Making an Activity Series of Metals using different Solutions Purpose/ Hypothesis: The purpose of this lab was to clearly identify the reactivity of magnesium‚ zinc and copper. The metals reactivity will be exemplified as it will be tested with different solutions such as zinc sulfate (ZnSO4)‚ copper sulfate (CuSO4)‚ hydrochloric acid (HCL)‚ magnesium sulfate (Mg2SO4)‚ iron (II) sulfate (FeSO4) and tin (II) chloride (SnCl2). This will allow us in creating an activity series to visually see the reactivity
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Mohan 03-11-2013 Experiment: Chemical reactions‚ and Equations Materials: 3 mL of copper(II) sulfate solution. 5 mL of 6 M HCl piece of zinc wooden splint test tube Bunsen burner 3 mL of zinc chloride solution. pentahydrate distill water 0.1 g of ammonium
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decrease in oxidation state. If zinc completely reacts with HCL‚ then the theoretical yield of copper should be equivalent to the actual yield. Purpose: In this lab‚ we will determine the percent composition of a modern (post-1982) penny by using a strong acid to react and dissolve the zinc core‚ leaving only the copper coating. Once only copper remains‚ we will compare its mass to the entire mass of the penny to determine how much of a penny is copper and how much is zinc. Titration Experiment Day
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the solution of sodium chloride. Ans:- (i) BaCl2 (aq) + Na2SO4 (aq) →BaSO4 (s) + 2NaCl (aq) (ii) Sodium hydroxide solution (in water) react with hydrochloric acid solution (in water) to produce sodium chloride and water. Ans. (ii) NaOH (aq) + HCl (aq) → NaCl (aq) + H2O (liq) Q.4. A reaction of a substance X is used for white washing. (i) Name the substance X and write its formula. Ans.The substance X is lime which
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Evelyn Ramos CHEM LAB 201-003 Professor Ruddock Experiment #4 - Chemical Reactions Performed: 3/6/13 DUE: 3/13/13 Pre Lab Questions: 1. Before you can write a chemical equation‚ what must you know? You have to know what the products and reactants are. 2. What observations might you make that suggest that a chemical reaction has occurred? If a gas is produced or precipitates are formed that indicates chemical reaction. Also‚ if color changes occur or
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balloon. C. Single Replacement: Stand a clean and dry test tube on the test tube rack and add about 5mL of HCl. Carefully drop a piece of zinc metal and observe briefly. Quickly cover the test tube with a cork and after a minute‚ insert a lighted match on the mouth of the test tube. A “Pop” indicates the presence of hydrogen. Pour 5mL of CuSO4 in a clean test tube and add a piece of zinc metal. Let it stand in the rack for five minutes. Pour 5mL of CuSO4 in another test tube. Using a pipette‚ transfer
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series. Without it‚ cars or buildings could very well be rusting and dissolving around us. Metal/ Cation or Solution HCl H2O CuSO4 ZnSO4 MgSO4 SnCl2 Fe(NO3)3 Cu NR NR NR NR NR NR NR Mg R NR R R NR R R Sn R NR R NR NR NR NR Zn R NR R NR NR R R Fe R NR R NR NR R NR Steel (FeAl) R NR R NR NR R NR Table 1 : Predictions Metal/Cation Or Solution HCL Mg2+ H2O Cu2+ Zn2+ Fe2+ Sn2+ Cu Rusted‚ Less shiny No reaction No reaction bubbles bubbles tarnished No reaction
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may increase the actual mass of water in each trial. In the density part‚ the mass and density of zinc electrode was measured and calculated to determine the accuracy of the measurement. The result shows that the densities of zinc electrode in two trials are 6.2±1.6 g/cm3 and 9.4±3.8 g/cm3 (The average density is 7.8±3.8 g/cm3)‚ which is not quite accurate‚ compared to the standard of solid zinc density1 (7.14 g/cm3)1. The random error may result from the reading of volume of water in graduated
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Steel Purpose The goal of this lab is to determine the thickness of the coating of zinc on galvanized steel using the mass and volume of a sample of galvanized steel‚ and by using a larger mass; it is possible to minimize percent uncertainty. Reactions Molecular: Complete Ionic: Net Ionic: Oxidation Half Reaction: Reduction Half Reaction: Data and Calculations Density of Zinc: Density: Specifications of Galvanized Steel from Trial 1: 1.07cm x 1.51cm
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Research Question: Does the mass(±0.005g) of various types of corrosive metals (iron‚ nickel‚ zinc‚ copper and tin) change when placed in a solution of 1 molar hydrochloric acid over a period of 8 days at an average room temperature of 24 degrees Celsius? Aim: To be able to record and understand if and why a change in mass (±0.005g) occurs in various types of corrosive metals that include iron‚ nickel‚ copper‚ zinc and tin when placed in a solution of 1 molar concentration of hydrochloric acid over a period
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