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What is the expected pH of a solution that results from mixing 25.6 mL acetic acid...

What is the expected pH of a solution that results from mixing 25.6 mL acetic acid (pKa=4.76, 1.05 g/ml) and 36.2g sodium acetate (CH3COONa) and diluting to 100 ml?

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Answer #1

mass of acetic acid = volume x density

                               = 25.6 x 1.05

                              = 26.88

moles of acetic acid = 26.88 / 60 = 0.448

moles of sodium acetate = 36.2 / 82 = 0.442

pH = pKa + log([CH3COO-]/[CH3COOH])

pH = 4.76 + log (0.442 / 0.448)

pH = 4.75

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