If a buffer solution is 0.250 M 0.250 M in a weak base ( K b = 8.0 × 10 − 5 ) Kb=8.0×10−5) and 0.540 M 0.540 M in its conjugate acid, what is the pH ?

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Question:

If a buffer solution is 0.250 M 0.250 M in a weak base ( K b = 8.0 × 10 − 5 ) Kb=8.0×10−5) and 0.540 M 0.540 M in its conjugate acid, what is the pH ?

Answer:

Answer:

9.57

Explanation:

Given that:

?f=pK %7Bb%7D%3D %5Clog%5C%20K %7Bb%7D%3D %5Clog(8.0%5Ctimes%2010%5E%7B 5%7D)%3D4

Considering the Henderson- Hasselbalch equation for the calculation of the pOH of the basic buffer solution as:

?f=pOH%3DpK b%2Blog%5Cfrac%7B%5Bconjugate%5C%20acid%5D%7D%7B%5Bbase%5D%7D

So,  

?f=pOH%3D4.1%2B%5Clog%5Cfrac%7B0.540%7D%7B0.250%7D%3D4

pH + pOH = 14  

So, pH = 14 – 4.43 = 9.57

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