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Introduction

Composition of Hydrates Purpose: The purpose of this lab was to determine the percentage of water in a hydrate and to calculate the coefficient of the water of hydration of a hydrate. Data Table: Mass of Crucible & Cover 22.03 g Mass of Crucible & Cover & Hydrate 24.45 g Mass of Crucible & Cover & Anhydrous Salt 23.71 g Analysis: Hydrate Mass (Before Heating): 24.45-22.03 = 2.42 g Anhydrous Salt Left (After Heating): 23.71-22.03 = 1.68 g Water Lost: 24.45-23.71 = .74 g Molar Mass of Hydrate used: CuSO4?5H20 = 63.55+32.07+64+10.10+80 = 249.72 g/mole Molar Mass of Anhydrous Salt: CuSO4 ...read more.

Middle

Regardless of the mass of hydrate, the percentage of water lost stays the same. But, the value is not always the theoretical value, often close; it may vary, depending on the time you have kept the hydrate over the fire. 2) If I used 5 grams of hydrate, I would expect to lose around 36.98% of water. That's about 1.849 grams. Conclusion: The purpose of this lab was to determine the percentage of water in a hydrate and to calculate the coefficient of the water of hydration of a hydrate. ...read more.

Conclusion

This report has shown that regardless of the mass of hydrate, the percentage of water loss stays the same. But, the value is not always the theoretical value; it may vary, depending on the time you have kept the hydrate over the fire. Sometimes you can overheat it and sometimes you can under-heat it. In our case, we under-heated the hydrate. We were aiming to lose 36.98% of water but only 30.58% was evaporated, that is, .74 grams out of 2.42 grams. Throughout the lab, we have faced only a single problem, we have not distributed the hydrate evenly through the crucible, one hydrate was over another hydrate. ?? ?? ?? ?? ...read more.

This student written piece of work is one of many that can be found in our AS and A Level Organic Chemistry section.