instructions provided‚ no changes were made to the procedure. Data: Part A: Trial 1: Amount of H C O 2H O: 0.96 g Buret before titration: 3.6 mL Buret after titration: 32.5 mL Trial 2: Amount of H C O 2H O: 0.095 g Buret before titration: 3.0 mL Buret after titration: 31.9 mL Part B: Unknown acid # 310 Trial 1: Amount of unknown: 1.001 g Buret before titration: 1.4 mL
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Despite following rigorous experimental procedures‚ there are limitations that exist‚ but were not addressed due to insufficient time and limited resources to carry out the experiment. Firstly‚ varying the length of boiling might not be the best method to determine the amount of calcium ions. If time permits‚ I could perhaps investigate other variables such as pH‚ surface area and concentration and their effect on calcium leaching. Moreover‚ I could also use other types of fish soup stocks and compare
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meniscus shows the measurement line. Usually‚ the surface of the solution will form a curve known as meniscus. Typically the accuracy of the measuring cylinder is +/- 0.05mL. A burette is a vertical cylindrical piece of laboratory glassware with a volumetric graduation on its full length and a precision is necessary. It is accurate and has a tolerance of 0.1cm3. A pipette is used to transport a measured volume of liquid. Its accuracy is 0.5mL.
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containing your own data and the other containing the class data. 2. The liquid in this experiment that is flammable as well as poisonous is Methanol. 3. The two variables that will be being measured are mass and volume. To measure the volume‚ a buret and 250mL Erlenmeyer Flask. To measure the mass‚ a scale and an Erlenmeyer Flask will be used. 4. It is important to the class that accurate results are obtained because a class data graph will be made after all the data is recorded. Objectives
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so as to check the feasibility of the idea behind the development of automated system for the measurement of pH and to have enough confidence in performing future experiments and also to check the response of the interface towards the pH change. Calibration was performed before the start of the each experiment so as to calibrate the LabVIEW program against the value of mV generated by the probe per value of pH. After the end of the experiments‚ the observed changes in the value of pH during the experiment
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using potassium hydrogen phthalate (KHP) III. When given whether the acid is monoprotic‚ diprotic‚ or triprotic ‚ determine the molar mass of the unknown organic acid. IV. Calculate the Molarity of the Soft drink. Materials: * 50 mL Buret * Beaker * Erlenmeyer Flask * Sodium Hydroxide * Water * Balance * Unknown Acids
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Experiment 20: pH Titration: Phosphoric Acid in Cola Drinks Post-lab Assignment or Report The post-lab report for this experiment is due at the beginning of the following lab period. Student notes for the lab will be available on the lab T-Square site. Learning Objectives Students will be able to... • Use a known mass of solid acid to determine an unknown concentration of a basic solution (this process is called “standardization”). • Execute a titration using good‚ reliable technique.
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of water with 4.2 mL of 19.1 M NaOH‚ the diluted solution of NaOH was poured in a buret until the initial volume on the buret was 30.00 mL. 0.3005g of KHP was dissolved in 40.0 mL of 50% ethanol‚ and a drop of indicator was added to the Erlenmeyer flask containing the KHP solution. When the titration of KHP solution with NaOH reached its endpoint‚ pale pink color was observed‚ the final volume of NaOH in the buret‚ 45.00 mL‚ was recorded. Based on the data obtained and the equivalent weight of KHP
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Not enough added‚ wouldn’t kill the microorganisms in the water to make it safe to drink. II. Procedure First the standardization of Sodium Thiosulfate was completed. A 50mL buret was obtained and rinsed twice with the sodium thiosulfate solution. It was then filled with the solution. The tip of the buret was checked to make sure there weren’t any bubbles in it. Then a 250mL beaker was obtained. A 25mL pipette was used to add exactly 25mL of the KIO₃ solution. Then 50mL of deionized
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management‚ e.g. chemical‚ biological; ordering procedures; calibration of equipment‚ e.g.pH meters‚ graduated pipettes; maintaining equipment‚ e.g. burettes and Bunsen burners; collection/transport of substances and equipment for disposal; use of centrifuges; instrumentation techniques‚ e.g. colorimeter‚ electrophoresis; desiccators and vacuum storage; handling and disposal of radioactive substances; handling and use of glassware; handling of solvents and poisons;
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