Chemistry Coursework Planning Aim: To find the effect of concentration of thiosulphate on the rate of reaction between sodium thiosulphate and hydrochloric acid. Introduction: Word Equation for the reaction: Balanced Symbol Equation for the reaction: Observations during the reaction: • A yellow precipitate of Sulphur starts to form and the reaction mixture goes cloudy. • A colourless‚ poisonous gas of sulphur dioxide is given off. • Sodium Chloride (salt) and Water
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greatly enhanced when the water is acidic. The gradual dissolution of marble and limestone‚ as well as coral and seashells‚ in acids is due to acid− base neutralization. The products of the neutralization reaction between calcium carbonate and hydrochloric acid‚ for example‚ are calcium chloride and carbonic acid‚ or H2CO3. Carbonic acid is unstable‚ decomposing to give carbon dioxide gas and water. CaCO3(s) + 2HCl (aq) → CaCl2 (aq) + H2CO3(aq) H2CO3 (aq) →CO2 (g) + H2O (l) The rate of the overall
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altering concentration (mol dm-3) of hydrochloric acid (HCl) on the rate of reaction (mol dm-3 s-1) for the following chemical reaction: CaCO3(s) + HCl(aq) CaCl2(s) + H2O(l) + CO2(g) Research question: How does altering concentration (mol dm-3) of hydrochloric acid (HCl) affect the rate of reaction (g/s) for the following reaction: CaCO3(s) + HCl(aq) CaCl2(s) + H2O(l) + CO2(g) Background information: The reaction between calcium carbonate and hydrochloric acid is an example of a neutralization
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chosen must be suitable according to the type of reactions. But in this experiment‚ there are only two types of reactions which is strong acid-weak base titration and weak acid-strong base titration will be investigated. Materials Chemicals 0.1M Hydrochloric acid‚ 0.1M acetic acid‚ 0.1M sodium hydroxide‚ 0.1M ammonium hydroxide‚ phenolphthalein‚ screened methyl orange‚ methyl orange Apparatus 100mL Beakers‚ 250mL Conical flasks‚ 50mL Burettes‚ 25mL Pipettes‚ Pipette fillers‚ Funnels‚ pH meters Procedure
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Independent | Volume of titrated excess of hydrochloric aced | cm3 | Controlled | Volume of hydrochloric acid Weight of eggshell Temperature Amount of phenolophateine | cm3 g oC drop | Uncontrolled | Purity of solutions Biological diversity of eggs Pressure | - - hPa | Equipment: buret 5 beakers 50 cm3 baguette 1 plastic pipette balance clamp 2‚5 g of eggshell mortar 100 cm3 of 1moldm-3 hydrochloric acid ap. 70 cm3 of 1moldm-3 sodium hydroxide
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processing beginning with chemicals in the saliva from the salivary glands. This is called mastication. Then it travels down the esophagus into the stomach‚ where hydrochloric acid kills most contaminating microorganisms and begins mechanical break down of some food (e.g.‚ denaturation of protein)‚ and chemical alteration of some. The hydrochloric acid also has a low pH‚ which is great for enzymes. After some time (typically an hour or two in humans‚ 4–6 hours in dogs‚ somewhat shorter duration in house
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The Dissolving of Solid Sodium Hydroxide in Water Procedure: 1. Measure out approximately 200 mL of distilled water and pour it into the calorimeter. Stir carefully with a thermometer until a constant temperature is reached. Record the volume of water and the constant initial temperature of the water on your data table. 2. Place a plastic measuring trough on top of the digital balance‚ and then zero the balance (press the tare button) so that the mass of the trough will be "ignored" and
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Table of Contents Laboratory Safety and Laboratory Guidelines Common and Special Laboratory Equipment Materials and Other Requirements Common Laboratory Operations and Techniques Experiment 1 …………………………………………………………………………..10 Properties of Matter Experiment 2 …………………………………………………………………………. 12 Chemical Changes Experiment 3 …………………………………………………………………………. 15 Classification of Matter Experiment 4 …………………………………………………………………………
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salts Rust red residue Fe2O3 formed (from decomposition of iron compounds) Black residue from blue or green sample CuO formed (from decomposition of copper(II) compounds) Yellow residue when hot‚ white when cold ZnO formed (from decomposition of zinc compounds) Orange residue when hot‚ yellow when cold PbO formed (from decomposition of lead(II) compounds) Ammonia evolved Some ammonium salts Carbon dioxide evolved Some carbonates; hydrogencarbonates Nitrogen dioxide evolved Nitrates and
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light yellow but on the bottom of the test tube the yellow is darker. 3. Magnesium metal and hydrochloric acid solution Place one scoop of magnesium turnings into the test tube. Add hydrochloric acid slowly and observe the reaction. Next‚ place a burning splint near the mouth of the test tube to test for the presence of hydrogen gas. Observations when its put the magnesium metal and the hydrochloric acid solution it look like many bubbles Observacion: cuando se pone el metal de magnesio ala
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