Question
Asked Oct 23, 2019
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What volume (in mL) of the following acid would be required for complete neutralization of 50.00mL of 0.100 M NaOH?

b. 0.100M Oxalic acid H2C2O4(aq), (a diprotic acid)

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Expert Answer

Step 1

The volume (in mL) of the following acid that would be required for complete neutralization of 50.00mL of 0.100 M NaOH is to be calculated-

b. 0.100M Oxalic acid H2C2O4(aq), (a diprotic acid)

Step 2

Oxalic acid (H2C2O4) is a diprotic acid, thus it will require to 2 equivalents of NaOH to neutralize 1 equivalent of H2C2O4.

Equation showing the complete neutralization of the oxalic acid-
HC204 (aq)2N2OH (aq)
Na,C,0, (aq) +H20 (1I)
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Equation showing the complete neutralization of the oxalic acid- HC204 (aq)2N2OH (aq) Na,C,0, (aq) +H20 (1I)

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Step 3

Therefore, for complete neutralization:

Moles of ...

Moles of H2C2O. =
Molarity of H,C,01xVolume ofH2C20
and
Moles of NaOH = Molarity of N2OH x Volume of NaOH
As for neutralization,
Moles of H,C,0, = 2x Moles of N2OH
:. Molarity of HC,0,xVolume of H,C,0 2x (Molarity of NaOH x Volume of NaOH
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Moles of H2C2O. = Molarity of H,C,01xVolume ofH2C20 and Moles of NaOH = Molarity of N2OH x Volume of NaOH As for neutralization, Moles of H,C,0, = 2x Moles of N2OH :. Molarity of HC,0,xVolume of H,C,0 2x (Molarity of NaOH x Volume of NaOH

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