Question

In: Chemistry

Calculate the percent ionization of acetic acid solutions having the following concentrations. A. 1.20M B. 0.550...

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

A. 1.20M

B. 0.550

C. 0.100

D. 4.60*10^-2

Solutions

Expert Solution

A)

CH3COOH dissociates as:

CH3COOH -----> H+ + CH3COO-

1.2 0 0

1.2-x x x

Ka = [H+][CH3COO-]/[CH3COOH]

Ka = x*x/(c-x)

Assuming x can be ignored as compared to c

So, above expression becomes

Ka = x*x/(c)

so, x = sqrt (Ka*c)

x = sqrt ((1.8*10^-5)*1.2) = 4.648*10^-3

since c is much greater than x, our assumption is correct

so, x = 4.648*10^-3 M

% dissociation = (x*100)/c

= 4.648*10^-3*100/1.2

= 0.3873 %

Answer: 0.387 %

B)

CH3COOH dissociates as:

CH3COOH -----> H+ + CH3COO-

0.55 0 0

0.55-x x x

Ka = [H+][CH3COO-]/[CH3COOH]

Ka = x*x/(c-x)

Assuming x can be ignored as compared to c

So, above expression becomes

Ka = x*x/(c)

so, x = sqrt (Ka*c)

x = sqrt ((1.8*10^-5)*0.55) = 3.146*10^-3

since c is much greater than x, our assumption is correct

so, x = 3.146*10^-3 M

% dissociation = (x*100)/c

= 3.146*10^-3*100/0.55

= 0.5721 %

Answer: 0.572 %

C)

CH3COOH dissociates as:

CH3COOH -----> H+ + CH3COO-

0.1 0 0

0.1-x x x

Ka = [H+][CH3COO-]/[CH3COOH]

Ka = x*x/(c-x)

Assuming x can be ignored as compared to c

So, above expression becomes

Ka = x*x/(c)

so, x = sqrt (Ka*c)

x = sqrt ((1.8*10^-5)*0.1) = 1.342*10^-3

since x is comparable c, our assumption is not correct

we need to solve this using Quadratic equation

Ka = x*x/(c-x)

1.8*10^-5 = x^2/(0.1-x)

1.8*10^-6 - 1.8*10^-5 *x = x^2

x^2 + 1.8*10^-5 *x-1.8*10^-6 = 0

This is quadratic equation (ax^2+bx+c=0)

a = 1

b = 1.8*10^-5

c = -1.8*10^-6

Roots can be found by

x = {-b + sqrt(b^2-4*a*c)}/2a

x = {-b - sqrt(b^2-4*a*c)}/2a

b^2-4*a*c = 7.2*10^-6

roots are :

x = 1.333*10^-3 and x = -1.351*10^-3

since x can't be negative, the possible value of x is

x = 1.333*10^-3

% dissociation = (x*100)/c

= 1.333*10^-3*100/0.1

= 1.3327 %

Answer: 1.33 %

D)

CH3COOH dissociates as:

CH3COOH -----> H+ + CH3COO-

4.6*10^-2 0 0

4.6*10^-2-x x x

Ka = [H+][CH3COO-]/[CH3COOH]

Ka = x*x/(c-x)

Assuming x can be ignored as compared to c

So, above expression becomes

Ka = x*x/(c)

so, x = sqrt (Ka*c)

x = sqrt ((1.8*10^-5)*4.6*10^-2) = 9.099*10^-4

since x is comparable c, our assumption is not correct

we need to solve this using Quadratic equation

Ka = x*x/(c-x)

1.8*10^-5 = x^2/(4.6*10^-2-x)

8.28*10^-7 - 1.8*10^-5 *x = x^2

x^2 + 1.8*10^-5 *x-8.28*10^-7 = 0

This is quadratic equation (ax^2+bx+c=0)

a = 1

b = 1.8*10^-5

c = -8.28*10^-7

Roots can be found by

x = {-b + sqrt(b^2-4*a*c)}/2a

x = {-b - sqrt(b^2-4*a*c)}/2a

b^2-4*a*c = 3.312*10^-6

roots are :

x = 9.01*10^-4 and x = -9.19*10^-4

since x can't be negative, the possible value of x is

x = 9.01*10^-4

% dissociation = (x*100)/c

= 9.01*10^-4*100/0.046

= 1.9587 %

Answer: 1.96 %


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