Procedure: Within this experiment‚ we used two 50mL burets‚ distilled water‚ 10mL graduated cylinder‚ vinegar (acetic acid‚ HC2H3O2)‚ phenolpthalein and 2 flasks of 125mL and 250mL. With using these materials‚ we first determine the titration of base unknown concentration. Using a buret‚ we allowed the buret to fill with the NaOH solution and it gained the initial volume of 5mL. After doing this‚ we read the initial and the final volume of the buret after the 10.0mL of acid was added. Then‚ three drops
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solution. In relation to this method was the so called principle‚ the Beer-Lambert’s Law‚ which was used in getting the relationship of the absorbance and the concentration with one another. Then from the data gathered absorbance and concentration‚ a calibration curve was made and the equation of the line was determined. The absorbance of an aliquot of unknown copper-ammonia complex solution was then gathered in triplicate and its concentration was determined by the use of the equation determined earlier
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with 20mL of 6M HCl in a 150mL beaker. A 1.5g piece of Alka-Seltzer was added to this mixture and all CO2 was allowed to escape. The mixture was filtered then added to a 50mL buret until full. The glass tube end of the rubber tubing was inserted about 2 inches in to the buret. Using a finger to cover the mouth of the buret‚ it was quickly inverted and placed into the water in the 600mL beaker. The water level was brought to 50mL by carefully adjusting the stopcock. 25mL of the prepared HCl solution
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potentials are positive which means that they are spontaneous‚ as directly observed. There is also a percent difference from the theoretical and experimental cell potentials. The sources of error are also incorrect solution preparations‚ contaminated glasswares and materials‚ and the resistance of the electrodes. Keywords: cell potential‚ half-cell‚ electrode potential‚ oxidation-reduction reactions‚ standard electrode potential Introduction Chemical reactions can be used to produce electricity and
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accurately known concentration. Titration is a common laboratory method of quantitative chemical analysis that is used to determine the unknown concentration of an identified analyte.¹ Titrant means substance with known concentration existing in buret‚ analyte means substance with unknown concentration in erlenmayer and indicator means chemical which is used to observe acid-base reaction.² In this investigation‚ titrant is NaOH‚ analyte is HCl and indicator is phenolphtalein. Figure 1: Setup
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moles of each reactant. 3. To predict which reactant is in excess. 4. To use drawings to relate microscopic events‚ to write a chemical equation that represent those microscopic events. 5. To learn how to measure the volume of a liquid using a buret. Prelab Questions: 1. Calculate the number of moles in 2.65g of zinc. 2. Calculate the number of moles of hydrochloric acid in 37.5mL of a 3.00M HCl solution. 3. Calculate how many moles of HCl are required to react with 0.244
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Oxygen in Liquids (DISSOLVED OXYGEN) Dissolved Oxygen – the amount of dissolved oxygen in a body of water as an indication of the degree of the health of water and its ability to support a balanced aquatic ecosystem. Oxygen – is a clear‚ colorless‚ odorless‚ and tasteless gas that dissolves in water. Small but important amounts of it are dissolved in water. OXYGEN: Aquatic Life Depends on it Plants and Animals depend on dissolved oxygen for survival. Lack of dissolved oxygen can cause aquatic
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Introduction: Calcium hydroxide is a soft white caustic powder used in making mortar‚ cements‚ calcium salts‚ paints‚ and petrochemicals. It is also used in saltwater aquaria to make up kalkwasser/limewater solutions for reef tanks‚ and is used as a pH regulating agent. Notice that calcium hydroxide is divalent and thus has twice the neutralizing power as molecules like NaOH that are monovalent. A Calcium Hydroxide Molecule: Calcium hydroxide is manufactured industrially by adding
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9565 g Molar mass of Na2 EDTA*2H2O 372.25 g/mol Expected M of EDTA solution 8.57 E-3 M Standardization of EDTA Solution Concentration of Zn2+: 0.010009M Volume used: 10.00 mL Trial 1 Trial 2 Trial 3 Final buret reading‚ EDTA 18.83 ml 37.20 ml Initial buret reading‚ EDTA 0.00 ml 18.83 ml Volume used‚ EDTA 18.83 ml 18.37 ml Molarity of EDTA solution 5.312 E-3 mol/L 5.445 E-3 mol/L Average molarity of EDTA solution: 5.379 E-3 mol/L Determination of % MgO of Unknown:
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indicator menu is available under the chemicals main menu (ChemicalsIndicators) or the context menu. Step 3: Fill buret with NaOH‚ obtain a 50 ml buret and fill with .100M NaOH solution. Step 4: Titrate NaOH into HCl until end point‚ record initial buret volume and add NaOH (quickly at first then slowly) until the HCl solution turns pink and record the final buret volume of NaOH in buret. Step 5 repeat steps 1-4 using pH meter‚ add a pH meter to the acid solution. Record numerous points of
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