at different pHs Abstract These experiments aimed to determine the optimum pH ranges various buffers are effective and provide opportunity for the use of the Henderson-Hasselbalch equation to prepare a buffer of a specific pH. Three different buffer systems were initially investigated; volumes of weak acid and weak bases of specified concentration were prepared and titrated against strong acid or strong base solutions with pH readings taken at frequent intervals to determine pH ranges over which
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acid and 1–2 mL of starch indicator solution. Immediately titrate the mixture with iodine solution. Record the burette reading the moment the mixture turns permanently blue (end point). 5. Repeat the above steps with each of the other two flasks. pH Level Procedure 1. Fill up the beakers with 20mL of wine sample. 2. Wash the pH tube with distilled water so that no particles left behind and give wrong results. 3. After washing the pH tube‚ put the pH tube in the wine sample beaker
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50% w/v NaOH solution (50 g in 100 cm3 solution) Eriochrome Black T indicator pH 10 NH3 - NH4Cl buffer Hydroxynaphthol blue indicator 0.01 M EDTA (disodium salt) Safety Equipment Enclosed footwear Laboratory coat Safety glasses Rubber gloves Method Part A: Determination of total hardness 1. Pipette 50 cm3 mineral water into a conical flask. 2. Add 2 cm3 buffer solution followed by 3 drops of Eriochrome Black T indicator solution. 3. Titrate with 0.01 M EDTA until the solution turns from
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or base1. Titration starts with a beaker or Erlenmeyer flask containing a very precise volume of the known concentration solution and a small amount of indicator‚ which is put underneath a burette containing the solution with unknown concentration1. Small drops of the titrant are then added to the known solution and indicator until the indicator changes which means the endpoint has been reached. Single drops of the titrant can sometimes make a permanent or temporary change in the indicator2.
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Factors that affect how the PH changes during a titration experiment. Concentration of the alkali Having a higher concentration of alkali will mean that there will be more molecules closer together for the acid to collide with. This will speed up the reaction as collision theory suggests that molecules have to collide to react and if there are more molecules to collide with the reaction will happen faster as there is a higher chance of a collision. Volume of alkali An increase in volume would mean
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Investigation Into The Effect Of PH On The Activity Of Potato Tissue Catalase Aim The aim of my investigation is to see how pH affects the activity of potato tissue catalase‚ during the decomposition of hydrogen peroxide to produce water and oxygen. Catalase + 2H2O2 Catalase + 2H2O +O2 Catalase + Hydrogen Peroxide Catalase + Water + Oxygen Independent Variable The independent variable in this investigation is pH. Each individual enzyme has it’s own pH characteristic. This
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Determining the Unknown Concentration of NaHCO3 (aq) Through Titration Introduction Titration is the accurate addition of a titrant- solution in a burette- into a measured volume of a sample (Kessel‚ 2003). There are many different types of titration‚ such as acid-base reaction‚ redox reactions‚ precipitation reaction and more (Dohrman). In this lab an acid base titration will be explored. In an acid-base titration‚ the concentration of an acid or base is unknown and is determined by the adding
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the surface area of a cell relatively to its volume‚ then the diffusion time will decrease. Materials: Agar cubes‚ bromothymol blue- pH indicator‚ vinegar‚ ruler‚ spatula‚ beaker. Methods: I used agar cubes as cell models. The agar was cut into blocks corresponding to the sizes indicated to us in Table 1. The cubes have been dyed with bromothymol blue- pH indicator. Then they were placed into vinegar‚ where they began to turn yellow as the vinegar diffuses into the agar. I timed this diffusion process
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titrations with acids in order to gain information about those acids. The first acid tested was hydrochloric acid. This titration showed that the equivalence point occurred at a pH of 7.0. The second acid tested was the polyprotic phosphoric acid. This titration resulted in two equivalence points‚ one at pH 5.01 and the second around pH 9.25. The pKa1 of this acid was 2.25 and pKa2 was 6.90‚ compared with the known values of 2.16 and 7.21‚ respectively. Three titrations with the unknown acid “O” showed that
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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 and observe - if solution turns cloudy = Cl- Test for SO42-: ( same as Cl- test but with 0.025M Ba(NO3)2 instead of 0.02M AgNO3) -white ppt = SO42- Test for HOSO3-: -pH test then “Test
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