Hi,
I have attempted this question a number of times and I'm completely stuck - I can see what you're meant to do, but the numbers I get never match up to the question.
1.575 g of hydrated ethanedioic acid, H2C2O4.xH20, was dissolved in 250 cm^3 distilled water. In a titration, 25.0 cm^3 of this acid solution was neutralised by exactly 25.0 cm^3 of dilute sodium hydroxide, concentration 0.100 mol dm^3. The equation is shown below:
H2C2O4 +2NaOH --> Na2C2O4 + 2H20
a) Calculate the number of moles of anhydrous ethanedioic acid in the weighed sample of hydrated ethanedioic acid.
b) Calculate the mass of anhydrous ethanedioic acid in the weighed sample and thus calculate the mass of water of crystallisation in the hydrated acid.
c) Calculate the number of moles of water of crystallisation in the hydrated acid and hence state the formula of the hydrated acid.
Anyone know what to do?
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