A student weighs 1.575 g of oxalic acid dihydrate, H₂C₂O₄· 2H₂O (126 g/mol), dissolves it in…
Contributed by StemPy LabTry it on paper first. A hint, the key idea and the worked solution are here when you need them.
A student weighs 1.575 g of oxalic acid dihydrate, (), dissolves it in distilled water and makes the solution up to 250.0 mL in a volumetric flask. Find the amount of oxalic acid, the molarity of the solution, and the concentration of acidic hydrogen ions, in moles of for each litre, that it can give to a base.
Need a reminder? The key ideaShow
Molarity with in litres. For a titration with the equation , . Oxalic acid, , gives two for each molecule. Sodium carbonate takes two . Concordant titres agree within .
The worked solution
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Work it out on paper first. It is fine to get stuck or make a mistake: that is how we learn. When you are ready, go through the solution one step at a time, and check each step against your own.
Step 1. .
Step 2. .
Step 3. Two acidic hydrogen ions for each molecule: .
Answer: , and .
Check. The water of crystallisation is part of the weighed mass: .
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