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Chemistry practical on titration
Chemistry practical on titration
Titration practicals
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Stoichiometry of Reactions Jessica Scanlan
Experiment No. 7 CHMY 142-25
10/14/14 Trenton Hopkins
I. Introduction
The purpose of this experiment was to examine how the stoichiometry, “the quantitative relationships between substances involved in a chemical reaction”, can be applied to determine the quantity of sodium hypochlorite found in a bleach product. This experiment allowed it to determine how much oxidizing agent is in a cleaner by using a redox reaction, which is a reaction involving the transfer of electrons from the compound being oxidized to the compound being reduced. To determine the amount of oxidizing agent, it is necessary to accurately measure out known amounts of redox reactants, know the stoichiometry
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Record the volume of the sodium thiosulfate solution used in the titration, and repeat the procedure in a duplicate titration.
Using the Volumetric Pipette:
1. Compress the safety bulb, hold it firmly against the end of the pipette. Then release the bulb and allow it to draw the liquid into the pipette.
2. When the liquid level is above the calibration line on the pipette, remove the bulb quickly and put your thumb or index finger over the pipette. Carefully “roll” finger to the side and allow the liquid to drop until the meniscus is level with the mark. Then hold the pipette over the flask to receive the liquid and remove the finger. Allow the liquid to drain out.
Determination of the Oxidizing Capacity of a Household Cleaner:
1. Place a clean, dry 125 mL Erlenmeyer flask on balance, and slowly dispense liquid bleach until there is about .5 g. Record the mass of bleach, and add 25 mL of de-ionized water and about 2 g of KI. Swirl contents until the KI dissolves. Then add 3 drops of 1 M H2SO4, mix, and let stand for 1 or 2 minutes.
2. Then titrate with the sodium thiosulfate solution as in the standardization procedure, adding 6 drops of starch indicator near the end of the titration. Record the volume of thiosulfate solution used in the titration. Make a duplicate
Each subsequent trial will use one gram more. 2.Put baking soda into reaction vessel. 3.Measure 40 mL vinegar. 4.Completely fill 1000 mL graduated cylinder with water.
We used the pipette filler and filled the glucose rinsed pipette to add 10ml of 10% of glucose in test tube 0.
When the flame was blown out and the glowing wooden splint was placed halfway into the test tube containing H2O2 and MnO2 crystals, the splint reignited and caught flame once again. This demonstrates the decomposition of H2O2 into water and hydrogen. MnO2 is a catalyst that increases the rate at which H2O2 decomposes. Adding oxygen to a fire will cause it to burn faster and hotter and the oxygen rich test tube allowed the splint to reignite.
neutralize 35ml of our base. Once we weighed out the KHP we then dissolved it
10. Point the flask away from everyone and open the two-way valve in order to release pressure from the flask. Remove the stopper assembly, then fill up the flask with water. Discard of the solution in the sink.
the mass and initial temperature of the water. Next, impale the food sample on the needle. Next, light
4. Pour about 300mL of tap water into the beaker. Set up a hot-water bath using a hot plate, retort stand, and thermometer clamp. Alternatively, use a Bunsen burner, retort stand, ring clamp, thermometer clamp, and wire gauze.
Rinse your beaker thoroughly to wash any excess powder. 12. Repeat steps 7-11 3 more times for reliability. To make sure the temperature still stays hot by continue heating the water a little bit using the hot plate. 13.
Fill another test tube with 200 mL of plain water and label it Negative Control.
3.) Divide your 30g of white substance into the 4 test tubes evenly. You should put 7.5g into each test tube along with the water.
In a 100ml beaker place 50mls of water, measure the temperature of the water and record this initial temperature onto a table. Set the timer and add one teaspoon of Ammonium Nitrate to the water, stir this continuously until the Ammonium Nitrate has dissolved.
Also a funnel should be used to ensure that all 30 cm3 of sodium thiosulphate is in the burette. Back to the bleach, where I would have to transfer 25mls of the bleach
Apparatus: Ÿ Sodium thiosulphate solution Ÿ Hydrochloric acid Ÿ 250 cm Conical flask Ÿ Thermometer Ÿ Measuring cylinder Ÿ Heat proof mat Ÿ Bunsen burner Ÿ
2. In the large beaker, put water and boil it completely. After that, remove the beaker from heat. 3. Sample tubes (A-D) should be labeled and capped tightly.
In this experiment three different equations were used and they are the Stoichiometry of Titration Reaction, Converting mL to L, and Calculating the Molarity of NaOH and HCl (Lab Guide pg. 142 and 143).