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# alevel chemistry moles watch

1. did i get this right and if not can u show how to get the full marks2 A solution of ethanedioic acid was prepared by dissolving 1.01 g of the acid in water and making the volume up to 250 cm3 in a volumetric flask. A 25.0 cm3 sample of this solution was titrated against NaOH and required 18.40 cm3 NaOH for neutralisation.
(COOH)2  2NaOH → (COONa)2  2H2O
a Calculate the number of moles of ethanedioic acid in 1.01 g. (1 mark)
b Calculate the concentration of the ethanedioic acid solution. (1 mark)
c Calculate the number of moles of ethanedioic acid used in the titration and hence calculate the number of moles of NaOH required for neutralisation.
d Calculate the concentration of the NaOH solution in:
i mol dm−3
ii g dm−3
2. this is my answer and workin out
mas/mr =1.01/90=0.0112
conc=massXvolume =0.0112/(250/1000)=0.448x2 = 0.896
0.896/0.025=35.84
3. hi, did you find the answer to this?
4. (Original post by loregillis99)
hi, did you find the answer to this?
nah cant remember prob not
5. (Original post by jkjj)
this is my answer and workin out
mas/mr =1.01/90=0.0112
conc=massXvolume =0.0112/(250/1000)=0.448x2 = 0.896
0.896/0.025=35.84
You've only given 3 answers to 4Q's. If you can order it properly I might be able to help u.

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