pH Titration of Phosphoric Acid & Spectrophotometer Determination of the Percentage of Phosphoric Acid‚ in Cola Drinks (Experiment 23 & 24) Robbie Kinsey Partner: Debnil Chowdhury Chem. 1312-D TA’s: Russell Dondero & Sylvester Mosley Performed Feb. 16‚2000 Purpose The objective of this lab was to determine the concentration of phosphoric acid in cola through two different methods: a pH titration and a spectrophotometer
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Chemistry 101 12-STANDARDIZATION OF SODIUM HYDROXIDE Standard solutions for titrations are especially pure mixtures with exactly known concentrations. Primary standards are very pure solids. They have the advantage that they can be weighed (the analytical balance is normally the most accurate instrument in the laboratory) and they are stable under laboratory conditions. In this experiment‚ the primary standard is oxalic acid dihydrate‚ H2C2O4 ( 2H2O. It will be used to standardize a
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other is by dilution of a concentrated solution into the desired concentration. In diluting concentrated solution‚ the concentration of the diluted solution can be determined by standardization. To standardize a solution‚ we will need to perform titration. In this experiment‚ we will standardize acid and base solutions. In this experiment‚ the students to students will be able to know the proper way of preparing solutions from solid and liquid reagents by using the proper pieces of glassware and
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determine the percentage of calcium carbonate in eggshells. In this experiment‚ back titration is used. First‚ excess acid is reacted with the calcium carbonate in eggshells: 2HCl(aq) + CaCO3(s) → CaCl2(aq) + H2O(l)+ CO2(g) Later‚ if we can find out the number of mole of unreacted acid‚ number of mole of calcium carbonate can then be found out. The number of mole of unreacted acid can be found by titration with the following reaction: HCl(aq) + NaOH(aq) → H2O(l) + NaCl(aq) Percentage by mass
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The Royal and Pontifical University of Santo Tomas The Catholic University of the Philippines College of Education‚ Department of Food Technology Experiment #3 Food Toxicants FT 104 B Food Chemistry II Group 2 Submitted by: Collado‚ Dan Mark R. Eustaquio‚ Shekinah A. Isuga‚ Aedrian Lorenzo E. Luna‚ Maria Nikkita H. Santos‚ Kim Joshua C. Sombrano‚ Mary Chenneth S. Torres‚ Vincent Joseph P. Villaceran‚ Danielle P. Submitted to: Asst. Prof. Eufemio Barcelon Ph.D Submitted
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Quantitative Analysis of Soda Ash by Double Indicator Method Results and Discussion The experiment focuses in the use of double indicator titration in quantitative analysis of soda ash sample. Titration refers to the process of measuring the volume of titrant required to reach the equivalnece point. This method of analysis‚ is based on the chemical reaction aA + bB → products (1) where a is the molecules of the unknown substances to be analyzed or the analyte. Analyte reacts with b molecules
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DETERMINATION OF FRUIT ACIDS BY TITRATION AND CALCULATION OF THE SUGAR/ACID RATIO It is the sugar/acid ratio which contributes towards giving many fruits their characteristic flavour and so is an indicator of commercial and organoleptic ripeness. At the beginning of the ripening process the sugar/acid ratio is low‚ because of low sugar content and high fruit acid content‚ this makes the fruit taste sour. During the ripening process the fruit acids are degraded‚ the sugar content increases and
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| [Solubility Product Constant] | Experiment 11 | | Molly McCabe | 4/18/2013 | | Data Tables: Part 1 and Part 2 Experimental Data: Standard | Calculated volume of copper sulfate in standards | Absorbance values | Blank | 0.0 mL | 0.0 | 1 | 1.25 mL | 0.094 | 2 | 3.75 mL | 0.065 | 3 | 2.50 mL | 0.099 | 4 | 3.50 mL | 0.129 | 5 | 5.00 mL | 0.187 | Collected Data | Test tube 1 | Test tube 2 | Test tube 3 | Test tube 4 | Test Tube 5 | Initial volume (mL) | 0.05
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in water to give intense purple solutions. It reacts with reducing agents and gives colourless Mn2+ ions. So the solution itself acts as the indicator for the titration‚ the end point is noted when the first permanent pink colour appears. The sulphuric acid is used as a catalyst for the reaction. The oxalic acid is heated before titration because if the temperature is too low‚ the interaction between the acid and the potassium permanganate will move too slowly. Apparatus: 250cm3 conical
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Exercise 4 - Titrations and indicators 1. 20 cm3 of methanoic acid (Ka = 1.8 x 10-4 moldm-3) of concentration 0.10 moldm-3 is titrated against sodium hydroxide of concentration 0.05 moldm-3. a) Calculate the pH of the solution: i) initially ii) after 10 cm3 of the alkali has been added iii) after 20 cm3 of the alkali has been added iv) after 30 cm3 of the alkali has been added v) after 50 cm3 of the alkali has been added b) Sketch a pH titration curve
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