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Enter your answer in the provided box. calculate the ph at 25°c of a 0. 11 m solution of a weak acid that has ka = 9. 2 × 10−6. ph =

Sagot :

The pH at 25°c of a 0. 11 m solution of a weak acid that has ka = 9. 2 × 10−6 is 3.

What is base dissociation constant?

The base dissociation constant is termed as Kb. Throughout a base split into ts constituent ions in water is determined by its base dissociation constant.

Kb = [H+] [A-]/[HA]

Now, let the concentration of [H+] = [A-] = x

Given,

Ka = 9.2 × 10−6.

Firstly we will calculate the value of the concentration of [H+]

pKa = x^2/(0.11-x)

9.2 × 10−6 = x^2/(0.11-x)

x^2 = 1.012 × 10−6

x = 1.002 × 10^−3.

The concentration of [H+] = [A-] = 1.002 × 10^−3.

Now, we will find pH as

pH = -log[H+]

pH = -log(1.002 × 10^−3)

pH = 3

Thus we calculated that the pH of the solution is 3.

learn more about pH :

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