tables of pKa provided A buffer solution is prepared by mixing 66.1 mL of 0.0360

Question

tables of pKa provided

A buffer solution is prepared by mixing 66.1 mL of 0.0360 M sodium hydrogen citrate with 17. mL of 0.285 M sodium citrate. 1. Calculate the pH (to two decimal places) of this solution. Assume the 5% approximation is valid and that the volumes are additive 2. Calculate the pH (to two decimal places of the buffer solution afterthe addition of 2.61 g of sodium citrate Na3C3H50 Coo 3) to the buffer solution above. Assume 5% approximation is valid and that the volume of solution does not change

Explanation / Answer

1. pH = pKa + log[sodium citrate]/[sodium hydrogen citrate] pH = 6.40 + log[.285x17.6]/[0.0360x66.1] pH = 6.72 is the answer 2.) 2.61 g of sodium citrate = 2.61/258.06 = 0.01 Thus, pH = pH = 6.40 + log[.285x17.6]/[0.0360x66.1] = 6.80

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