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Svet_ta [14]
3 years ago
15

A student prepares a 0.61mM aqueous solution of propionic acid C2H5CO2H. Calculate the fraction of propionic acid that is in the

dissociated form in his solution. Express your answer as a percentage. You will probably find some useful data in the ALEKS Data resource.
Chemistry
1 answer:
MAXImum [283]3 years ago
4 0

Answer:

The 13.76% of propionic acid is in the dissociated form in the solution

Explanation:

Concentration of propionic acid = c = 0.61mM = 0.61\times 10^{-3}M

mM=10^{-3}M

Degree of dissociation = α

C2H5CO2H\rightleftharpoons C2H5COO^-+H^+

At initial

c                             0   0

At equilibrium

c - cα                     cα   cα

The value of dissociation constant of propionic acid = K_a=1.34\times 10^{-5}

The expression of dissociation constant of propionic acid is given by :

K_a=\frac{c\times alpha c\times \alpha}{c(1-\alpha )}

K_a=\frac{c\alpha ^2}{(1-\alpha )}

1.34\times 10^{-5}=\frac{0.61\times 10^{-3}M\times \alpha ^2}{(1-\alpha )}

Solving the equation for \alpha:

\alpha =0.1376

\alpha=\frac{0.1376}{1}\times 100=13.76\%

The 13.76% of propionic acid is in the dissociated form in the solution

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