Specific Heat Lab Objective: Find the specific heat of the unknown metal given using calorimetry. Background Theory: In every reaction‚ energy is transferred between a system and its environment. A system encompasses the substances that are involved in a reaction‚ and everything else in the universe other than the system is called the environment. The standard SI unit of energy is Joules (J). Temperature is the level of excitement of the atoms in a substance. In most cases‚ energy is
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Experiment 3: Separating and Determining the Mass of Calcium Ion in a Calcium-Enriched Tablet In this lab‚ we dissolved a calcium-enriched tablet and participate the calcium ion as calcium carbonate. Our purpose is to determine the masses of calcium carbonate and calcium ion‚ to determine the mass percent of calcium ion in the tablet and to compare the masses and the percent with the listed tablet ingredients. This time we used a 150mL beaker‚ analytical balance‚ forceps‚ a 50mL graduated cylinder
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solution (Figure 9E). 3. Place the glass cover on the top of the Neubauer chamber so that it covers the central area. Note: in this step it is essential that the glass cover is tightly sticking to the Neubauer chamber. To guarantee this we slightly heat
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Results : Calculation : Part A Molecular weight of 1M of NaOH = 23g/mol + 16g/mol + 1g/mol = 40g/mol 1M = 40g/mol dissolved in 1L and 20g dissolved in 500ml 20g of NaOH was used to prepare 500ml of 1M NaOH. Part B Molecular weight of 1M of HCl = 35.5g/mol + 1g/mol = 36.5g/mol Specific gravity = 1.19kg/L 37% HC1 × 1.19kg/L = 0.44kg/L Convert w/v to mol/v = = 12mol/L = (12mol/L) = (1M)250ml = 20.83ml ≈ 21ml 21ml of concentrated HC1 is used to prepare 250ml of 1M of HC1. Part C For 0.1N of NaOH
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the test tube in a cold water bath. This reaction is very fast! (Instead‚ your teacher may tell you to run cold water over the outside of the test tube. Be sure to use a test tube holder to hold the test tube since the reaction gives off considerable heat.) The products forming in this step are hydrogen gas‚ H2(g)‚ aluminum chloride solution‚ AlCl3(aq)‚ and metallic copper‚ Cu(s). When the reaction is finished‚ remove and discard the liquid. Wash the solid with half a pipet of distilled water. Discard
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This lab was carried out by reacting a known amount of Mg with HCl in a eudiometer tube filled with water so that volume of the gas created would be measurable. The main purpose of the lab was fulfilled because for both trials the percent error was fairly low which means this lab was completed with a close eye to directions and held little error. The calculated results for the molar volume
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Post lab The unknown solution 4055 was tested by the separation scheme in order to identify the four cations that exist in it. The cations found were Ag+‚ Ba2+‚ Mn2+‚ and Ni2+. When I added 5 drops of 3M NaCl to the unknown solution‚ we had some precipitate‚ we centrifuge and then we divided to two test tubes‚ and they were put in hot water and got confirmatory tested. The Ag+ appeared to be in the solution because it melted‚ however Pb2+ didn’t. With the rest of the solution we added Na2SO4 we had
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In the first process of the lab‚ you measure the mass of water transferred from a buret to a beaker‚ to determine the experimental mass of the water‚ and the volume of the water collected. We measured the temperature of the water so we could calculate the density of the water‚ which enabled us to calculate the actual volume of water‚ by using the density and the measured volume of water. To determine the percent error‚ we had to subtract the actual volume of water by the experimental volume of water
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I. Objective: The objective of this experiment is to determine the mass percent of iron in an iron compound using a spectrophotometer. From there‚ determine which iron compounds are in the stock room bottles based off of the experimental mass percent results. II. Introduction: The objective is to determine the mass percent of iron in an iron compound using a spectrophotometer. From there‚ determine which iron compounds are in the stock room bottles based off of the experimental mass percent results
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Figure 1: Titration curve of 0.160 grams of an unknown diprotic acid that was dissociated in distilled water. Shown is the pH versus the volume in milliliters of 0.1 M NaOH‚ a strong base‚ added to the solution. The initial pH reading of the solution was a pH of 2.60. Although the pH of the ½ equivalence point was unknown‚ it could be estimated by halving the volume of NaOH used at the first equivalence point. At the first equivalence point‚ 13.63 milliliters of NaOH had been added to the unknown
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