University of New Haven Properties of Hydrates Chemistry Lab Report

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Before heating After heating Mass of crucible and sample Mass of crucible Mass of sample Mass of crucible and sample Mass of crucible Mass of sample Mass of water loss by dehydration 30.8 g 35.8 g 38.54 g 16.52 g 34.05 28.9g 28.9g 34.8g 16.15 33.64 1.9g 6.9g 3.7g 0.378g 0.406g 30.2 33.5 37.2 16.38 33.903 28.9 28.9 34.8 16.15 33.903 1.3 4.6 2.4 0.2344 0.260 0.6 2.3 1.3 0.1443 0.146 This is table 2 mass of crucible before and after
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Hello, I have completed the lab report. It has the sections of a formal report, calculations, and appendices. Please, if you need any clarification please contact me I will be glad to help you. Regards!

Running head: PROPERTIES OF HYDRATES LAB REPORT

Properties of Hydrates Lab Report
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PROPERTIES OF HYDRATES LAB REPORT
Hydrates are compounds that contain water molecules in their chemical composition.
According to Slowinski and Wolsey (2008), most of the hydrates are ionic salts. They hold water
in their crystals, which is referred to as the water of hydration. The water molecules can be
removed from the hydrate easily through heating. The dehydrated compound can also be
reversed to a hydrated compound by adding or exposing it to humidity. Examples include
sulfates of copper, cobalt, and iron. The heating reaction may also lead to color change.
However, while the loss of water is a significant characteristic of the hydrates, not all compounds
lose water due to dehydration. Some may produce water vapor as they break down into other
compounds such as sugar.
The aim of the experiment that was carried out in three distinct parts, discussed in this
report was to understand the properties of hydrates such as hydration and reversibility by
identifying hydrates among other compounds. Another objective was to determine the mass of
water in hydrated copper sulfate. Last but not least, the experiment sought to compare the
characteristics of Epsom salt or magnesium sulfate with those of the sulfates of iron, cobalt, and
copper.
Method and Materials
Part I: Hydration and Reversibility of Hydrates
In part, I of the experiment, four test tubes, three hydrated salts (sulfates of copper,
ferrous, and cobalt), test tube holder, a Bunsen burner and a striker, a beaker of water,
eyedropper, and a water bottle were the materials and equipment used.
A pea-sized amount of the three salts and the sugar were placed in four separate test
tubes. The test tubes were heated on a lit Bunsen burner for about a minute, and observations of
any colour change and reactions were made and recorded. Then, they were left to cool in a

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PROPERTIES OF HYDRATES LAB REPORT
beaker of water for a few minutes. Two to three drops of water were added to the test tubes once
they cooled, and the changes observed.
Part II: Percentage Mass of Water Determination in Hydrated Salts
Part II of the experiment involved one salt (Copper sulfate) divided into five samples.
The materials and the equipment included a Bunsen burner, five crucibles, a wire triangle, scale,
and iron ring. The procedure started with taking the mass of a crucible and recording it in a table
(see table 1 in the appendices), and adding 0 to 7 grams of the hydrated copper sulfate into five
separate crucibles. The mass after adding the sample was also recorded in the table. The crucible
containing the salt was then placed on the Bunsen burner using the wire triangle put on the iron
ring as a stand. The crucible was heat at the bottom gently until the salt changed color. It was
heated for an additional five minutes after changing the color. The sample was allowed to cool
and the mass recorded. The mass of water lost through dehydration was obtained by subtracting
the mass of the sample after the heating from the mass of the sample before heating, and it was
entered into the table accordingly. The procedure was repeated for all the samples, and the
correspondent data was recorded.
Part III
Part III of the experiment involved heating Epsom salt. A pea-sized amount of the Epsom
salt was placed in a test tube, and the appearance observed and recorded. Then, it was heated on
a Bunsen burner for around one minute, and observations were made as it heat and noted.
Results and Discussion
Part I
For experiment Part I, upon heating the substances, they reacted differently and resulted
in different colors. Before heating sugar had a white color and a soft texture, copper had a blue

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PROPERTIES OF HYDRATES LAB REPORT

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color and appeared crystal-like, while ferrous had a grey/yellow color and looked like sand.
Cobalt was dark red and also had a sandy texture. During heating, sugar heated very fast, and it
melted in no time. Copper began heating very fast too, and a stream of vapour was seen rising,
and ferrous sulfate also burned quickly, and gas was observed. Cobalt changed into a liquid
consistency when it was heated and changed color. After heating all the compounds changed in
color and texture. Apart from sugar that transformed into a sticky brown liquid, the salts turned
into solids. Copper and ferrous sulfates changed color to become white from blue and yellow
respectively, while cobalt turned blue from dark red (See...


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Really great stuff, couldn't ask for more.

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