Determine the pH (to two decimal places) of a solution prepared by adding 239 mL of...
Determine the pH (to two decimal places) of a solution prepared
by adding 239 mL of 0.750 M sodium dihydrogen citrate
(NaC3H5O(COOH)2COO) to 3.99 g of
sodium hydrogen citrate
(Na2C3H5O(COOH)(COO)2).
Assume the volume of the solution does not change and that the 5%
approximation is valid. pKa=4.77
Homework Answers
we have
pKa = 4.77
moles of sodium hydrogen citrate = 3.99 g / 236.09 g/mol = 0.0169 mol
moles of sodium dihydrogen citrate = 239 ml x 0.750 M = 0.17925 mol
therefore
using the henderson equation , we have
pH = pKa + log[sodium hydrogen citrate]/[sodium dihydrogen citrate]
= 4.77 + log( 0.0169 / 0.17925 )
= 4.77 + log(0.0943)
= 4.77 - 1.03
= 3.74
therefore pH of the solution is = 3.74
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Determine the pH (to two decimal places) of a solution prepared
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