Observations Part I: Equilibrium Involving Thymol Blue Table 1 Reagent Added | Stress (Ion Added) | Colour Observation | Direction of Equilibrium Shift | NaOH (Step 5) | OH⁻ | Green | Left | NaOH (Step 6) | OH⁻ | Blue | Left | HCl (Step 3) | H⁺ | Green | Right | HCl (Step 4) | H⁺ | Yellow | Right | Part II: Equilibrium Involving Thiocyanatoiron (III) Ion Table 2 Reagent Added | Stress (Ion Added) | Spectator Ion | Observation | Direction of Equilibrium Shift | KCl | None | K⁺‚ Cl⁻ |
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To learn how to measure the volume of a liquid using a buret. Prelab Questions: 1. Calculate the number of moles in 2.65g of zinc. 2. Calculate the number of moles of hydrochloric acid in 37.5mL of a 3.00M HCl solution. 3. Calculate how many moles of HCl are required to react with 0.244 moles of zinc. Procedure: 1. Put on safety equipment. 2. Label small glass vial so your group can identify it later. 3. Determine the mass of the clean dry vial and record
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Chemistry Lab Report Stoichiometry Design Experiment Percentage Yield of Calcium Carbonate and HCl I. Background Information When marble chips and hydrochloric acid are added together‚ they form sodium chloride‚ water‚ and carbon dioxide. This reaction can be displayed by the balanced equation below; CaCO3 (s) + HCl (l) NaCl(s) + H2O(l) + CO2 (g) As the carbon dioxide is formed‚ it will leave the open beaker as a gas. This will result in a loss of mass. The mass change can then be
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instructor. III. Pre-lab Questions 1. Define ΔHrxn. ΔHrxn is enthalpy of products – reactants. (ΔHrxn = Hprod-Hreact). 2. In today’s lab you will be using 50.0 mL of 2.0 M HCl. Using Equation 3 (M=mol/L) from above‚ calculate the number of moles of acid used. M=mol/L 2.0M = x / 0.0500L x = 0.10 mol HCl 3. You will also be using 50.0 mL of 2.0 M NaOH. How many moles of base are used? M=mol/L 2.0M = x / 0.0500L x = 0.10 mol NaOH 4. The specific heat of a solution is 4.18 J/g
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Deborah Bell April 17‚ 2012 Chemistry 1212K Lab Synthesis Report Introduction In this Chemistry Lab the main objective is to perform accurate chemical analysis for the quantity of elements and compounds in a sample. There will be a compound made then synthesized. The methods used were acid-base titrations‚ redox titrations‚ gravity filtration‚ and distillation. General conclusions included Procedures Weight of Crucibles 1. The first experiment is Preparation of a Cobalt Amine
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Introduction: The students were handed 10 test tubes with no identification. The students were supposed to design a method in determining what chemical was in each test tube. The list of chemicals is CuSO4‚ NH4Cl‚ NaOH‚ AgNO3‚ KI‚ H2SO4‚ NaBr‚ CaCl2‚ HCl‚ and Pb(NO3)2. The students are expected to determine the chemicals using physical properties‚ litmus paper‚ solubility‚ and the process of elimination. Physical properties‚ such as the color‚ can be determined by sight. Litmus paper can be determined
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Joseph Corey‚ Chris‚ Grant Thermodynamics – Enthalpy of Reaction and Hess’s Law I. Purpose The purpose of this lab is to verify Hess’s Law through the three reactions of NaOH and HCl‚ NH4Cl and NaOH‚ and NH3 and HCl. The sum of the enthalpies of the first two reactions should equal the enthalpy of the third reaction. II. Background Hess’s Law is used to determine the enthalpy of a reaction from adding two or more preceding reactions. To determine the enthalpies of certain
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reaction 2 HCl(g) +I2(s) [pic] 2 HI (g) + Cl2(g) has Kc = 1.0 x 10-34 at 25˚C. If a 1.00 L reaction vessel initially contains 0.100 mol of each HCl and solid I2‚ what are the concentrations of HI and Cl2 at equilibrium? 2. Consider the following gas-phase reaction and equilibrium constant at 25 oC: 4 HCl(g) + O2(g) [pic] 2 Cl2(g) + 2 H2O(g) The concentrations of all species were measured at a particular moment in time and the following data were obtained: [HCl] = 0.00050
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metals included in the lab. Materials: Apparatus Test-tube rack 4 test tubes (25 mm x 150 mm) 4 beakers (150 mL) Safety goggles Lab apron Plastic gloves Full face shield Reagents Zinc Magnesium Iron Copper 1M hydrochloric acid‚ HCl 1M sulphuric acid‚ H2SO4 1M acetic acid‚ HC2H3O2 1M phosphoric acid‚ H3PO4 Procedure: Please refer to Health Chemistry‚ Laboratory Experiments‚ page(s) 75-76. Data and Observations: Table 1: Comparison of Metal Activities Zinc
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electrolyte‚ HCL‚ NaOH‚ NH4CL‚ NaC‚ conc.H2SO4; it contains a highconcentration of ions and so the bulb glows brightly. Introduction Substances that dissolve in water are either nonelectrolytes or electrolytes. Non-electrolytes are substances that do not form ions and are electrically non-conducting in solution. A common example is table sugar (sucrose) which dissolves in water as shown in Equation 1. Electrolytes are substances‚ such as NaCl and HCl‚ which form
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