mx + b which would be attained from a calibration curve. And Beer Lambert law: . Experimental Procedures To prepare the standard iron solution weighed 0.0351 g of ferrous ammonium sulfate and added 1.25 mL of sulfuric acid. We added distilled water to make 500 mL. We dissolved 0.1005 g of 1‚10-phenanthroline in a 100 mL volumetric flask. We then prepared 25 mL hydroquinone solution containing 0.2510 g of hydroquinone. In a 250 mL volumetric flask 6.2515 g of sodium citrate was
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EXPERIMENT 10 Volumetric Analysis I Standardization of NaOH Solution Outcomes After completing this experiment‚ the student should be able to: 1. 2. 3. 4. Demonstrate the concept of quantitative analysis. Make solution and standardize it. Explain the difference between primary and secondary standard solutions. Quantitatively determine the concentration of a base. Introduction Titration is a common method of quantitative analysis used to determine the concentration of an unknown substance in a solution
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acetic acid in vinegar by titration with sodium hydroxide to a phenolphthalein endpoint. This procedure may be modified by titrating an acidic beverage such 7-up or Sprite. Equipment and Material (Total Time 60 – 90 min.) Variety of Berel Pipet Long glass stirring rod Wash bottle 10-mL graduated cylinder 100 mL beakers Material NaOH‚ Sodium hydroxide Titrant solution White vinegar phenolphthalein Distilled water Discussion Acetic acid (CH3COOH) is the chemical compound which
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Introduction: Density is defined by its mass per unit volume‚ and is most often written in mathematical terms as; d = m / v Mass is usually given in grams‚ g‚ and volume is given in cubic centimeters‚ g/cm3‚ or‚ grams per milliliter‚ g/mL. Density is not a property that depends upon the amount of substance present. For example‚ one gram of lead and one ton of lead have the same density. Density also does depend on temperature. For instance cold water is denser than warm water;
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accuracy of scientific glassware. I figured the smaller the glassware the more accurate the measurements would be. Which when we were preforming the experiment proved my theory. As the glassware got smaller the easier it was to get the accurate amount of water into the glassware. We went from a big flask to a small beaker to an even smaller pipette. We used a scale to get the appropriate weight of the water in the different beakers. To test this‚ we weighed multiple glassware and different sized
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Nitric Acid * 0.5M Copper sulfate – sulfuric acid mixture * 0.1M Sodium hydroxide * Acetone * Distilled water The apparatus used were the following: * Phywe Transference Number Apparatus * Analytical Balance * Buret * Beaker * pipet The experiment starts off with the preparation of the set-up for the transference vessel. Fill the double U-tube with 0.1M Nitric acid. The double U-tube should be filled to the same level in the three legs even after the electrodes were
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at the electrophilic trimethylcarbocation. The resulting product will be recrystallized using methanol and characterized using TLC and melting point analysis. Materials: 400-mL beaker‚ ice for ice bath‚ 25 mL Erlenmeyer flask‚ several volumetric and Pasteur pipets‚ 1.0-mL 10 x 100 mm reaction tube‚ glass stirring rod‚ rubber bulb‚ TLC plate Table 1. Chemicals used in Friedel Crafts synthesis of 1‚4-di-t-butyl-2‚5-dimethoxybenzene Substance Molecular Weight (g/mol) Amount Used Moles Used Mole Ratio
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Determination of Formation Constant‚ Kf of Thiocyanoiron(III)‚ FeSCN+2 Dr. Fred Omega Garces Chemistry 201 Miramar College Chemical Equilibrium: Finding the Formation Constant of FeSCN2+ (aq) Fe3 +(aq) iron(III) + SCN–(aq) FeSCN2+(aq) D thiocyanate thiocyanoiron(III) kf = € FeSCN2 + [ ] Fe +3 [SCN− ] [ ] Objective The purpose of this experiment is to determine the constant formation‚ Kf‚ (equilibrium constant) for the formation of thiocyanoiron(III)
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CHEMISTRY 205 REDOX TITRATIONA. Purpose: • To learn some technique in volumetric analysis: Redox titration. • To review the stoichiometry of an oxidation- reduction reaction. • To determine the concentration of an unknown sodium oxalate (Na2C2O4) solution by titrating it against standardized potassium permanganate solution (KMnO4). • To determine the percent by mass of Fe(II) in the form of ferrous ammonium sulfate Fe(NH4)2(SO4)2.6H2O in a mixture by
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[pic] [pic] Florida A&M University Department of Chemistry CHM 1045 Lab Syllabus | COURSE SYLLABUS | |Course Number: CHM 1045L |Course Title: General Chemistry I Laboratory | |Prerequisite(s):
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