# What are the limitations of a waters of hydration experiment? [closed]

When a hydrated salt such as $$\ce{CuSO4.5H2O}$$ is subjected to heat, an anhydrous salt ($$\ce{CuSO4}$$) is produced. However the theoretical molar ratio of $$\ce{H2O:CuSO4}$$ and experimental molar ratio of $$\ce{H2O:CuSO4}$$ are not the same. Instead there is a percentage error, why does this occur? And how can we minimise this in this experiment? The hydrated salt was left on hot plate at 70 degrees celsius for 25 mins.

## closed as off-topic by andselisk♦, Todd Minehardt, Jon Custer, Tyberius, MithoronMar 6 at 22:41

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• Why, all experiments contain errors. If you want to know more, you have to tell us more. What is your experimental molar ratio, to begin with? – Ivan Neretin Mar 6 at 11:36
• My experimental molar ratio of H2O: CuSO4 is 4:1 – Huda Alnusairi Mar 6 at 11:49
• Then perhaps your experiment resulted in a monohydrate, rather than an anhydrous salt? – Ivan Neretin Mar 6 at 12:05
• The hydrate contained 4 moles of water for every 1 mole of CuSO4. The expected was 5 moles of water for every 1 mole of CuSO4. It was not a monohydrate as there was more than 1 mole of water per mole of compound. – Huda Alnusairi Mar 6 at 12:12
• Are you saying that maybe the hydrated salt was not heated enough, therefore not all water turned into steam therefore we were left with CuSO4.H2O + 4H2O (gas) instead of the intended CuSO4 + 5H2O (gas) – Huda Alnusairi Mar 6 at 12:26