Titrations D1 Laura Andrijaityte Chemistry Assignment BTEC Forensic Science Titration definition: A measured amount of solution of unknown concentration is added to a known volume of a second solution until the reaction between them is complete; the concentration of the unknown solution (the titre) can then be calculated. Acid based titration: determination of the concentration of an unknown acid or base by neutralizing the acid or base with an acid or base of a known substance. Redox
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Co(acac)3 + 2 C2H3O2NO2 ( 2/3 Co(acac-NO2)3 + 2 C2H3O2 • Moles of reagent used - Cu(NO3)2·3H2O‚ MW: 241.59 g/mol [pic] - Acetic anhydride‚ MW: 102.1 g/mol‚ D: 1.080 g/mL [pic] - Co(acac)3‚ MW: 356.24 g/mol [pic] • Limiting Reagent From the stoichiometry of the reactions‚ acetic anhydride is in excess‚ and 2/3 (0.67) mole Co(acac)3 should reaction with 1 mole copper nitrate trihydrate. The actual mole ratio when 0.49 g Co(acac)3
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Turkish Journal of Agriculture and Forestry http://journals.tubitak.gov.tr/agriculture/ Research Article Turk J Agric For (2014) 38: 55-61 © TÜBİTAK doi:10.3906/tar-1212-4 Oxidative stress and antioxidant defense mechanism in mung bean seedlings after lead and cadmium treatments Meher HASSAN‚ Simeen MANSOOR* Department of Genetics‚ University of Karachi‚ Karachi‚ Pakistan Received: 02.12.2012 Accepted: 25.05.2013 Published Online: 13.12.2013 Printed: 20.01.2014 Abstract:
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EXPERIMENT 1 “HOW DO I LOVE THEE LET ME COUNT THE WAYS...” DETERMINATION OF AVOGADRO’S CONSTANT Techniques Calibration drop counting MSDS available for • • stearic acid‚ CH3(CH2)16COOH cyclohexane‚ C6H12 Principles molar volume molecular structures surface areas and volumes Avogadro’s constant percent error Recommended Advanced Reading Chapter 3 in Petrucci‚ Herring‚ Madura‚ & Bissonnette’s General Chemistry‚10th Ed. Avogadro Constant...1 INTRODUCTION
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DETERMINATION OF THE SOLUBILITY PRODUCT CONSTANT OF CALCIUM HYDROXIDE ABSTRACT This experiment aimed to determine the solubility product constant (Ksp) of Ca(OH)2 as well as to evaluate the effects of common and non-common ions on its solubility. Ca(OH)2 solids were dissolved in eight various media: distilled water‚ 1.0 M KCl‚ 0.5 M KCl‚ 0.1 M KCl‚ 0.05 M KCl‚ 0.005 M KCl‚ 0.001 M KCl‚ and 0.1 M Ca(NO3)2. The concentration of dissociated OH- concentrations was determined by means of titrimetric
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sodium chlorite‚ NaClO2; sodium hypochlorite‚ NaClO; and sodium chloride‚ NaCl. All are white solids at room temperature. It is possible to determine the chemical equation for the decomposition of sodium chlorate by applying the principles of stoichiometry to the masses of the reactants and products. Safety Precautions: Sodium chlorate is a strong oxidizing agent and a dangerous fire risk; it is slightly toxic by ingestion. Contact with metal powders or combustible organic compounds may cause
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mCn Hm + (n +m/4)O2 = nCO2 + m/2 H2O + Q S + O2 = SO2 + 9260 kJ/kg of sulfur Calcination CaCO3 = CaO + CO2 – 1830 kJ/kg of CaCO3gCO3 = MgO + CO2 – 1183 kJ/kg of MgCO3. Sulfation CaO + SO2 + 1/2 O2 = CaSO4 + 15141 kJ/kg S. Basic Stoichiometry C + O2 = CO2 + q 1 kmol of carbon combines with 1 kmol of oxygen to produce 1 kmol of carbon dioxide and release q amount of heat. 1 kmol of reactant = M kg of the reactant when M is the molecular weight of the reactant. So mass
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Synopsis The objective of this experiment is to determine the percentage by mass of calcium carbonate‚CaCO3 in toothpaste using back titration technique. A known weight portion of toothpaste is obtained to react with known volume and concentration of standard acid solution. After completing the reaction‚ the resulting solution containing excess acid is back titrated with known volume and concentration of standard base solution. Determination of excess acid after reaction allow us to calculate the
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MAC1105 CO-REQUISITES: CHM1045L Upon successful completion of this course‚ the students should be able to demonstrate a familiarity with introductory material in general chemistry such as units for measurement‚ formula writing and nomenclature‚ stoichiometry‚ atomic structure‚ periodicity and bonding‚ terms and problem solving in the areas of changes of state‚ acid and base chemistry‚ ionic reactions‚ oxidation-reduction reactions‚ solutions and descriptive chemistry of selected non-metals. The students
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potassium iodide. The reaction will release iodine:Example: (a) With KMnO4 2MnO4- + 16H+ + 10I(b) With KIO3 IO3- + 5I+ 6H+ 3I2 + 3H2O 2Mn2+ + 5I2 + 8H2O The iodine that is released is titrated against a standard thiosulphate solution. From the stoichiometry of the reaction‚ the amount of iodine can be determined and from this‚ the concentration of the oxidising agent which released the iodine‚ can be calculated. In an iodometric titration‚ a starch solution is used as an indicator as it can absorb
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