1. Determine the pH of the buffer solution that is prepared by mixing 39.6 mL of 0.0956 M ADA−H (C6H9N2O5− ) to 49.4 mL of 0.0302 M ADA (C6H8N2O52− ). Assume the 5% approximation is valid. Report your answer to 2 decimal places. The pKa of ADA−H is 6.84.
2. Determine the pH of the ADA−H/ADA buffer solution after the addition of 376 mL of 0.00616 M solution of sodium hydroxide to the existing buffer solution. Assume the 5% approximation is valid.
millimoles of salt = 49.4 x 0.0302 = 1.492
millimoles of acid = 39.6 x 0.0956 = 3.786
pH = pKa + log [salt/acid]
= 6.84 + log [1.492 / 3.786]
= 6.44
pH = 6.44
2)
on addition of ’ C’ moles of base to acidic buffer salt moles increases and acid moles decreases
so
C = 376 x 0.00616 = 2.316
pH = pKa + log [Salt +C/acid - C]
= 6.84 + log [1.492 + 2.316 / 3.786 - 2.316]
= 7.25
pH = 7.25
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