The Enthalpy of Formation of Magnesium Carbonate By: Jessica Miller T.A: Thomas Lab Partner: Rebekah Melanson Thursday Lab Room 106 Chemistry 1001-A Due Date: Thursday February 3rd 2011 Abstract The purpose of this experiment was to determine the enthalpy of formation of magnesium carbonate in a lab setting. This was done using a calorimeter‚ which was calibrated by adding a known amount of both hot and cold water. Following the calibration of the calorimeter‚ HCl was placed into the empty calorimeter
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BACK TITRATION- DETERMINATION OF THE CARBONATE CONTENT IN GARDEN LIME NAME: OSEI BONSU ERIC ID: 3906409 EXPERIMENT: I.2.2.1.
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Bio Cement The project aims at attaining high durability of concrete and gaining high strength of cement. We plan to make use of bacterial species which can hydrolyze the enzyme Urease efficiently to produce microbial concrete. Such bacterial are known to produce calcium which is useful in giving strength to cement. We are working in 2 stages. Stage 1: Here we check the effect of bacterial solution on cement mortar and along with that we check the effectiveness of the bacterial solution
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Vb = the volume of the base Cb = the concentration of the base Va = the volume of the acid Ca = the concentration of the acid n = the mole factor In the case of hydrochloric acid and Sodium Bicarbonate (Baking
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acid by heating an aqueous solution of maleic acid in the presence of hydrochloric acid. The hydrochloric acid serves as a catalyst of the reaction. The properties of two acids are then compared. Chemicals Maleic acid‚ magnesium ribbon‚ sodium carbonate‚ concentrated hydrochloric acid‚ bromine water‚ pH paper Apparatus 100cm3 and 250cm3 beakers‚ watch glass‚ apparatus for suction filtration (Büchner funnel and filter flask)‚ melting point apparatus‚ 25 cm3 measuring cylinder Procedures
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hydrochloric acid (HCl) with a pH of 2-3. When too much of this acid is formed in the stomach‚ heartburn and other discomfort occurs. This is when people grab for their antacids; these are bases that neutralize the excess acid in the stomach. Calcium carbonate‚ magnesium hydroxide‚ and aluminum hydroxide are all examples of bases used in antacids. In addition to these active ingredients‚ antacids also contain sweeteners‚ colourings‚ and “fillers” that may or may not affect the effectiveness of the neutralization
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INTRODUCTION Sodium hypochlorite is considered one of the most efficient irrigant in endodontics 1-4. Due to its antimicrobial‚ tissue dissolving properties and low cost‚ it is one of the most widely accepted irrigant in Endodontic practice 5-8. Sodium hypochlorite as a solution is relatively an unstable compound. On exposure to organic compounds‚ heat‚ light‚ air and metals‚ the available chlorine ions reduce and there is subsequent loss of tissue dissolving and antimicrobial properties 9-10. Recent
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A1 NaHCO3 SodiumBicarbonate HCl Hydrochloric Acid Bubbles yes A2 NaOCl Sodium-Hypochlrite Kl Potassium Iodide Observation 1: None Add 2 drops of solution Observation 2: Solution turned blue Yes A3 Kl Potassium Iodide Pb(NO3)2 Lead Nitrate Turned Yellow Yes A4 NaOH Sodium Hydroxide C20H14O4 Phenolphthalein Turned pinkish red (magenta) Yes A5 HCl Sodium Hydroxide C20 H14 O4 Phenolphthalein Turned Cloudy Yes A6 NaOH Sodium Hydroxide AhNO3 Silver Nitrate Turned Brown Yes B1 AgNO3 Silver Nitrate
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Baking Soda (NaHCO3) Lab (Stoichiometry) - Physical Science Name: __________________________________________________ Purposes: 1. Calculate theoretical mass of NaCl based on a known mass of NaHCO3. 2. Experimentally determine the actual mass of NaCl produced. 3. Calculate the percent yield for your experiment. Reaction Equation: NaHCO3(s) + HCl(aq) ( NaCl(s) + CO2(g) + H2O(l) Materials: safety glasses baking soda (NaHCO3) 1 M HCl and
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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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