Consider that you have two solutions of acetic acid, ka = 1.8x10-5, one solution that is 1.59 m and another solution that is 0.186 m. compare the percent dissociation of acetic acid in these two solutions. what is the ratio of percent dissociation of the 1.59 m solution to the 0.186 m solution? (% dissociation of 1.59 m / % dissociation of 0.186 m) enter your answer numerically to three significant figures.

The ratio of percent dissociation of the 1.59 M solution to the 0.186 M solution: 0.343 : 1.

Explanation:

Initially c  

At equilibrium c-cα  cα cα

Dissociation constant of an acetic acid:

Degree of dissociation = α

Dissociation constant of an acid is given by:

1) Concentration of acid = c = [HAc] = 1.59 M

Degree of dissociation = α

Percentage of dissociation = 0.3359%

2) Concentration of acid = c' = [HAc] = 0.186 M

Degree of dissociation = α'

Percentage of dissociation = 0.9789%

The ratio of percent dissociation of the 1.59 M solution to the 0.186 M solution:

sure what is it? ^w^

they are both synthetic elements

explanation:

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