This lab will investigate these affects on the rate of a specific reaction. Aim: How does the concentration of HCl affect the rate of the following reaction? CaCO3 (s) + 2HCl (aq) CaCl2 (aq) + CO2 (g) + H2O (l) Variables: Independent variable: Concentration of HCl Dependent variable: Amount of CO2 produced Controlled Variables: Temperature of the room‚ and the HCl No stirring or shaking of the experiment at any times The same type test tube should be used in each trial Try
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Standard Hydrochloric Acid Solution Abstract The aim of the experiment was how to determine the molarity of a solution. My hypothesis was if I have to determine the molarity of a NaOH solution‚ then I would have to use a standard solution of HCl solution because I would need to neutralize each other to determine the concentration of the solution of NaOH. The method that I used for this experiment was titration. Titration helped me achieved the result on figuring out the unknown molarity of
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Coleman Chem 3411 Dr. Eidell October 24‚ 2014 Preparation and IR Analysis of 2-chloride-2-methylbutane Line Reaction Abstract The purpose of this experiment was to react 2-methyl-2-butanol with concentrated HCl in order to form 2-chloride-2-methylbutane. The hydrogen for the HCl make the -OH from the 2-methyl-2-butanol into a good leaving group because H2O is formed. The H2O leaves and Cl- is free to bond with the carbocation creating 2-chloride-2-methylbutane. The materials needed for the
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Aim: To determine the effect of altering concentration (mol dm-3) of hydrochloric acid (HCl) on the rate of reaction (mol dm-3 s-1) for the following chemical reaction: CaCO3(s) + HCl(aq) CaCl2(s) + H2O(l) + CO2(g) Research question: How does altering concentration (mol dm-3) of hydrochloric acid (HCl) affect the rate of reaction (g/s) for the following reaction: CaCO3(s) + HCl(aq) CaCl2(s) + H2O(l) + CO2(g) Background information: The reaction between calcium carbonate and hydrochloric acid
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Hydrochloric acid (HCl). This one method of measuring the rate of reaction. We will use a balance to measure this mass loss as the reactants are used up to form product. Safety: * As Hydrochloric acid is corrosive wear a lab coat‚ gloves and safety goggles. * Take care when using the glassware not to cut yourself. * When the reaction is taking place Carbon dioxide gas is given off and it bubbles. Place a cotton wool stopper in the top of the conical flask to prevent any to the HCl splashing
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of a color indicator. We also learn about the standardization of bases (NaOH) and acids (HCl) which is basically making a dilution to change the molarity. The first reaction consists of titrating sodium hydroxide (NaOH) into potassium acid phthalate (KHP or K[HC8H4O4]): K+[HC8H4O4]- + Na+OH- => K+Na+[HC8H4O4]- + H2O The second titration we did was hydrochloric acid (HCl) with sodium hydroxide (NaOH): HCl(aq) + NaOH(aq) => NaCl(aq) + H2O(l) Procedure: You need to calculate the volume of 3 M
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|[pic] | | | | |UNIVERSITI TEKNOLOGI MARA | | | |FAKULTI KEJURUTERAAN KIMA | | | |CHEMICAL ENGINEERING LABORATORY III | | | |(CHE575)
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PROJECT REPORT ON “CASE STUDY AND SCOPE OF ENTERPRISE RESOURCE PLANNING (ERP) APPLICATION IN EDUCATION DOMAIN IN PUNJAB” SUBMITTED TO: PUNJAB TECHNICAL UNIVERSITY‚ JALANDHAR In Partial Fulfillment of the Requirement for the degree of Master of Business Administration SUBMITTED BY: PARAMPREET SINGH ROLL NO:-94302236209 MBA(2009-11) Under The Guidance of: ER. SHART SOOD CHANDIGARH BUSINESS SCHOOL LANDRAN (MOHALI) CERTIFICATE FROM PROJECT SUPERVISOR This is to certify
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Young people seeking training and education leads to surprising drop in unemployment figures (Martin Kornacki‚ 20 Jan 2010‚ Training journal‚ www.timesjournal.com) A surprising fall in UK unemployment figures has been attributed to increasing numbers of young people turning to training and education to avoid the dole. The Chartered Institute of Personnel and Development (CIPD) says the latest figure of 2.46m jobless for the three months to November‚ which is down 7‚000 on the figure for the previous
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Abstract By using acid-base titration‚ we determined the suitability of phenolphthalein and methyl red as acid base indicators. We found that the equivalence point of the titration of hydrochloric acid with sodium hydroxide was not within the ph range of phenolphthalein’s color range. The titration of acetic acid with sodium hydroxide resulted in an equivalence point out of the range of methyl red. And the titration of ammonia with hydrochloric acid had an equivalence point that was also out of
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