Illinois Central College CHEMISTRY 130 Laboratory Section: ________ Page 1 Name ______________________ Evaluation of the Gas Law Constant Objectives In this experiment‚ we will determine the Ideal Gas Constant‚ R‚ which relates the number of moles of gas present to its volume‚ pressure and absolute temperature. Background To see how "R" was derived‚ we must look at the proportionalities defined by the other fundamental gas laws. For example‚ Charles’ Law showed us that the volume of a gas sample
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Analysis of a Commercial Bleach Purpose: The purpose of this lab is to determine the amount of sodium hypochlorite (NaClO) in commercial bleach. This can be done by forming triiodide ions. To make the measurement more accurate‚ starch was added to help determine the endpoint of the solution. The significance of this lab is that industry can use these techniques to determine the amount of NaClO in the bleach of the rival industry and improve it. Hypothesis: The hypothesis is that‚ an accurate
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Preparation of Aspirin The purpose of this experiment is to synthesize aspirin (acetyl salicylic acid) from salicylic acid and acetic anhydride. CO2H OH salicylic acid 2g 0.014 mole O O O CH3 H2SO4 ethyl acetate CO2H O O acetyl salicylic acid acetic acid CH3 O + H3C + H3C OH acetic anhydride 5 mL 0.05 mole The limiting reagent is salicylic acid. The theoretical yield of acetyl salicylic acid is 2.52 g. Physical Data:* mp MW salicylic acid 157-9˚ 138 acetyl salicylic acid
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Sunny Ng Wing Lam G10L (20) Chemistry A Lab 10.2 Determining the Concentration of Ammonia in Window Cleaner Solution Design (D) Aim To determine the concentration of ammonia‚ NH3‚ in the commercial window cleaner solution Background Window cleaner contains ammonia‚ NH3‚ a weak base‚ which helps remove dirt from glassware. The concentration of ammonia in the window cleaner solution varies by brands. Titrating the window cleaner solution with an acid of known concentration allows us
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Synopsis: The main aim of the experiment is to find out the amount of calcium carbonate in toothpaste through back titration since calcium carbonate does not dissolve in water. A roughly weighed amount of calcium carbonate is mixed with hydrochloric acid and then titrated against sodium hydroxide. When the indicator turns from pink to orange‚ the volume of sodium hydroxide used is taken down. After doing some calculations‚ the average percentage of calcium carbonate in toothpaste is 19.2%. This average
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the product this reaction produce dependent on the limiting reactant. For example‚ 1000kg O2 and 1 gram H2 to form water. In this case‚ the 1 gram of H2 will be the limiting reactant. Same thing in displacement reactant. If one of the reactants is (Mole) less than the other one‚ then that reactants becomes the limiting reactants. Once the limiting reactants will completely be ran out of‚ the reaction is done. So the limiting reactant is the key to start and finish the chemical reaction. B. Procedures
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Topic 2 METALS What is this topic about? To keep it as simple as possible‚ (K.I.S.S.) this topic involves the study of: 1. OUR USE of METALS 2. CHEMICAL ACTIVITY of the METALS 3. PATTERNS of the PERIODIC TABLE 4. QUANTITY CALCULATIONS... the MOLE 5. METALS from their ORES ...all in the context of how Chemistry contributes to cultural development but first‚ an introduction... Chemistry of the Metals Technology Needs Metals In the previous topic you learnt about the Elements of the
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is negligible) (915.141 g) 4. A mixture of noble gases contains 4.46 moles of Neon and 0.74 moles of Krypton and y mole of Xenon at a pressure of 2 atm. (a) Determine y mole of Xenon if the partial pressure of Neon is 1.214 atm. (2.148 moles) (b) Determine the partial pressure of Krypton. [Sep 2014] (0.2 atm) 5. Calculate the number of moles of sulfur dioxide gas‚ SO2‚ transported in a 2 L container at s.t.p. (0.089 mole) 6. Water has a vapour pressure of 24 mm Hg at 25 °C and 182 mm Hg at
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The aim of this experiment was to calculate the concentration of an unknown solution of Sodium Hydroxide (NaOH) by titrating it with Hydrochloric Acid (HCl) and to identify any possible sources of error. A colour change from pink to yellow signified the end of each individual titre as the NaOH had been neutralised. Experimental: Method: Firstly two solutions were prepared to show the colour of the Phenol Red indicator in acid and alkaline conditions. These colours were then used to determine the
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the solution is raised. Thus‚ a 0.1 M acetic acid solution has a pH of 2.87 but a solution of 0.1 M acetic acid and 0.1 M sodium acetate has a pH of 4.74. Thus 4.74 is the pH of the buffer. On addition of 0.01 mole NaOH the pH changes from 4.74 to 4.83‚ while on the addition of 0.01 mole HCl the pH changes from 4.74 to 4.66. Obviously the buffer solution maintains fairly constant pH and the changes in pH could be described as marginal. Buffer Action: A buffer solution containing equimolar
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