[functions]

A solution contains 0.063g of oxalic acid, H₂C₂O₄·2H₂O, in 250 mL. What is the molarity of this solution?

This oxalic acid occurs as dihydrate. In the calculation of the molarity, we should take the number of moles to be the number moles of the dihydrate H₂C₂O₄·2H₂O or just the number of moles of the anhydrous H₂C₂O₄?

[sjb]

A solution contains 0.063g of oxalic acid, H₂C₂O₄·2H₂O, in 250 mL. What is the molarity of this solution?

This oxalic acid occurs as dihydrate. In the calculation of the molarity, we should take the number of moles to be the number moles of the dihydrate H₂C₂O₄·2H₂O or just the number of moles of the anhydrous H₂C₂O₄?

Are you (mentally) weighing out the dihydrate, or the anhydrous form when this solution is prepared?

[functions]

A solution contains 0.063g of oxalic acid, H₂C₂O₄·2H₂O, in 250 mL. What is the molarity of this solution?

This oxalic acid occurs as dihydrate. In the calculation of the molarity, we should take the number of moles to be the number moles of the dihydrate H₂C₂O₄·2H₂O or just the number of moles of the anhydrous H₂C₂O₄?

Are you (mentally) weighing out the dihydrate, or the anhydrous form when this solution is prepared?

The mass of 0.063g is for H₂C₂O₄·2H₂O.

[Borek]

The mass of 0.063g is for H₂C₂O₄·2H₂O.

If you are weighing dihydrate - can you you ignore water, or is it part of the mass of the sample?

[functions]

The mass of 0.063g is for H₂C₂O₄·2H₂O.

If you are weighing dihydrate - can you you ignore water, or is it part of the mass of the sample?

I not think so.

[Borek]

You don't think you can ignore, or you don't think it is part of the mass of the sample?

And if you will answer just "Yes" it will be funny, but I will lock the thread.