Lab Report
Chemistry Lab Report
Water Hydration
Introduction:
A hydrated crystal or hydrated occurs when water becomes tightly attracted to a metal salt base on it’s polarity. The water molecules maintain integrity as molecules, however they are considered to be part of the formula of the hydrate. When the hydrate metal salt crystal is heated, the attractions to the water are broken by the heat energy and the water escape from the crystal. After heating the salt crystal is called as anhydrous, which means without water. Many of the salt contain transition metals such as cobalt that is colorful (purple). Often the color of transition metal like cobalt’s color will change as a function of how many waters it is attracted to. Compounds containing water (H2O) of hydrated are written with water separate by a dot (.). This (.) means for hydrated metal salt there are how many number of moles of water bound to each mole of that metal salt.
Research Question:
The aim of this experiment is to calculate the number of moles of water bounded to each mole of cobalt chloride ( CoCl2. H2O). This cobalt chloride hydrated may be monohydrate with 1 mole of water attracted to cobalt chloride. It may be dihydrate, trihydrate, tetrahydrate or pentahydrate; your task is to determine which one you are given.
Hypothesis:
If cobalt chloride were heated until there is no further lose in weight, 6 moles of water would be lost from 1 mole of salt. Therefore it is predicted that there are 6 moles of water in this reaction.
Materials (Apparatus):
1. 3 gram of cobalt chloride 2. Evaporating dish 3. Tongs to hold the evaporating dish 4. Ring stand 5. Iron ring 6. Clamp 7. Bunsen burner 8. Matches 9. 40.20 g size of the crucible 10. Digital balance/ g 0.01 11. Clay triangle 12. Gloss rod
Procedure:
1. Place an empty crucible on digital balance by uncertainty of 0.01g 2. Measure the size of the crucible
Water Hydration
Introduction:
A hydrated crystal or hydrated occurs when water becomes tightly attracted to a metal salt base on it’s polarity. The water molecules maintain integrity as molecules, however they are considered to be part of the formula of the hydrate. When the hydrate metal salt crystal is heated, the attractions to the water are broken by the heat energy and the water escape from the crystal. After heating the salt crystal is called as anhydrous, which means without water. Many of the salt contain transition metals such as cobalt that is colorful (purple). Often the color of transition metal like cobalt’s color will change as a function of how many waters it is attracted to. Compounds containing water (H2O) of hydrated are written with water separate by a dot (.). This (.) means for hydrated metal salt there are how many number of moles of water bound to each mole of that metal salt.
Research Question:
The aim of this experiment is to calculate the number of moles of water bounded to each mole of cobalt chloride ( CoCl2. H2O). This cobalt chloride hydrated may be monohydrate with 1 mole of water attracted to cobalt chloride. It may be dihydrate, trihydrate, tetrahydrate or pentahydrate; your task is to determine which one you are given.
Hypothesis:
If cobalt chloride were heated until there is no further lose in weight, 6 moles of water would be lost from 1 mole of salt. Therefore it is predicted that there are 6 moles of water in this reaction.
Materials (Apparatus):
1. 3 gram of cobalt chloride 2. Evaporating dish 3. Tongs to hold the evaporating dish 4. Ring stand 5. Iron ring 6. Clamp 7. Bunsen burner 8. Matches 9. 40.20 g size of the crucible 10. Digital balance/ g 0.01 11. Clay triangle 12. Gloss rod
Procedure:
1. Place an empty crucible on digital balance by uncertainty of 0.01g 2. Measure the size of the crucible