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Lab 2 post lab - In experiment 2 a qualitative experiment...

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Benjamin McKinney Lab 2 In experiment 1 heat was used to evaporate the water from an unknown hydrate (Unknown B). Using a Bunsen burner, 0.497g of the compound was heated in a crucible. There were three fifteen minute heating sessions, and the sample was weighed after each of the sessions. The mass of the anhydrous sample was 0.372g, so the amount of water in the hydrate was 0.125g. The calculated percent of water in the unknown sample is 25.2%. The identity of the sample was found by comparing the percentage of water to that of five different given compounds. Unknown B had the smallest difference of percent of water to CuCl 2 *2H 2 O (26.46% water); therefore it can be assumed the sample was to CuCl 2 *2H 2 O. The reason for the small difference in percent of water could be due to the sample not being completely heated to constant weight, but there was not enough time in lab to do this completely.
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Unformatted text preview: In experiment 2, a qualitative experiment must be written to determine which compound is being formed from using the same reactants but a different ion of iron. In the first equation, iron (2+) reacts with copper sulfate to form copper and iron(II) sulfate; in the second equation, iron(3+) is reacted with copper sulfate to form copper and iron(III) sulfate. For the experiment 1g iron should be mixed with 2-2.5g copper sulfate. Iron should be the limiting reagent in the first equation, so if there is extra iron left from the reaction then iron(III) sulfate and copper are produced. If there is not any iron left from the reaction then iron(II) sulfate and copper are formed. When the experiment was performed, iron (1.01g) was reacted with copper sulfate (2.435g) in 100mL of water. There was no extra iron left, so iron(II) sulfate was the compound formed....
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