Titration Lab Cherno Okafor Mr. Huang SCH4U7 November 21st‚ 2012 Data Collection and Processing Concentration of the standard HCl solution: 0.1 M Data Collection: | Trial 1 | Trial 2 | Trial 3 | Final HCl Buret Reading ± 0.05 mL | 38.3 | 45 | 54.5 | Initial HCl Buret Reading ± 0.05 mL | 29.9 | 38.3 | 45 | Volume of NaHCO3 used ± 0.1 mL | 9.2 | 9.5 | 9.8 | Qualitative Data: * I used the methyl orange indicator which was suitable
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1198.1 | 6 | 1038.1 | 7 | 921.3 | 8 | 826.2 | 9 | 752.6 | 10 | 688.5 | 11 | 638.5 | 12 | 593.8 | 13 | 557.0 | 14 | 519.9 | 15 | 492.0 | 16 | B. Determining the Ideal Gas Constant Molar calculations: Mgs+2HClaq→MgCl2aq+H2(g) 5mL of 3M HCl nHCl=0.005L×0.3M1L=0.015mol nHCl 5×excess=0.0155=0.003mol nMg=0.0032=0.0015mol mMg=0.0015×24.31=0.0365g Volumes: * Tubing: Inner diameter= 0.53 cm Length= 46 cm V=πr2h=π0.265246=10.15mL * Flask: Measured empirically by filling the flask
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tube and an agar-water gel. In glass tube test‚ two cotton plugs submerse with two different substances – hydrochloric acid (HCL) and ammonium hydroxide (NH4OH) on the other end of the tube. By their molecular weight‚ NH4OH has a small molecular weight that diffuses at a faster rate. While the formation of a white cloud was first occurred at the end of the tube containing HCL with a large molecular weight. In agar-water gel test‚ using agar plate and agar-water gel‚ 2 different substrate were tested-
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. AIM :. To Determine which Antacid could Neutralize the most Stomach Acid. (Chemistry Project) Project Prepared By: Name Class- Roll no. INDEX page no. Objective 3 Introduction 3 Acids 4 Stomach Acid
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chemicals was mixed as follows and the observations of the reactions were recorded in Data Table 1. A1) Two drops of NaHCO3 and two drops of HCl. B1) Two drops of HCl and two drops of BTB. C1) Two drops of NH4OH and one drop of BTB. D1) Two drops of HCl and two drops of blue dye. A2) Two drops of blue dye and two drops of NaOCl. One drop of HCl was then added. F) Two drops of KI and two drops of Pb(NO3)2. G) Two drops of NaOH and two drops of phenolphthalein. H) Two drops of HCI and two
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hydrochloric acid particles to produce the salt Mg chloride and hydrogen gas. The amount of gas will be monitored at certain time intervals to find out the rate of reaction. However I will be changing the molarity of the HCl by diluting it with water. The water molecules will prevent the Mg and HCl particles to collide‚ this is because the water molecules will get in the way of the collisions therefore providing an obstacle for the two reacting particle. This will have an influence on the rate of reaction
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t Design and preparation of buffers effective at different pHs Abstract These experiments aimed to determine the optimum pH ranges various buffers are effective and provide opportunity for the use of the Henderson-Hasselbalch equation to prepare a buffer of a specific pH. Three different buffer systems were initially investigated; volumes of weak acid and weak bases of specified concentration were prepared and titrated against strong acid or strong base solutions with pH readings taken at frequent
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Data Tables: Part 1: Chemicals Well No. Observations of the Reaction A. NaHCO3 + HCl A1 clear‚ bubbles B. HCl + BTB B1 yellow‚ clear C. NH3 + BTB C1 clear blue D. HCl + blue dye D1 green E. Blue dye + NaOCl E1 clear blue with the 1 drop of HCl green/blue F. NaOCl + KI A2 rusty-yellow with 1 drop of starch black G. KI + Pb(NO3)2 B2 yellow‚ not clear H. NaOH + phenolphthalein A3 purple‚ violet I. HCl + phenolphthalein A4 clear J. NaOH + AgNO3 D3 murkey‚ brown K. AgNO3 + NH3 A4 purple
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and NaOH * Hydrochloric acid ranging from 1-3 molars * A scalpel Diagram: Method: * Take the large gelatine cube and cut into 15 equal pieces * Place on piece of the cube into the test tube * Measure out 10mls of HCl in the measuring cylinder * Pour the HCl into the test tube with the gelatine cube and start the clock * Time how long it takes for the pink colour inside the gelatine cube to completely disappear * You will also notice that the cube dissolves slightly Fair test:
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parts of this experiment. In Part I of the experiment‚ two different reactions are performed to determine the enthalpy of formation for magnesium oxide. One reaction will involve only Mg‚ and the other will involve MgO – both will react with 1M HCl. Using the change in heat for both of these reactions‚ the enthalpies can be determined. With the use of Hess’s Law‚ the enthalpies of both reactions along with the enthalpy of water can be used to determine the enthalpy of formation for magnesium
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