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Chemistry Practical: Finding the water content of Na2 CO3 .xH2O by Titration

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Introduction

Chemistry Practical: Finding the water content of Na2 CO3 .xH2O by Titration Method Step 1: making up the solution Step 1. Weigh about 4g of sodium carbonate hydrate crystals into a dry weighing bottle. Place bottle, lid and powder onto the balance and weigh using an accurate balance to record weight to 3 d.p. Note: remember not to expose crystals to air for too long to avoid water loss from crystals. Step 2. Transfer the powder to a beaker (100 ml+ in size) Step 3. Reweigh the bottle and lid (and subsequently any powder left in the bottle that didn't fall out). Hence find the weight of sodium carbonate transferred to the beaker by subtracting it from the weight of the bottle, lid and powder. Step 4. Dissolve the powder in distilled water by stirring the solution. Step 5. Transfer the solution to a 250cm3 volumetric flask washing the beaker out with distilled water into the flask to ensure as much of the solution is washed into the flask as possible. ...read more.

Middle

v.) At this point run the acid into the solution at a slower rate (dripping it in slowly and shaking the solution in the process) so you can read the volume of HCl required to neutralise the solution to one drip (0.05 cm3). Note: take an accurate reading to within 0.05 and take the reading at the first colour change in the solution. Step 8. Repeat steps 12 and 13 until satisfactory results are obtained: vi.) Two results are obtained within 0.05 of each other vii.) Three results within 0.10 of each other Results For 25cm3 of Na2 CO3 .xH2O the following results were obtained by titration using HCl. Rough Accurate Accurate Burette Reading end (cm3) 28.75 28.85 28.90 Burette Reading beginning (cm3) 0.00 0.00 0.00 Volume of HCl added (cm3) 24.15 24.10 24.30 Average Titre (cm3) 28.875 Colour change at end point: slightly pinkie orange Calculations 1. Number of moles in 28.875 cm-3 of 0.1 moldm-3 of HCl =(28.875 x 0.1)/1000= 2.89x10-3 2. ...read more.

Conclusion

that I could have been more accurate when conducting my experiment: One inaccuracy may be due to the fact that when titrating I shook the flask too vigorously and not all the drops landed directly in the solution but on the inside of the flask which would have resulted in an over estimate of the volume of HCl. This problem could be resolved by reducing the rate at which I did the titration which would enable me to shake the flask more steadily. I could also repeat the titration more times- by doing this and averaging the closest few I would be more likely to find the precise volume of HCl required to neutralise the solution. I could also shake the volumetric flask before taking the 25 cm3 sample from it as the dissolved crystals settled to the bottom of the flask after a while resulting in a varied concentration throughout(it was not homogenous and would subsequently give varied results in titration). ?? ?? ?? ?? Sodium Carbonate Titration 08/05/2007 ...read more.

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