Question

A buffer contains equal concentrations of a weak base, B, and its conjugate acid, BH+. If...

A buffer contains equal concentrations of a weak base, B, and its conjugate acid, BH+. If the value of Kb for B is 1.0 x 10-9, what is the pH of the buffer?

A. 13.0

B. 9.0

C. 1.0

D. 7.0

E. 5.0

Please show your work. Thank you.

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Homework Answers

Answer #1

Use Handerson's equation to determine the pOH of the given weak base.

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

Given Kb = 1.0 x 10-9

pKb = -log(1.0 x 10-9)

       =9.0

Let the concentration of weak base B and its conjugate acid BH+ = 10M

pOH = 9.0+log[10/10]

=>pOH = 9.0

We know that pH+pOH =14

pOH = 9.0

Then pH = 14.0-9.0

               = 5.0

Hence, optionE is the correct answer.

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