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11 Nov 2019

The acid dissociation constant (Ka) of acetic acid at 25 C was found to be 1.75 x 10^-5. Under these conditions, the base hydrolysis constant (Kb) of the acetat ion should be this:

Correct answer is 10^-11 mol/L. Please show all work.

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Jamar Ferry
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22 Mar 2019

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Related questions

An aqueous buffer solution (volume 1.00 L0 was prepared at 25 C by dissolving 6.00 g of acetic acid (Ka = 1.75 x 10^-5) and 4.10 g sodium acetate. This was the pH the resulting buffer solution:

Correct answer is 4.46. Please show all work.

a) Trichloroacetic acid, CCl3COOH, has an acid dissociation constant of 2.0 × 10-1 at 25 °C. Calculate the pH of a 0.0420 M trichloroacetic acid solution. (The correct answer is 1.45 but I would like to see the work)

ph = ______

b) Trichloroacetic acid, CCl3COOH, has an acid dissociation constant of 2.0 × 10-1 at 25 °C. How many times greater is the H3O+concentration in this solution than in a 0.0420 M acetic acid (Ka = 1.8×10-5)? (The correct answer is 41 but I would like to see the work)

1.00 M acetic acid (Ka = 1.75 x 10^-5 at 25 C) and 1.00 M sodium acetate were used to prepare a buffer solution. This buffer will have maxium buffer capacity at this pH:

correct answer is 4.76. Please show all work.

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