Suppose you have 1.00 Liter of an aqueous buffer containing 60.0 mmol benzoic acid (pKa=4.20) and 40.0 mmol benzoate.
Calculate the pH of this buffer.
What volume of 2.00M NaOH would be required to increase pH to 4.93?
Given,
pKa = 4.20
Benzoic Acid = 60 mmol
Benzoate (salt) = 40 mmol
We know that,
pH of a buffer = pKa + log (Salt / Acid)
=> pH = 4.2 + log (40 / 60) = 4.2 - 0.176 = 4.024
pH after adding NaOH = pKa + log (salt + X / Acid - X)
where,
X = mmol of NaOH added
=> 4.93 = 4.2 + log (40 + X / 60 - X)
=> 0.73 = log (40 + X / 60 - X)
=> (40 + X / 60 - X) = 5.37
=> X = 44.3
=> We will need 44.3 mmol of NaOH
Molarity of NaOH = 2
Volume = Moles / Molarity
=> Volume = 44.3 / 2 = 22.15 mL of NaOH is required
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