Use information from Appendix D in the textbook to calculate the pH of the follo

Question

Use information from Appendix D in the textbook to calculate the pH of the following solutions. A solution that is 6.5 times 10^-2 M in potassium propionate (C_2H_5COOK or KC_3H_5O_2) and 8.5 times 10^-2 M in propionic acid (C_2H_5COOH or HC_3H_5O_2) Express your answer using two decimal places. a solution that is 7.5 times 10^-2 M in trimethylamine. (CH_3)_3N. and 0.11 M in trimethylammonium chloride, (CH_3)_3NHC1 Express your answer using two decimal places. a solution that is made by mixing 50.0 mL of 0.16 M acetic acid and 50.0 mL of 0.22 M sodium acetate Express your answer using two decimal places.

Explanation / Answer

Answer for Part A:

pH = -log[H+] (base is 10 here with the log i.e. the log used here is cmmercial logarithm)

So, we need to know the concentration of H+ i.e. [H+]

The only reason for the production of H+ is propionic acid. Here the dissociation constant is not mentioned in the question so I will consider it as 1.

Molarity of Propionic acid is given here. As we have considered the dissociation constant as 1, it means that each of the Propionic acid gives one "H+" ion.

So the concentration of H+ is equal to the concentration of Propionic acid.

So, pH = -log[8.5 x 10-2] = - {log 8.5 + log 10-2} = -{0.93 -2} ; (using the property of logarithm, log mn = log m + log n)

pH = -{-1.07} = 1.07

Apply the reasoning mentioned above to find the pH of the different parts of your question

Thank You

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