of soil to ensure that all the site is safe‚ not just a small area where you would have taken your first sample from. I will return to the lab with the samples of soil I have extracted from the site. Here I will make a solution from the samples in order to carry out the identification tests. In order to turn my soil samples
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carboxylic acids and alcohols with the presence of a catalyst. A carboxylic acid contains the -COOH group‚ and in an ester the hydrogen in this group is replaced by a hydrocarbon group of some kind. Sulfuric acid (H2SO4)is used as a catalyst for this reaction in order to accelerate the rate at which the product is formed. The general formula of an ester is RCOOR’ in which R is the alkyl group that comes from the carboxylic acid while R’ is the alkyl group that comes from the alcohol and COO is the functional
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It must be noted that the actual undertaken procedure included a few differences from the ideal protocol. A total of 7 ml of extra water was added to the reaction before it was treated in the separatory funnel due to there being so much white precipitate that the mixture had turned to a paste as opposed to a liquid. The aqueous layer was accidentally not drained between adding the two different ether fractions‚ so the aqueous layer was drained after that and 10 ml of extra diethyl ether were added
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Introduction In a Grignard reaction‚ a Grignard reagent (R–MgX) adds to the carbonyl group in an aldehyde or ketone to form an alcohol (Figure 1). The reaction of a Grignard reagent with formaldehyde can be to synthesize a primary alcohol‚ with any other aldehyde can be used to synthesize a secondary alcohol‚ while the reaction with ketone is useful in the synthesis of a tertiary alcohol. Figure 1. General reaction mechanism of a Grignard Reaction The preparation of the Grignard reagent involves
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CHEMICAL REACTIONS OF COPPER AND PERCENT YIELD Objective To gain familiarity with basic laboratory procedures‚ some chemistry of a typical transition element‚ and the concept of percent yield. Apparatus and Chemicals |0.5 g piece of no. 16 or no. 18 copper wire |evaporating dish | |250 mL beaker (2) |weighing paper | |concentrated HNO3 (4 – 6 mL)
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All chemical reactions are processed through energy exchanges. Chemical reactions either absorb energy or release energy into their surroundings. In thermodynamics‚ endothermic reactions absorb energy where exothermic reactions release energy. In this experiment‚ we will be observing the chemical reactions that occur when a specific liquid is combined with a specific solid. We will measure the temperature of the liquid before the solid is added. Then we will measure the temperature of the liquid
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Joanna Park Mrs. Carrillo CP chemistry per. 5 September 17‚ 2012 i. Beverage Density Lab Report ii. Purpose: The purpose of this experiment is to determine the percentage of sugar content in beverages. iii. Materials: Distilled water‚ beverages (juice‚ soda‚ sport drinks)‚ Sugar reference solutions (0‚ 5‚ 15‚ ad 20%) 25ml each‚ Balance‚ centigram(0.01g precision)‚ Beaker (100-mL)‚ Erlenmeyer flask (125-mL to collect rinse solutions)‚ Pipet(10-mL)‚ Pipet bulb or pipet filler iv
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JOMO KENYATTA UNIVERSITY OF AGRICULTURE AND TECHNOLOGY DEPT: CIVIL ENGINEERING UNIT: CHEMISTRY 1 (SCH 2109) PRACTICAL REPORT EXPT 2: Standardization and Determination of Concentration of Hydrochloric Acid in a Given Solution by ARAKA BRAMWEL MBOGO EN251-0221/2010 TITLE: STANDARDIZATION and DETERMINATION OF THE CONCENTRATION OF HYDROCHLORIC ACID PRESENT IN A GIVEN SOLUTION Aims: To be able to standardize Sodium Hydroxide (NaOH) solution using a standard solution of Oxalic acid
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original state and the percent of the hydrate recovered was calculated by using the mass of the rehydrated sample by the mass of the original hydrate and then multiplied by 100%. Data Presentation & Analysis Table 1: The data was collected from the lab experiment. Sample calculations are shown. Mass of beaker with sample 30.765g Mass of empty beaker 30.263g Mass of sample .502g Mass of beaker with sample after 1st heat 30.661g Mass of beaker with sample after 2nd heat 30.657g Heating mass
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Experiment 12: Calorimetry and Hess’s Law Purpose: The purpose of this lab is to determine the enthalpy of reaction for the burning of one mole of magnesium in oxygen. Although the reaction is exothermic‚ the ∆HRXN will be determined by using calorimetry and then using Hess’s Law to manipulate the data collected to yield the answer needed. Procedures: Dillon‚ Stephanie. “ Calorimetry and Hess’s Law.” Laboratory Manual. Pearson Publishing‚ 2012‚ pp.168-177. Data and Results Part A
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