a) Barium chloride solution is mixed with copper sulphate solution and a write precipitate is formed. b) On heating copper powder in a china dish‚ the surface of copper powder become black. c) On heating green ferrous sulphate crystals‚ reddish brown solid is left as residue and a gas having smell of burning Sulphur is evolved. d) Iron nails when left dipped in blue copper sulphate solution become brownish in colour and blue colour of copper sulphate solution fades away. e) Quicklime reacts vigorously
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Percent water of crystallization is calculate by (1.17/3.31)+(1.39/4.18) divided by 2 which equal to 0.34300051=34.3 percent The Formula of Hydrate is CuSO4 times 5H2O Errors and Uncertainties 1. First of all‚ when I heating the hydrated copper sulphate‚ some of powder sticks on the glass-stirring rod. Therefore‚ I could not measure the exact weight since there was still a small amount of hydrate copper (II) Sulfate left on the stirring rod. 2. Second‚ I believe that there are major errors in
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Ammonium sulphate (NH4)2SO4. FW = 132.14‚ Eq. = 66g/l. 250ml 0.05M = 1.325g = 0.1N | Adipic acid HO2C(CH2)4CO2H‚ FW = 146.4‚ Eq. = 73.03g/l 250ml 0.05M = 1.83g = 0.1N | Barium hydroxide Ba(OH)2.8H2O‚ FW = 315.48‚ Eq. = 157.5g/l 250ml 0.05M = 3.94g = 0.1N | Benzoic acid C6H5COOH‚ FW = 122.12‚ Eq. = 61g/l 250ml 0.05M = 1.52g = 0.1N | Calcium carbonate CaCO3‚ FW = 100.00‚ Eq. = 50g/l 250ml 0.05M = 1.25g = 0.1N | Furroic acid FW = 112.08‚ Eq. = 112g/l 250ml 0.1M = 2.8g = 0.1N |
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Surfactant Surfactants are also known as ‘surface active agents’. They are usually organic compounds that contain hydrophobic tails and hydrophilic heads. They have wetting‚ emulsifying and dispersing properties‚ which can be used to improve the wetting ability of water‚ break up stains and keep the dirt in the water solution to prevent re-deposition of the dirt onto the surface from which it has just been removed. Surfactant can act as wetting agent as it lowers the surface tension of water.
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DETERMINATION OF THE CHEMICAL FORMULA FOR A HYDRATE USING MOLE RATIO OF WATER MASS AND MAGNESIUM SULPHATE INTRODUCTION Ionic (salt) compounds are able to hold loose bonds with water molecules. A hydrate is a compound that incorporates water molecules into its crystalline lattice structure (McGraw-Hill Ryerson‚ 2014). Identifying a compound as hydrated or anhydrous is important as the mass of the compound increases if it contains water molecules. In nature‚ hydrates exist with a fixed ratio
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and camphor. 2. To separate sand and salt in pure and dry state from the given mixture of sand and salt. 3. To prepare common salt by treating acid with base. 4. To prepare crystal of copper sulphate from the given mixture of sand and copper sulphate. 5. To prepare barium sulphate by treating barium chloride with dilute sulphuric acid in pure state. 6. To separate sand and calcium carbonate in pure and dry state from the given mixture of sand and calcium carbonate. 7. To obtain
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BONE BROTH: WHAT AM I DRINKING ANCIENT HISTORY Bones are hard unflattering to the eye and supposedly lifeless but yet they are an embodiment of life’s essential nutrients. Imagine everything you get from your vitamin capsules and supplements but in a spicy hot form. Bone broth is typically made with bones and can contain a small amount of meat attached to the bones it provides essential nutrients in an easily absorbable form‚ as with stock. Bones are typically roasted to improve the flavor of the
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Hong Kong Diploma of Secondary Education Examination Chemistry School-based Assessment Sample Tasks Teachers may use the sample tasks for non-profit making educational and research purposes with proper acknowledgement. © 留 2010 Hong Kong Examinations and Assessment Authority All Rights Reserved 2010 Chemistry School-based Assessment Practical Related Tasks Volumetric analysis Teacher Notes NSS Chemistry Curriculum Link: Time Required: 40 minutes Topic IV Acids and Bases Students
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Brooks‚ 2012‚ page 12-19. With the following changes: The mass of recrystallization mixture is 10.05g not 10g. Results: Part A: Compound (copper sulphate‚ sand and table salt) dissolved into hot water the solution turned a blue homogenous colour‚ leaving unwanted sand particles and a small amount of undissolved copper sulphate laying at the bottom of the beaker. Ethanol was added to the mixture and crystals started to from. After cooling duration crystals are visibly bound together.
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When the sugar dissolves... -The moving water molecules crash into the sugar particles -The sugar particles then break away from the crystal and into the water -The sugar and water particles then mix and diffuse evenly throughout. Copper sulphate- blue crystals‚ hydrated because they have water trapped within them. When they are heated this water evaporates‚ the crystals become dehydrated and turn white. Equation for this Reaction. CuSo4 5H2O ---> CuSo4 + 5H2O Solute- Solid which
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