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9 September, 09:34

Out of the following, which is the best acid/base to use to prepare a buffer with a pH of 11.00? a. hydrogen peroxide b. phenol c. propylamine What ratio of masses of the weak acid/base and its conjugate should you use to make the buffer of the required pH? Use the sodium salt of the conjugate base if you chose a weak acid or the chloride salt of the conjugate acid if you chose a weak base.

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  1. 9 September, 12:53
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    Considering the Henderson - Hasselbalch equation for the calculation of the pH of the buffer solution as:

    pH=pKa+log[base]/[acid]

    Where K is the dissociation constant of the acid.

    The weak acid for making the buffer must have a pKa value near to the desired pH of the weak acid.

    Propyl amine has pka = 10.71

    So, Propyl amine will be the best. It is a base. So, the conjugate will be chloride salt of it.

    pH=pKa+log[base]/[acid]

    pH = 11.00

    pKa = 10.71

    So,

    log[base]/[acid] = 11.00 - 10.71

    [base]/[acid] = 1.95
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