Stirring rod Evaporating dish Magnet Magnifying glass Crucible tongs Spatula Balance Meeker burner Ring stand Iron ring Wire gauze Forceps Sulfur Iron filings Sodium Bicarbonate Sodium Chloride Sugar Sand Magnesium ribbon Hydrochloric Acid Distilled water Filter paper 9 disposable dishes Procedure: 1. Label 7 of the dishes with the names of the following products: Sulfur‚ Iron‚ Sodium Bicarbonate‚ Sodium Chloride‚ Sugar‚ Sand‚ and Magnesium. Place small samples of each in
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Did you observer any chemical changes in this experiment? Yes What evidence did you use to decide that something was a chemical change? I observed during the application of the hydrochloric acid to some of the substances bubbling‚ and smoking Give at least two examples of chemical changes you observed. Green changed from blue to application of HCL to Mg smoking and bubbling and CuCO3 Classify the following properties of sodium
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10.1 COMMON ACIDS and ALKALIS in DAILY LIFE A. ACIDS 1) In our daily life‚ there are many foods‚ drinks and flavourings that taste sour. e.g. yoghurt’ lemons and vinegar. 2) They taste sour because they contain acids‚ which give the sour taste. e.g. Yoghurt contains lactic acid. Lemons contain citric acid. Vinegar contains ethanoic acid. 3) Many household cleaners and personal care products also contain acids. e.g. Toilet bowl cleaners contain hydrochloric acid. Some body lotions
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Chapter 10 ComMon Acids and Alkalis 10.1 Acids and Alkalis 1. Acids taste sour. Many fruits contain acids. 2. The three mineral acids commonly found in the laboratory are hydrochloric acid‚ sulphuric acid and nitric acid. 3. Alkalis taste bitter and feel soapy or slippery. 4. The common alkalis found in the laboratory are sodium hydroxide solution‚ potassium hydroxide solution‚ calcium hydroxide solution and ammonia solution. 10.2 Acid-Alkali Indicators 1. An acid-alkali indicator
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mixture of sand‚ sodium chloride and calcium carbonate. Materials and Equipment 1. Two beakers 2. Experimental mixtures 3. Distilled water 4. Funnel 5. Filter paper 6. Evaporating dish 7. Buchner funnel 8. Weighing machine 9. Conical flask 10. Hydrochloric acid(HCl) 11. Potassium carbonate(K2CO3) 12. Rubber hose pipe 13. Heater Procedure 1. Obtain two clean beakers‚ then weigh and label them. 2. Get the mixture and weight it. Then add 50ml of water to beaker 1 and stirrer the mixture. 3. Prepare
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Measure out between 20 milliliters and 40 milliliters of the unknown HCl solution. 4. Record volume. 5. The amount of unknown HCl is then added to the 100-milliliter Erlenmeyer flask. 6. Add two drops of the indicator‚ phenolphthalein‚ to the acid in the flask. 7. Using the slider on the right hand side‚ add NaOH to the HCl in the Erlenmeyer flask (This action is known as titrate). Add the indicator until the color of the indicator turns a light shade of pink. 8. Record the volume. 9.
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Tin container testing Following are the different tests that are performed: 1) Temper Test: Standard: IS 1993- 1982 Take the sample strip of 90mm width. Carry out the ‘zero setting’ on Erichsen Testing machine. After zero setting‚ clamp the dial by tightening the screw. Insert the sample strip in machine and lock it by test piece holder. Confirm the light arrangement and the mirror is placed on its respective position. Switch on the lamp. Rotate the back screw at uniform speed‚ so that
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magnesium sulphate + zinc Double displacement is the swapping of elements‚ usually forming a solid. Eg. Lead nitrate + sodium chloride = sodium nitrate + lead chloride Neutralization is the reaction between an acid and alkali/base/carbonate . One example of neutralization is Sulphuric acid + magnesium oxide = magnesium sulphate + water Sodium hydroxide is a corrosive metallic base‚ and it is also called caustic soda. Nowadays‚ it is made along with hydrogen and chlorine‚ using the chloralkali process
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Well Chemical #1 (4 drops) Chemical #2 (4 drops) Observations: Chemical Change (Y/N) A1 NaHCO3 Sodium Bicarbonate HCl Hydrochloric Acid A2 NaOCl Sodium Hypochlorite KI Potassium Iodide Observation 1: + Add 2 drops of starch Observation 2: A3 KI Potassium Iodide Pb(NO3)2 Lead Nitrate A4 NaOH Sodium Hydroxide C20H14O4 Phenolphthalein A5 HCl Hydrochloric Acid C20H14O4 Phenolphthalein A6 NaOH Sodium Hydroxide AgNO3 Silver Nitrate B1 AgNO3 Silver Nitrate NH4OH Aqueous Ammonia Observation
Free Chemical reaction Hydrochloric acid Sodium bicarbonate
Hydroxide (NaOH) by titrating it with Hydrochloric Acid (HCl) and to identify any possible sources of error. A colour change from pink to yellow signified the end of each individual titre as the NaOH had been neutralised. Experimental: Method: Firstly two solutions were prepared to show the colour of the Phenol Red indicator in acid and alkaline conditions. These colours were then used to determine the end point of each titre. In the experiment 0.100M HCl (acid) was added‚ from a burette‚ to a solution
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