up. By adding 100mL 6M HCl to 200mL deionized water‚ 300mL of 2M HCl solution was prepared. Then 150mL 2M NaOH solution was prepared by adding 100mL 3M NaOH to 50mL deionized water. Finally‚ the LabQuest was connected to the temperature probe‚ and set up to collect data every 15 seconds‚ the duration was set to be 180 seconds. In part B‚ three reactions were performed. In reaction 1‚ two Styrofoam cups were stacked together and placed in a 400mL beaker. Then 50mL of 2M HCl solution was added to the
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Data Table 1: Add 0.1M HCl Drops pH Paper Color 0 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 Data Table 2: Add 0.1M NaOH Drops pH Paper Color 0 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 Data Table 3: Add 6M HCl Drops pH Paper Color 0 1 2 3 4 Data Table 4: Add 6M NaOH Drops pH Paper Color 0 1 2 3 4 5 Data
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ACID BASE TITRATION OBJECTIVES 1. To demonstrate the basic laboratory technique of titration 2. To learn to calculate molarity based on titrations INTRODUCTION Molarity (M) or molar concentration is a common unit for expressing the concentration of solutions. It is defined as the number of moles of solute per liter of solution (or millimoles of solute per milliliter of solution). The concentration of a basic solution can be determined by titrating it with a volume of a standard acid solution (of
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Experiment 2 Title: preparation of a halogenoalkane Objective: To synthesis 2-cholo-2-methylpropane by using corresponding alcohol and HCl(aq). The reaction is via SN1 of tertiary alcohol. Techniques: i) Distillation of the reactant and the product ii) Purification by separating funnel Theory: In the experiment‚ SN1 reaction take place‚ HCl is added to initiate the reaction. The R-OH attack the H+ with the lone pair on O. Then the R-O+H2 bond breaks the release a water molecule and
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__________________________________ MATERIALS AND PROCEDURE As per Essential Experiments for Chemistry pages 163–170 RESULTS TABLE 1 Equilibrium involving bromocresol green Initial colour of bromocresol green in water = Reagent added HCl (step 3) more HCl (step 4) NaOH (step 5) more NaOH (step 6) Stress Colour change and # of drops required Direction of shift ver. 02/2012 1 Chemistry 12 Unit 2 Reaction Equilibrium TABLE 2 Equilibrium involving iron(III) thiocyanate ion Colour
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18.9 g 9. Percent acid or base in unknown 3.84 % 3.84 % 10. Manufacture’s claim 5.8 % 5.9 % 11. Percent deviation 23 % 23 % Table 3 Trial 1 Trial 2 1. Liters of Unknown‚ NaOH 0.020 L 0.020 L 2. Molarity of HCl 1.0 M 1.0 M 3. Liters of HCl used to titrate 0.0141 L 0.0154 L 4.
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important in determining whether a reaction will produce a precipitate. Starting out the experiment‚ HCl was added to the solution in the test-tube in order to form a reaction between the HCl‚ Ag‚ Pb‚ and Hg cations. The products of this addition of HCl were PbCl2‚ AgCl‚ and Hg2Cl2. After the HCl was added‚ the solution turned a milky white color. It was important to not add too much HCl because excess HCl would have caused an aqueous complex of PbCl2 and AgCl to form instead of the desired solid PbCl2
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Acid Base Titration Purpose: The purpose is to calculate the molarity of a NaOH solution by titrating the base with 5mL of standard HCl solution in each trial. By adding the base with unknown molarity to the acid with 0.10M the molarity of NaOH can be calculated. The base‚ NaOH‚ helps bring the pH of the acid‚ HCl‚ closer to seven‚ which neutralizes it. When using the buret the amount of NaOH used is able to be determined. Then by writing a balanced chemical equation and using the titration
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Exercise 14: Qualitative Anion Tests PURPOSE: The purpose of this experiment is to identify some commonly occurring anions & to study some of the reactions used for their identification. PROCEDURE: You must first determine to which of the three groups the various anions belong. Since no two people observe the same event in exactly the same way it is important to also conduct specific confirmation tests on the known samples of each anion. This information will help identify the anion
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