vinegar into wells D1 through D5 of 24-well plate Place the reaction plate on white paper to make it easier to see any changes that occur 5. Cut 2 5-mm pieces of phenolphthalein test paper and add to wells D1—D5 6. Titrate with 0.1 M NaOH a. Hold dropping bottle vertically above well
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for Heat Change q=60g(160g*4.4c) =(60g*4.18J)/4.4j =1104.56 Joules CLASS TABLE part I Result Table Part II A-D PART Reaction Part A 15ml H₂O+ 25ml NaOH+ 20ml HCl Part B 34ml H₂O+25ml HCL+ 1g NaHO Part C 59g H₂O+ 1g NaOH Part D 10ml H₂O+ 25ml NaOH+25ml HOA PART Initial Tempature Final Tempature Change in Tempature ∆H Part A 24.2C 30.1C 5.9C 1481.136 J Part B 24.7C 28.5C 3.8C 0953.952 J Part C 24.0C 28.4C 4.4C 1104
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Miguel Paulo D. Valdez BS Chem-3 EXPERIMENT 14- Heat Effects and Calorimetry Objective/ Introduction: Heat is a form of energy‚ sometimes called thermal energy‚ which can pass spontaneously from an object at a high temperature to an object at a lower temperature. If the two objects are in contact‚ they will‚ given sufficient time‚ both reach the same temperature. Heat always travels from hot to cold objects and two objects will reach an equilibrium temperature. Heat flow is commonly measured
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remaining unreacted HCl with NaOH solution to determine the amount of acid which did not react with the calcium carbonate. The difference between the moles of the acid (HCl) initially added and the moles of HCl left unreacted after the reaction‚ is equal to the moles of HCl that did react with CaCO3. The reaction used to determine the amount of unreacted acid by titration is given below. This type of analysis is generally referred to as a back-titration. HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)
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PH at the UN Alfredo Vidal Ceballos 7/10/2014 Group Support Part 1: Solution Group Name and M. cons. Chem formula Type Experimental pH 1 Deidre Acetic Acid 0.1M HC2H3O2 Weak Acid 3.03 3.03 2 Acetic Acid 1M HC2H3O2 Weak Acid 2.59 2.54 3 Hydrochloric Acid 0.5M HClStrong Base 0.85 0.90 4 Jonah Nitric Acid 0.1M HNO3 Strong Acid 2.14 2.14 5 Sodium Acetate 1M NaC2H3O2 Weak Base 9.42 9.42 6 Potassium Dihydrogen Phosphate 0.1M KH2PO4 Weak Acid 5.47 5.47 7 Andy Potassium Hydrogen Phosphate 0
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cotton balls and acetic anhydride with acidic condition under heating. Materials: Styrene‚ 1 M NaOH solution‚ CaCl2(s)‚ xylene‚ t-butyl peroxybenzoate‚ methanol‚ 5% aqueous solution of 1‚ 6-hexanediamine‚ NaOH(s)‚ 5% sebacoyl chloride in hexane‚ glacial acetic acid‚ concentrated H2SO4‚ cotton balls‚ acetic anhydride‚ CH2Cl2 Procedure: For the synthesis of polystyrene‚ 10 ml styrene and 20 ml of 1 M NaOH solution was placed in separatory funnel and they were shaked for several times. Aqueous layer
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water. 3.00 mL of 0.1M NaOH was added to each of the 25mL buffer samples and to the distilled water and were mixed well in each tube. The pH of each solution was then recorded after the addition of the alkali. The results were recorded in a table. 20mL of an unknown sample was pipetted into a 100mL beaker. A burette was used to add 0.5mL aliquots of 0.1M NaOH and the pH was recorded from the pH meter. This procedure was repeated until pH of around 11 or 60mL of NaOH had been added with each
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reaction. Independent variable: The number of moles of the reactants Dependent Variable: The limiting reagent Constant Variable: The volume of reactants added Equipment: 2 100 ml beaker 2 measuring cylinders 10 ml of 0.1 molL-1 HCL(aq)‚ NAOH(aq) 20 ml of 0.1 molL-1H2SO4(aq)‚ CuSO4(aq) 30 ml of 0.1 molL-1 Ba(NO3)2(aq) Universal indicator Filter Paper Funnel 4 test tubes Reaction A- Method: 1) Measure 10 ml of 0.1 molL-1 of Hydrochloric Acid using a measuring cylinder
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MA‚ PAULINE Date Performed: 10 SEPTEMBER 2014 NACIONGAYO‚ DANIELLE Date Submitted: 17 SEPTEMBER 2014 TEDERA‚ YVES HEAT EFFECTS AND CALORIMETRY Experiment No. 2 I. RESULTS A. Determination of Heat Capacity In this experiment‚ an improvised calorimeter was used to determine the heat capacity. The calorimeter weighed 4.47 grams prior to the addition of water. Tap water‚ 40 mL to be exact‚ was added to the calorimeter which increased the weight to 43.87 grams. The water was measured using
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Chapter 8: Salts 1. Salts A salt is an ionic compound. The anion part comes from the acid while the cation part comes from a base. Example: KCl‚ KOH(aq) + HCl(aq) KCl(aq) + H2O(l) A salt is a compound formed when the hydrogen ion. H+ from an acid is replaced by a metal ion or an ammonium ion‚ NH4+. Salts Nitrate salts Carbonate salts Chloride salts Soluble All nitrate salts Potassium carbonate‚ K2CO3 Ammonium carbonate‚ (NH4)2CO3 Sodium carbonate‚ Na2CO3 All chloride salts Except Sulphate salts
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