Name: |Date:| Exp 1: Observations of Chemical Changes|Lab Section: | Data Tables: Part 1: |Chemicals|Well No.|Observations of the Reaction| A.|NaHCO3 + HCl| H12|White and bubbled slightly and settled down to smaller smaller bubbles| B.|HCl + BTB| H11|Golden yellow; looked darker under the black paper| C.|NH3 + BTB|H10 |Dark blue| D.|HCl + blue dye| H9|Greenish color| E.|Blue dye + NaOCl| H8|Blue and lighter than NH3+BTB solution color| | with the 1 drop of HCl| H8|Turned blue green
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by determining the concentration of HCl in the water. • Using a pipette and pipette filler‚ we accurately pipetted 25 cm3 of 0.010 mol dm-3 sodium hydroxide solution into a conical flask. • Then we added a few drops of methyl orange indicator and placed it on the white tile. This solution was then titrated with the water obtained from the river. • After we stood the burrette up using a stand and clamp. • We then filled up the burrette to approximately the 0.00 mark with the
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Investigating the effects of acid rain in the growth of cress seedlings IntroductionAcid rain is rain or any other form of precipitation‚ which is unusually acidic. It has harmful effects on plants‚ animals and buildings. Acid rain is mostly caused by human emissions of sulphur and nitrogen compounds which react in the atmosphere to produce acids. Acid rain can slow the growth of vulnerable forests and cause leaves and needles to turn brown and fall off. In addition‚ it depletes minerals from the
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AVIATION 111 PRIVATE PILOT GROUND SCHOOL Spring 2013 5.0 CREDITS Instructor: Mark Richardson Phone: 253-833-9111 ext. 4708 Office Hours: 11:00 - 12:00 Monday-Thursday TC 129 Email: mrichardson@greenriver.edu Course Description: Includes aerodynamics‚ navigation‚ weather‚ communications‚ regulations‚ flight physiology‚ weight and balance and other subjects preparatory to the FAA Private Pilot written exam. Materials For Course: Text: Pilot Handbook of Aeronautical
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ammonia and turns suspended litmus paper blue‚ NH4+ is present. Sample Solubility and Solution Tests *For DIW-soluble sample‚ dissolve about ½- 2/3 of sample in about 10-15 mL DIW. pH Test Fill several vials with solution‚ and determine pH using indicators (starting with HBtB) pH 1.5: HSO4- must be present‚ and OH- must be absent pH about 2-2.5: SO42- may be present in mixture‚ but not in pure substance pH 3-3.5: OH- not present pH 5-6: NH4+ present pH 7: Cl-‚ NO3-‚ SO42-‚ K+‚ and/or Na+ could
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molarity of NaOH‚ we rinsed a burette with about 5ml of water and another 5ml of NaOH to prepare it for the experiment. We then measured exactly 25ml of the prepared KHP from the previous part into a 250ml Erlenmeyer flask and added 2 drops of the indicator‚ phenolphthalein. Next we filled the burette with the approximately 0.1 M NaOH so that our initial volume will be 0.0mls. We then started our titration by carefully pouring a little amount of the base into the prepared 25ml of KHP with phenolphthalein
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analysis‚ acid - base reactions are often used to provide a basis for various titration techniques. The equivalence points of acid - base titrations can be estimated from the colour change of chemical indicators‚ such as phenolphthalein‚ methyl red‚ methyl orange and so on. The choice of an indicator suitable for a particular titration requires a detailed knowledge of the chemical properties of the acid and base. This difficulty can be avoided by using physical methods‚ which follow the change in
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reagent -Observe - ppt forms = K+ and/or H4N+ - no ppt = No K+ or H4N+ Blue Litmus test for H4N+: -Mix the sample in DIW -Add 6M NaOH -Suspend damp red litmus -Observe - red litmus turns blue = H4N+ pH test: -Test sample solution with Indicators -2 HSO4 ; 3-5 Al(OH2)63+;4 Cu2+; 5-6 (NH4 ‚ Mg(OH2)62+‚Zn(OH2)62+ ; 7 neutral ions (Ag+‚ Na+‚ K+‚ Ca2+‚) ; 13 OH- ; Test for Cl-: -add 1M HONO2 till solution is acidic test -Add 1 drop of 0.02M AgNO3 to small amount of sample solution -Stir
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was determining the volume of a solution needed to react with a given mass or volume of a sample is called titration. The equivalence point is when the same number of moles of acid and moles of base has been added. Phenolphthalein is used as an indicator because it will have a color change when the equivalence point has been reached. Procedure See AP Chemistry. Chapter 4‚ Acid-Base Reactions‚ Titration Lab for procedure‚ or see worksheet. Data Standardization of Base with Solid Acid |
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most commonly the result of bicarbonate and carbonate ions; in treated waters‚ alkalinity may also be contributed by hydroxide‚ phosphate‚ silicate‚ and other treatment ions. The color changes of phenolphthalein indicator‚ which occurs at pH of 8.3 (P Alkalinity) and bromcresol green indicator‚ which occurs at pH 4.2 (Total Alkalinity) are the standard reference points for expressing alkalinity. For boilers operating up to 300 psig‚ the accepted alkalinity range is 200 ppm to 700 ppm‚ with P being
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