Is the N Factor of Oxalic Acid in Titration Correctly Applied?

[Prabs3257]

Homework Statement

[" 50mL of "0.5M" Oxalic Acid is needed to neutralize "25mL" of sodium hydroxide "],[" solution.The amount of "NaOH" in "50mL" of the given sodium hydroxide solution is "]

Relevant Equations

Equation moles

I got a answer by equation the moles i took the n factor of oxalic acid as 2 and the naoh solution came out to be 2M but i got an answer of 4grams but the answer given is 2 grams am i correct ??

 

[mjc123]

It's a bit ambiguous because there are two possible reactions:
OH^- + 1/2 H₂Ox → H₂O + Ox^2-
OH^- + H₂Ox → H₂O + HOx^-
I've written them that way because you are adding the oxalic acid to the NaOH (by the way, there's no such thing as naoh). You will first form disodium oxalate, then monosodium hydrogen oxalate. The titration will have two endpoints.
Can you estimate the pH at these endpoints? To make it a bit simpler, just try to calculate the pH of a 1M solution of Na₂Ox, and a 1M solution of NaHOx. Which do you think best corresponds to "neutralisation" (if that term is not better defined in the problem)?
hint: for oxalic acid, pKa1 = 1.27, pKa2 = 4.27 (This question is assuming a lot of knowledge. How many marks do you get?)

 

[Prabs3257]

It's a bit ambiguous because there are two possible reactions:
OH^- + 1/2 H₂Ox → H₂O + Ox^2-
OH^- + H₂Ox → H₂O + HOx^-
I've written them that way because you are adding the oxalic acid to the NaOH (by the way, there's no such thing as naoh). You will first form disodium oxalate, then monosodium hydrogen oxalate. The titration will have two endpoints.
Can you estimate the pH at these endpoints? To make it a bit simpler, just try to calculate the pH of a 1M solution of Na₂Ox, and a 1M solution of NaHOx. Which do you think best corresponds to "neutralisation" (if that term is not better defined in the problem)?
hint: for oxalic acid, pKa1 = 1.27, pKa2 = 4.27 (This question is assuming a lot of knowledge. How many marks do you get?)

this is a high school grade question but why can't we simply equate the milliequivallents of both oxalic acid and NaOH

 

[epenguin]

Titrations with oxalic acid are most usually done if I remember right by adding alkali to the acid, because you traditionally use as indicator phenolphthalein whose alkaline form is coloured (has pK_a about 9) well above the oxalic acid pK's, so both -COOH groups have been titrated when you see the pink colour appear.

I get 4g; the student would have to set out reasoning in more detail for us to identify any misconception or mistake.

 

[Prabs3257]

Titrations with oxalic acid are most usually done if I remember right by adding alkali to the acid, because you traditionally use as indicator phenolphthalein whose alkaline form is coloured (has pK_a about 9) well above the oxalic acid pK's, so both -COOH groups have been titrated when you see the pink colour appear.

I get 4g; the student would have to set out reasoning in more detail for us to identify any misconception or mistake.

ya i am also getting 4g hence the answer given must be wrong thanks

 

[epenguin]

What is the source of the question?

 

[Prabs3257]

What is the source of the question?

its a sample question for jee mains its an enterance exam in india

 

[epenguin]

Is 2g the official answer? I don't think I would be able to enter there.
However I hope we shall get a second opinion.

 

[Borek]

Something is definitely wrong, 2 g is amount of NaOH that reacted, not amount of NaOH in 50 mL of the solution.

 

[symbolipoint]

Which equivalence point? Are the two of them close-enough for using phenolphthalein as the only indication? My guess is both hydrogens from the oxalic would be strong enough ionized in solution for that one indicator to be good enough; but my judgement could be wrong (unless I review the theory thoroughly).

 

[Borek]

 

[symbolipoint]

Borek has given a graphical clarification about the endpoint pH's for the titration so that surely helps. If you want to go to both endpoints, then this will be titrating for BOTH hydrogen ions from the oxalic acid. Notice that the more endpoint to pH 2.8 is not going to be very sharp; maybe this means you would want to take just the first enpoint, for which phenolphthalein would be the suitable endpoint (for ONE hydrogen ion).

 

[Borek]

On the second thought the problem is this question is poorly defined. It doesn't specify what it means by "needed to neutralize". If taken literally (and that would be my approach), oxalic acid is diprotic. If it is about titration, only the first end point is sharp enough to be usable. That gives two possible answers that differ by exactly 100%.