The pH of a buffer solution containing 0.10 M acetic acid and 0.1...

Question

The pH of a buffer solution containing 0.10 M acetic acid and 0.10 M sodium acetate is 4.74.

Write the Henderson–Hasselbalch equation for this buffer.

Accepted Answer

Hello. In this problem, we are told a buffer solution was prepared by mixing .25 molar hyper chloric acid and .3 molar potassium hypochlorite. The P K of hyper chose acid is 7.52. And the P H of the resulting solution is 7.60. We're asked to provide the Henderson House back equation for the buffer. So the general form of the Henderson has back equation is P H is equal to the P K A plus the log of the concentration of the base to that of the acid. In our problem, the acid is hypos acid which has a concentration of 0.25 molar. And then we have our conjugate base of this acid. So that would be the hypo chloride aine concentration of hyper chloride is 0.30 molar R P H then is equal to the PKA of 7. plus the log then of the concentration of the base which is 0.30 molar. And that's divided by the concentration of the acid which is 0.25 molar. And this then all equals 7.60. This answer then corresponds to answer D. Thanks for watching. Hope this helped.

The pH of a buffer solution containing 0.10 M acetic acid and 0.10 M sodium acetate is 4.74. Write the Henderson–Hasselbalch equation for this buffer.

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