a paper tray using an electronic scale. 2. Take (60 ml-80ml) of HCl and dissolve crushed eggshell in solution for eight to ten hours or until reaction between eggshell and acid is complete. 3. Rinse burette with NaOH solution and place in burette stand. 4. Rinse pipette with HCl. 5. Rinse conical flask with distilled water. 6. Filter acid and eggshell solution into beaker through funnel to remove unreacted HCl. (This step is necessary not for chemical reasons‚ but rather so that
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Discussion The acid neutralising capacity (ANC) of 3 brands of calcium carbonate (CaCO3) tablets was determined by reacting the tablets in excess standardized hydrochloric acid (HCl) and then back-titrating with a standardized sodium hydroxide (NaOH) solution. Back titration was required for two reasons. Firstly‚ CaCO3 tablets are poorly water-soluble but dissolve rapidly in acid. Secondly‚ CaCO3 is a weak base so it is difficult to determine the end point of the reaction if titrated directly. Assuming
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Introduction The major component of eggshells is calcium carbonate (CaCO3). Calcium carbonate cannot be dissolved in water‚ but can dissolve in an acid using the reaction: 2HCl(aq)+CaCO3(s) Ca2+(aq)+CO2(g)+H2O+2HCl-(aq) This reaction is not used to titrate the CaCO3 because it is very slow when the reaction is close to the endpoint. Instead adding an 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
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percentage by mass of calcium carbonate‚CaCO3 in toothpaste using back titration technique. A known weight portion of toothpaste is obtained to react with known volume and concentration of standard acid solution. After completing the reaction‚ the resulting solution containing excess acid is back titrated with known volume and concentration of standard base solution. Determination of excess acid after reaction allow us to calculate the amount of acid react with CaCO3 in toothpaste sample. My result for
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soluble in water. 2. When 15% of HCl was added to CaCl2 as the teacher was performing the experiment I observed and realized some changes took place physically. It was physical change because the color was clear. 3. By adding 15% of HCl of CaCo3 ‚ made it change chemically‚ I would tell this by effervescence and observation. 4. The most obvious difference is that when CaCl2 was mixed with 15% HCl it changed physically and the solid remain on the filter paper is CaCo3 reacted to 15% it changed chemically
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Thermometer CaCO3 Kim Wipes 1 M HCl (aq) Mg Ribbon Quantitative balance Pressure sensor GLX Machine Syringe with white connectors Tygon Tubing 125 mL flask with one-hole stopper 50 mL graduated cylinders Procedure Record the Temperature and convert into K Determine the volume of the Flask and Tygon Tubing you will be using Connect the Pressure sensor to the GLX Machine and then connect the Tygon Tubing to the Pressure Sensor. Weigh the Mass of the Mg Ribbon and The CaCo3 and wrap
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the sample to be analysed‚ CaCO3 does not dissolve in water. Hydrochloric acid and sodium hydroxide are the reagents used in this experiment. The precise measured amount of HCl is added to the weighted portion of toothpaste which is CaCO3. When the reaction between HCl and CaCO3 is completed‚ the excess HCl is back-titrated against NaOH until the reaction reaches the end point and the indicator changes from pink to orange. Hence‚ the amount of HCl that has reacted with CaCO3 can be calculated by using
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will test this by seeing how much drops of hydrochloric acid (HCl) are required to neutralize a certain amount of the antacid. Antacids are used to resist heartburn. We sometimes use them to treat this because antacids are a mild base that can neutralize acids in our stomachs‚ such as HCl. The purpose of this lab is to see how well each antacid neutralize hydrochloric acid. Procedure: 1. Obtain two burets‚ one for use with the HCl and others for use with the NaOH. 2. Record the exact molarity
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To investigate how does the concentration of Hydrochloric acid affect the rate of reaction? Outline I aim to discover how different concentrations of Hydrochloric acid influence the rates of reaction. In order to carry out this investigation I have decided to use marble chips‚ which I will vary the sizes as powder‚ small chips and large chips. I will also be changing the concentration‚ the different concentrations are as follows 0.2m‚ 0.5m‚ 1m‚ 1.5‚ 2m. I have chosen these concentrations as they
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Chemistry Lab Report Stoichiometry Design Experiment Percentage Yield of Calcium Carbonate and HCl I. Background Information When marble chips and hydrochloric acid are added together‚ they form sodium chloride‚ water‚ and carbon dioxide. This reaction can be displayed by the balanced equation below; CaCO3 (s) + HCl (l) NaCl(s) + H2O(l) + CO2 (g) As the carbon dioxide is formed‚ it will leave the open beaker as a gas. This will result in a loss of mass. The mass change can then be
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