reaction in a reaction. Through the experiment‚ the concentration of NaOH‚ and mystery of the unknown acid # 25 was accomplished. In both parts A and B of the experiment‚ a weak acid-strong base reaction occurred. Results indicate that unknown acid # 25 is oxalic acid which is a weak acid. When oxalic acid dissolves in water ‚ a few of its molecules will ionize in water‚ and a small amount of hydronium ions are produced. When NaOH is added‚ the hydronium ions will react with the strong base. Due to
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Position a burette over the beaker and fill it up with the NaOH solution of unknown concentration. 6. Add NaOH in progressively shorter steps until you observe an abrupt rise in pH. 7. Record the pH each time . 8. Continue adding NaOH in progressively longer steps until the pH does not change considerably. Part II Repeat the above procedure using the ethanoic acid solution of unknown concentration Processing Part I 1. Plot pH versus volume of NaOH added to the acid 2. Find from the graph the equivalence
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this investigation was to determine the enthalpy of the solution created when dissolving Sodium Hydroxide (NaOH) in water (H2O). THEORY When a solid ionic compound is dissolved in water a change of enthalpy is involved. _The enthalpy of a solution_‚ ΔHsol is the enthalpy change when one mole of the substance is dissolved in water to form aqueous solution. � CHEMICAL Sodium Hydroxide (NaOH) PROCEDURE The recommended amount of compound ito use is around 0.1 moles. Add water into your caleriometer
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swish around fluids every 20 seconds. 5) Add 5 drops of methyl orange to each flask. 6) Record observations. 7) Add 1ml of NaOH until you see a color change (both flasks are the same color) 8) Record amount of NaOH used for each antacid. 9) The flask that needed the least NaOH is best/more effective. 10) Clean your equipment. Observations: Antacid Color MCL acid NaOH Tums Merky liquid‚ yellow 35ml 5ml Rexall Yellowish orange 35ml 5ml Results: In an experiment to determine whether
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of HCL Aqueous Alkalimetry Direct titration 0.1N NaOH Methyl Red TS HCL + NaOH NaCl + H2O Assay of Diluted H3PO4 Aqueous Alkalimetry Direct titration 0.1N NaOH Thymolphthalein TS H3PO4 + 2NaOH Na2HPO4 + 2H2O Assay of H3BO3 Aqueous Alkalimetry Direct titration 0.1N NaOH Phenolphthalein TS H3BO3 H+ + BO2- + H2O Assay of Tartaric Acid Aqueous Alkalimetry Direct titration 0.1N NaOH Phenolphthalein TS H2C4H4O6 + 2NaOH Na2C4H4O6
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Analysis of Soda Ash and Volumetric Analysis of a Carbonate-Bicarbonate Mixture Belardo‚ Pia Jobelle J. Department of Chemical Engineering‚ Faculty of Engineering University of Santo Tomas España‚ Manila February 27‚ 2013 Abstract The analyte used is the soda ash which is titrated with an HCl titrant‚ standardized by Na2CO3. The indicators used are phenolphthalein for basicity and methyl orange for acidity. The two volumes of the titrant are then used to calculate percent composition of
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excess of acid to dissolve all of the CaCO3 and then titrating the remaining H3O+ with NaOH solution can achieve the determination of the amount of acid‚ which has not reacted with the calcium carbonate. There are differences between amount of the acid (HCl) added and the amount left over after the reaction is equal to the amount used by the CaCO3. The reaction used to determine the leftover acid is: HCl (aq) + NaOH (aq) H2O + Na+ (aq) + Cl- (aq) Aim To measure the percent by mass of CaCO3 in an
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Experiment 11 Calorimetry and Hess’s Law Purpose- To determine the change in enthalpy for four reactions using calorimetry and Hess’s Law Procedures: A. Calibration of the Calorimeter 1. Obtain two copper cylinders and a Styrofoam cup with lid from your lab instructor. Check out a digital thermometer display from the storeroom window. 2. Set up a hot water bath using a 600mL beaker‚ ring stand‚ and Bunsen burner. Weigh the two copper cylinders
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Determining Stoichiometric Ratios: NaOH and HCl & NaOH and H2SO4 Reactions Contents Introduction 3 Materials & Procedure 4 Raw Data 8 Processed Data 15 Graphs 16 Conclusion & Evaluation 17 Introduction Background Information Stoichiometry is a critical component in chemistry‚ and helps in understanding the quantitative relationship between the number of moles of reactants and products in a reaction. Objective In this experiment‚ the reactions
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bunsen burner sparker 2 -250mL beakers 10mL grad cylinder 0.2M FeCl3 0.2M KSCN 0.2M KCl 0.2M Fe(NO3)3 6.0M NaOH CoCl26H2O 6.0M HCl water 0.1M K2CrO4 0.1M K2Cr2O7 1M NaOH 1M HCl 0.1M Ba(NO3)2 Procedure PART I 1. Use a 10mL graduated cylinder to measure 1mL of 0.2M FeCl3 and pour it into a 250mL beaker. Using another 10mL graduated
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