SAT, 24.11.2021 08:30 QueenMiah16

Determine the percent ionization of the following solutions of formic acid at 25°c:.

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The percent ionization of formic acid solutions having the concentrations of 1.20, 0.450, 0.130, and 5.10x10⁻² M is 1.22, 1.98, 3.61, and 5.69%, respectively.

The reaction of dissociation of formic acid is the following.

CHOOH + H₂O ⇄ CHOO⁻ + H₃O⁺

In the equilibrium we have:

CHOOH + H₂O ⇄ CHOO⁻ + H₃O⁺ (1)

Ci - x x x

(2)

Where:

Kc: is the equilibrium constant of formic acid = 1.8x10⁻⁴

Ci: is the initial concentration of formic acid

The percent ionization of formic acid can be calculated with the following equation:

(3)

With the above information, we can find the percent ionization of formic acid of each different concentration.

a) Ci = 1.20 M

We can find the H₃O⁺ concentration with equation (2)

After solving the above quadratic equation for x, we have:

Taking the positive value (x₁) we can find the percent ionization (eq 3)

Hence, the percent ionization of formic acid is 1.22% when the initial concentration is 1.20 M.

b) Ci = 0.450 M

From equation (2) we have:

After solving the above quadratic equation for x, we have:

With the positive value we can find the percent ionization (eq 3)

Therefore, the percent ionization of formic acid is 1.98% when the initial concentration is 0.450 M.

c) Ci = 0.130 M

From eq (2) we have:

After solving the above quadratic equation for x:

The percent ionization is (eq 3):

Then, the percent ionization of formic acid is 3.61% when the initial concentration is 0.130 M.

d) Ci = 5.10x10⁻² M

The H₃O⁺ concentration is:

So, the percent ionization is (eq 3):

The percent ionization of formic acid is 5.69% when the initial concentration is 5.10x10⁻² M.

Therefore, the percent ionization of formic acid solutions for the concentrations 1.20, 0.450, 0.130, and 5.10x10⁻² M is 1.22, 1.98, 3.61, and 5.69%, respectively.

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