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Part A Calculate the pH of a solution that is 0.060 M in potassium propionate (C2...

Question

Part A Calculate the pH of a solution that is 0.060 M in potassium propionate (C2...

Part A Calculate the pH of a solution that is 0.060 M in potassium propionate (C2 H5 COOK or KC3 H5 O2) and 0.080 Min propionPart B Calculate the pH of a solution that is 0.080 M in trimethylamine, (CH3)3N, and 0.11 Min trimethylammonium chloride, ((

Part C Calculate the pH of a solution that is made by mixing 50.0 mL of 0.16 Macetic acid and 50.0 mL of 0.20 M sodium acetat

Part A Calculate the pH of a solution that is 0.060 M in potassium propionate (C2 H5 COOK or KC3 H5 O2) and 0.080 Min propionic acid (С2 Hs СООН or HC3H$ O2). Express your answer to two decimal places ΑΣφ pH Request Answer Submit
Part B Calculate the pH of a solution that is 0.080 M in trimethylamine, (CH3)3N, and 0.11 Min trimethylammonium chloride, ((CH3)3NHCI) Express your answer to two decimal places. ΑΣφ pH Request Answer Submit t
Part C Calculate the pH of a solution that is made by mixing 50.0 mL of 0.16 Macetic acid and 50.0 mL of 0.20 M sodium acetate. Express your answer to two decimal places. ΑΣφ pH

Answers

Part A)

[propionate] = 0.060M

[acid] = 0.080M

pKa of propionic acid = 4.88

The solution is a buffer and its pH is calculated using Hendersen equation as

pH = pKa + log [ conjugate base]/[acid]

= 4.88+ log 0.060/0.080

= 4.755

Part B

this is a base and conjugate acid buffer

[methylamine] = 0.080 M

[ salt] = 0.11 m and

pKb of methylamine = 4.19

The pOH of this buffer by Hendersen equation is

pH = pKb + log [salt]/[base]

= 4.19 + log 0.11/0.08

= 4.328

and pH = 14-pOH= 14- 4.328 =9.6717

Part C

[acetate] = 0.160M

[acid] = 0.20M

pKa of acetic acid = 4.75

The solution is a buffer and its pH is calculated using Hendersen equation as

pH = pKa + log [ conjugate base]/[acid]

= 4.75+ log 0.160/0.20

= 4.653


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