Acid and Bases 1 Determining Acids and Bases SNC-2D1 April 02‚ 2013 Acid and Bases 2 Purpose The purpose of this chemistry lab is to investigate and find patterns/tendencies between substances Introduction An acid is a solution that has more free hydrogen ions (H + ) than hydroxyl ions (OH - ) and a pH less than 7. A base is a solution that has less free hydrogen ions (H + ) than hydroxyl ions (OH - ) and a pH of more than 7. In the late 1800s‚ the Swedish scientist Svante
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4/2/14 Period: 1st Chemistry Sour Acids and Bitter Bases Purpose: The purpose of this lab was to observe the different reactions formed between various acids and bases with the aid of indicators. Equipment: 1. Safety goggles. 2. Droppers. 3. Red Litmus paper. 4. Blue Litmus paper. 5. pH paper. 6. Well plate. 7. Micro spatula. Materials: 1. Zinc. 2. Magnesium. 3. Iron. 4. Copper. 5. HCL. 6. HC₂H₃O₂. 7. NaOH. 8. Phenolphthalein. Procedure: Part A: 1. Add five drops
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CHM 2046 L Scheme of Analysis for Unknown 9A/9B “Fair Game” Unknowns * Cations: Na+‚ K+‚ NH4+‚ Ca2+‚ Mg(H2O)62+‚ Al(H2O)63+‚ Zn(H2O)62+‚ Cu(H2O)2+‚ Ag(H2O)+ * Anions: Cl-‚ NO3-‚ SO4-2‚ HSO4-‚ OH-‚ CO3-2‚ HCO3-‚ S-2 * Insoluble Salts: Ca(OH)2‚ CaCO3‚ CaSO4‚ Mg(OH)2‚ MgCO3‚ Ag2O‚ AgCl‚ Ag2S‚ CuO‚ CuCO3‚ CuS‚ Zn(OH)2‚ ZnCO3‚ ZnS * Alums: [Al(OH2)6]2(SO4)3∙6H2O‚ Na[Al(OH2)6](SO4)2∙6H2O‚ K[Al(OH2)6](SO4)2∙6H2O‚ NH4[Al(OH2)6]2(SO4)2∙6H2O * Hydrated Ions: Na2CO3∙10H2O‚ Na2SO4∙10H2O
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Analysis: Water Analysis Jasmine Kennedy Bey Lab Partners: Mohammed Alabbad‚ Drew Blackson Chemistry 1290-020 3/26/2014 TA: Rajendr Thakuri Purpose/Abstract: Students are tested for their knowledge of basic titration technique and proper usage of specific-use probes (those used for conductivity‚ alkalinity‚ and pH‚ chloride‚ nitrate and hardness detection) on Logger Pro software. The purpose of this comprehensive lab is to determine the chemical properties
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reaction is complete. Knowing the volume of titrant added allows the determination of the concentration of the unknown. Often‚ an indicator is used to usually signal the end of the reaction‚ the endpoint. chemed.chem.purdue.edu/genchem/lab/techniques/titration/what.html In this study we will use an indicator solution called phenolphthalein as an indicator. Phenolphthalein is colourless when the solution is acidic or neutral. When the solution becomes slightly basic‚ phenolphthalein
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Questions Why does the pink color‚ which forms at the point where the NaOH comes into contact with the solution in the flask‚ disappear more slowly near the endpoint? The reason is that the Phenolphthalein indicator slightly dissolve in HCl solution‚ the OH-ions reacted with Phenolphthalein indicator first then titrates with H+ ions. As the NaOH solution dripped into the flask‚ the OH-ions react with H+ions and the pink color disappear. However the H+ is limited‚ as adding more OH-‚ all H+ ions will
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Determining the Unknown Concentration of NaHCO3 (aq) Through Titration Introduction Titration is the accurate addition of a titrant- solution in a burette- into a measured volume of a sample (Kessel‚ 2003). There are many different types of titration‚ such as acid-base reaction‚ redox reactions‚ precipitation reaction and more (Dohrman). In this lab an acid base titration will be explored. In an acid-base titration‚ the concentration of an acid or base is unknown and is determined by the adding
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affect the volume of NaOH used to titrate the solutions by approximately 0.01ml. Moreover‚ it is not certain that the right amount of indicator was used for the titration of the unknown acid in trial 2. It is stated that 2 drops of indicator should be used. It was uncertain whether 1 drop or 2 drops were used. Another drop was added. Using the wrong amount of indicator‚ such as too much can shift the end point which tampers the results dramatically. Conclusion The objective of this lab
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Experiment 1: Observations of Chemical Changes Abstract: In the lab 1 experiment‚ the objective was to observed properties of various chemical reactions between twelve different basic compounds. Each reaction revealed chemical properties consisting of color change‚ CO2 gas formation‚ and/or precipitate formation. Certain reactions made it possible to distinguish between an acid and a base. Through the results of this experiment‚ chemical properties observed in the reactions could be used to associate
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range for the scale is 0-14. If something has a pH value of 0‚ it is extremely acidic‚ while the opposite is if something is a 14 it is extremely basic. Pure water has a pH of 7 and is very neutral. Either extreme can be harmful to humans. The indicator is typically a chemical that changes color if it comes in contact with an acid or a base (How Can You Tell If Something Is An Acid Or A Base‚ 2007). One way of making this happen is to add an acid or a base to something like red cabbage
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