its (conjugate acid) Carbonic acid was used. The purpose of the experiment was to test the capacity of an undiluted and diluted buffer solution as well as examining the buffering capacity of distilled water using measured concentrations of NaOH and HCL. These replacements of strong acids and bases for weaker ones give buffers their ability to moderate pH. (Stoker 2013). Part 2 of the experiment‚ the buffering capacity of lake water was tested. The ions naturally present in rivers are buffering
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Materials: 0.20M HCl (±0.02moldm-3) 1.1g solid NaOH (±0.1g) A solution of vinegar of unknown concentration (density= 1.05gcm-3) Phenolphthalein Method: * A solution of NaOH was prepared by dissolving 1.1g in 250cm3 of water * 1.1g of solid NaOH was weighed and then dissolved in the stirred until dissolved in 250cm3 of water * 25cm3 of this solution was placed into a conical flask and 3 drops of phenolphthalein indicator were added * A burette was filled with 0.2±0.02moldm-3 HCl * The
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[pic] Drops |Water(HcL) |Water(NaOH) |Liver(HcL) |Liver(NaOH) |Egg White(HcL) |Egg White(NaOH0) |Potato(HCl) |Potato(NaOH) |Buffer(HCl) |Buffer(NaOH) | |0 |7 |4 |7.4 |5 |8.2 |7 |6.9 |4 |10.7 |10 | |5 |4.5 |7 |6.9 |6 |7.5 |8 |6.2 |5 |10.5 |10 | |10 |2.7 |9 |6.3 |6 |7 |9 |5.7 |5 |10.4 |11 | |15 |2.6 |12 |5.8 |6 |6.4 |9 |5.3 |6 |10.3 |12 | |20 |2.5 |12 |5.4 |6 |4.5 |10 |4.9 |7 |10.2 |12 | |25 |2.4 |13 |5.1 |6 |3.5 |10 |4.6 |8 |10.1 |13 | |30 |2.3 |13 |4.8 |6 |3.3 |11 |4.2 |8 |10 |13 | | 1.
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Approximately 40 mL of the ionized water was added to the 100 mL beaker‚ then in a 10-mL graduated cylinder‚ 5-mL of HCl was measured then added to the 100-mL beaker of water. The 100 mL beaker was then placed on the assembled ring stand. Approximately 40 mL of the 0.1M NaOH was added to the 250 mL beaker. The 40-mL of NaOH was then added to the buret which was then attached to the ring stand. The LabQuest and the Vernier pH sensor was then hooked up and turned on to measure and graph the pH of the
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Stoichiometry February 28th‚ 2013 Abstract: The reactions of the Sodium Hydroxide and two acids‚ Hydrochloric Acid and Sulfuric Acid were performed. The heat given off by these two reactions was used to determine the stoichiometric ratio and the limiting reactants in each experiment. Introduction: Coefficients in a balanced equations show how many moles of each reactant is needed to react with each other and how many moles of each product that will be formed. Stoichiometry allows us to
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CASE STUDY 1: Xstrata Produced Acidic Oxide – SULFUR DIOXIDE Industrial Process – Sulfur Dioxide is an acidic oxide produced domestically and industrially in many ways. Xstrata‚ particularly Mount Isa Mines LTD‚ produces sulfur dioxide as a by-product from the extraction of copper from ores. Copper ore mined in Australia is predominantly chalcopyrite (CuFeS2)‚ a sulfide ore of copper. The extraction of copper begins with crushing the ore and subjecting the crushed ore to froth floatation. In
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Iodine is a test for starch while Benedict’s solution is a test for reducing sugars. When solution A is tested by benidicts test‚ the clear blue solution changed to a little reddish and brick red precipitate is formed.this result show that solution A is a reducing sugar. When carried out iodine test with solution A‚ the colourless solution remain unchanged . this tell us that starch is absent is solution A. When solution B is tested with Benedicts test‚ the clear blue solution remain unchanged‚ we
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experiment. Reaction Equation: NaHCO3(s) + HCl(aq) ( NaCl(s) + CO2(g) + H2O(l) Materials: safety glasses baking soda (NaHCO3) 1 M HCl and dropper 500 ml Pyrex flask hot plate Procedure: 1. Find the mass of the 500 ml Pyrex flask. Record this mass in the Data Tables. 2. Add one teaspoon of baking soda to the flask‚ and record the total mass in the Data Table. 3. Use the dropper to drip HCl into the flask. Add HCl until the fizzing ceases. 4. Set the flask
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In my experiment I have found that 50 millilitres of HCL with 2 grams of sodium chloride had the highest conductivity rate compared to the second most conductive solution‚ 50 milliliters of vinegar with 2 grams of sodium chloride‚ and the last conductive solution‚ 50 milliliters of distilled water with 2 grams of sodium chloride. In my first hypothesis I stated if I added sodium chloride to distilled water‚ than the overall conductivity will become more conductive than just distilled water‚ since
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of the components of a buffer. For a given addition of acid or base‚ the buffer component concentration ratio change less when the concentration are similar than what they are different. Materials: Acetic acid (MW=60 g/mol)‚ NaOH solution (0.5M)‚ HCl solution (0.001M)‚ calibration buffer (pH3.5 and pH 5.5)‚ 7-UP‚ 100 Plus. Apparatus: pH meter‚ pipettes (10mL)‚ volumetric flask (250mL)‚ beakers (150mL)‚ burettes‚ burette holder and stand‚ funnel‚ graduated
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