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Enter your answer in the provided box. calculate the ph at 25°c of a 0. 0077 m solution of a weak base with a kb of 6. 2 × 10−9. ph =

Sagot :

The pH at 25°c of a 0. 0077 m solution of a weak base with a kb of 6. 2 × 10−9 is 8.8.

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 = [B+] [OH-]/[BOH]

Now, let the concentration of [B+] = [OH-] = x

Given,

Kb = 6. 2 × 10^-9

6. 2 × 10^-9 = x^2/(0.0077-x)

x = 6.909 × 10^(-6)

[B+] = [OH-] = 6.909 × 10^(-6)

As we know that,

pOH = -log [OH-]

pOH = -log( 6.909 × 10^(-6))

pOH = 5.2

As we also know that,

pOH + pH = 14

pH = 14 - pOH

pH = 14 - 5.2

pH = 8.8

Thus we calculated that the pH of the solution is 8.8.

learn more about pH :

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