiplied by 100%.

How does Le Principle explain this?

This principle predict the behavior of a system in equilibrium under different conditions. As the concentration of water increases the acid will get much more diluted this leads to decrease in the concentration of acid.

Thus, from above conclusion we can say that The percent ionization increases when the concentration of a weak acid because the ratio of the equilibrium concentration or ionized concentration to the initial concentration, multiplied by 100%.

Learn more about Percent ionization here: https://brainly.com/question/9080321
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