Calculate the percent ionization of formic acid solutions having the following concentrations.

Asked by maham237 @ 27/12/2020 in Chemistry viewed by 370 People

Calculate the percent ionization of formic acid solutions having the following concentrations.a) 1.20Mb)0.450Mc)0.130Md)5.10 x 10^-2

Answered by maham237 @ 27/12/2020

Answer:

a) 1.224 %.

b) 2.0 %.

c) 3.7 %.

d) 5.94 %.

Explanation:

To solve this problem, we have the relation:

Ka = (α²C)/(1 - α),

where, Ka is the Dissociation Constant of the acid; C is the Concentration of the acidic solution; and α is the degree of dissociation of the acid.

Since, α is a very small value, (1 - α) ≅ 1.

∴ Ka = (α²C).

∴ α = √(Ka/C).

a) 1.20 M:

∵ α = √(Ka.C)

Ka of formic acid = 1.8 x 10⁻⁴, C = 1.2 M.

∴ α = √(Ka/C) = √(1.8 x 10⁻⁴)/(1.2) = 0.01224.

∴ The percent of ionization = α x 100 = 1.224 %.

b) 0.45 M:

∵ α = √(Ka.C)

Ka of formic acid = 1.8 x 10⁻⁴, C = 0.45 M.

∴ α = √(Ka/C) = √(1.8 x 10⁻⁴)/(0.45) = 0.02.

∴ The percent of ionization = α x 100 = 2.0 %.

c) 0.13 M:

∵ α = √(Ka.C)

Ka of formic acid = 1.8 x 10⁻⁴, C = 0.13 M.

∴ α = √(Ka/C) = √(1.8 x 10⁻⁴)/(0.13) = 0.037.

∴ The percent of ionization = α x 100 = 3.7 %.

d) 5.10 x 10⁻² M:

∵ α = √(Ka.C)

Ka of formic acid = 1.8 x 10⁻⁴, C = 5.10 x 10⁻² M.

∴ α = √(Ka/C) = √(1.8 x 10⁻⁴)/(5.10 x 10⁻²) = 0.0594.

∴ The percent of ionization = α x 100 = 5.94 %.

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