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Discussion of a lab report under preparation and standardization of sodium hydroxide
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The 50 mL beaker was filled one third of the way with sodium hydroxide. The base was poured into the buret, and the buret was cleaned with it. The contents were spilled out into the sink.
The 125 mL Erlenmeyer flask was washed with distilled water. The contents were spilled out into the sink.
The 50 mL beaker was filled with 50 mL of sodium hydroxide. The sodium hydroxide was poured into the buret, it was ensured that the buret read zero. The buret was placed in the buret holder and the Erlenmeyer flask was placed to help adjust the height of the buret.
One antacid tablet was taken out of one of the containers. The weight boat was placed on the scale and the scale was zeroed. The tablet was then placed in the boat. The mass was recorded.
The tablet was
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The scale was zeroed. A scoopula was used to transfer the ground up antacid onto the weigh boat until the scale read approximately 0.2 grams.
The contents of the weight boat were then transferred into the Erlenmeyer flask.
The flask was taken to the second lab bench and 2-3 drops of methyl orange was added into the flask.
The stir bar was placed in the flask. The flask was placed on the stir plate which was under a buret with hydrochloric acid (Figure 2).
The buret was filled with acid, so that it read zero, using a funnel. The initial amount of acid was recorded. The stir plate was turned on and the buret nozzle was opened.
The speed of the stir bar was increased as the flask filled with acid. The flask was observed till there was a permanent colour change (Figure 3).
Once there was a permanent colour change, the acid was allowed to continue to pour for a short amount of time.
The buret nozzle was closed and the final amount of acid in the buret was recorded. The stir bar was taken out of the flask using a bar magnet.
The flask was then taken back to the first lab bench and placed under the buret with sodium hydroxide. The initial volume of the base in the buret was
Start with the hot water and first measure the temperature. Record it. 8. Then pour 40 ml into the beaker. You can measure how much water was used by looking at the meniscus.
3. The beaker was filled with water and the metal was placed in the water.
The procedure of the lab on day one was to get a ring stand and clamp, then put the substance in the test tube. Then put the test tube in the clamp and then get a Bunsen burner. After that put the Bunsen burner underneath the test tube to heat it. The procedure of the lab for day two was almost exactly the same, except the substances that were used were different. The
Apparatus: * 1 measuring cylinder * 1 test tube * 1 stop clock * A large gelatine cube containing indicator and NaOH * Hydrochloric acid ranging from 1-3 molars * A scalpel Diagram: Method: * Take the large gelatine cube and cut into 15 equal pieces * Place on piece of the cube into the test tube * Measure out 10mls of HCl in the measuring cylinder * Pour the HCl into the test tube with the gelatine cube and start the clock * Time how long it takes for the pink colour inside the gelatine cube to completely disappear * You will also notice that the cube dissolves slightly * Record your results and repeat this same process 3 times for each molar of acid: § 1 molar § 1.5 molar § 2 molar
For part C, the concentration of was determined to be 1.01 mol/L, 0.973 mol/L, and 1.158 mol/L. These results show a relatively closed to the accepted 1.00mol/L of NaOH. The differences of these results are understandable since the concentration of NaOH would changes over time because during the transfer of NaOH powder in part A, it was exposed to the air, thus it could reacts with CO2 in the atmosphere to produce Na2CO3 and water, therefore, changing the concentration of NaOH. Furthermore, the NaOH could also react with the glass thus it wills also reducing its concentration. However, all of the concentration of NaOH that was determine are maximum of 0.158mol/L differences compare to the standard 1.00 mol/L, therefore, it can be concluded that the result are accurate.
For this method of experimentation, the control was used to compare the colour change of the ethanol solution. Samples from each of the vials was taken at 0, 15, and 30 minute intervals; each of the treatments was started two minutes apart, this was to allow for correct incubation periods. A pipette was then used at each interval to draw out a sample of the solution, which was then transferred to a cuvette in order to find the
Second, a small sample of solutions must be collected and transferred to the beakers by pouring or pipetting from the 500 mL Erlenmeyer flasks containing the solution. Third, a clean wooden stick must be dipped into the solution, soaked for three to five seconds, and put to the flame created by the bunsen burner. It is very important to make sure that that the wooden stick should not catch fire and this may have to be done this several times in order to get a good color. Next, the color of the flame must be recorded in detail and the wooden stick must be ran under some running water to cool it off. Finally, the stick must be discarded into the trash and a new wooden stick must be obtained. Dipping the wooden stick into the solution and put toward the flame must be repeated for the remaining solutions and when you are all done all of the solutions , these solutions should be poured down the drain with a lot of water and rinsed with soap and water. Finally, the labels should be cleaned off, and the beakers should be left upside down to
== Refer to, Chemistry Lab #1 – What’s the substance? I didn’t change most materials when I did this experiment, but I added 4 materials, which are: * 5 test tubes * 2 stoppers * 1 large piece of paper And I deleted 1 material, which is: * Spatula Methods = == ==
Remove the extra solvent on a steam bath under a hood while flushing the flask with N2 gas, leaving the crude extract. Weigh extract.
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.
NOTE: The stirring rod was not used in the First and Second experiments, as it was not available. A substitute we used the thermometer.
Weigh out 0.6g of Sodium Chloride onto a watch glass with a Digital scale and pour into the beaker in step 1.
It makes the results as accurate as possible, as it allows the hydrochloric acid to be added drop by drop when the sodium hydroxide is close to neutralising. · Burette Stand - This holds the burette steady in place. · Funnel - This allows hydrochloric acid to be poured into the burette so none is spilt. · Pipette - This is used to accurately draw out the correct amount of a substance from a solution. · Safety Filler - This is used to draw the substance up the pipette
borate) and 1.0 g. of sodium hydroxide in 20 mL of warm water. It may
The purpose of this experiment is to use our knowledge from previous experiments to determine the exact concentration of a 0.1M sodium hydroxide solution by titration (Lab Guide pg.141).