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a) Calculate the pH of a solution 0.145M with respect to CH3CH2COOH and 0.115M with respect to K+CH3CH2COO-. Ka=1.3*10-5; pKa=4.89b) Calculate the pH of the same solution after adding 0.015M KOHc) Calculate the pH of the same solutions as in part (a) but after addition of 0.015M HBr

Question

a) Calculate the pH of a solution 0.145M with respect to CH3CH2COOH and 0.115M with respect to K+CH3CH2COO-. Ka=1.3*10-5; pKa=4.89

b) Calculate the pH of the same solution after adding 0.015M KOH

c) Calculate the pH of the same solutions as in part (a) but after addition of 0.015M HBr

check_circleAnswer
Step 1

Thankyou for posting your question but I am doing only (a) subpart because it seems that (b) and (c) subpart are incomplete as volume of added base and acid are required to solve these subparts. Kindly resubmit (b) and (c) subparts with complete information.

Step 2

Buffer solution:

A solution which can resist its pH when small amount of acid and base is added to it.

It is a solution consist of weak acid/weak base and its conjugate base/conjugate acid.

Here we have,

CH3CH2COOH= weak acid

CH3CH2COOK = salt.

Thus, above solution is a buffer solution.

Step 3

According to question:

pKa of CH3CH2COOH = 4.89.

Concentration of CH3CH2COOH = 0.145M

Concentration...

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