Calculate the pH and percent dissociation of a 0.05 M Acetic...

Name: Calculate the pH and percent dissociation of a 0.05 M Acetic acid solution and a 0.005 M Acetic Acid Solution (Acetic Acid: Ka = 1.8 x 10-5)? In comparing the percent dissociation of the two solutions what is the observed trend?
Uploaded: 2022-01-26T10:29:16-08:00
Duration: 6 min 23 s
Channel: Ishu S
Description: Calculate the pH and percent dissociation of a 0.05 M Acetic acid solution and a 0.005 M Acetic Acid Solution (Acetic Acid: Ka = 1.8 x 10-5)? In comparing the percent dissociation of the two solutions what is the observed trend?

Calculate the pH and percent dissociation of a 0.05 M Acetic acid solution and a 0.005 M Acetic Acid Solution (Acetic Acid: Ka = 1.8 x 10-5)? In comparing the percent dissociation of the two solutions what is the observed trend?

Transcript

00:01 In this question, we have to find out the ph as well as percentage dissociation of acetic acid at two different concentration.

00:10 First, concentration of acetic acid given to us is equal to 0 .05 molar and the another concentration which is given to us is equal to 0 .005 molar.

00:26 While the value of k -a, that is dissociation constant, given is 1 .8, multiply by 10 raised to per minus 5.

00:35 Let's consider the dissociation of acetic acid, which is this form, ch3 -coh, as weak acid will dissociate partially to give cs3 -c -o -negative ion as well as h -positive ion.

00:49 Initially, concentration c of cs3 -coh is present, while acetate iron and h -positive iron.

00:56 Iron are not present, then x concentration of ch3 coh is used while x of ch3 coo negative iron as well as h positive ion is produced.

01:08 Atically, viram, the concentration of cs3 coh would be c minus x, while that of ch3co negative is x and h positive iron concentration will also be x.

01:20 We have created ice table in this case.

01:23 Since ch3ch is very weak acid, it will dissociate very less, giving the value of x very small.

01:31 So it would be approximately equal to, so this value, c minus x, since x is very less, it will approximately equal to c.

01:39 From this we can calculate the dissociation constant, that is ka for this reaction, which is equal to concentration of acetic acid, multiply by, concentration of acetate ion, multiply by concentration of h positive ion divided by concentration of acetic acid, that is c.

01:58 From this we can say that x, that is concentration of h positive iron, also the concentration of cs3 -co negative iron, is equal to under root kc.

02:13 From this we can say the concentration of h -positive iron would be equal to under root k -a multiply by c.

02:21 Now we will use this equation in both cases and putting the value of c.

02:27 Now for cs3 -c -o -h, it would be equal to x is equal to under root ka, which is 1 .8, multiply by 10 raised to per minus 5, multiply by 0 .05.

02:43 After solving this, we will get the value of h -positive iron concentration, which is equal to 8...

Question

Calculate the pH and percent dissociation of a 0.05 M Acetic acid solution and a 0.005 M Acetic Acid Solution (Acetic Acid: Ka = 1.8 x 10-5)? In comparing the percent dissociation of the two solutions what is the observed trend?

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