Erlenmeyer Foils

In this lab experiment our main focus was to get skillful in using tools such as the metric ruler, balances, thermometer, and graduated cylinder to capture measurements of length, mass, temperature and volume. Additionally, this lab helped us to become more familiar with the uncertainty of measurements, as well as becoming efficient with rounding our measurements to the correct numbers of significant figures. Our results are measured consistently with rounding to the closest answer we could possibly acquire as the data can tell you.

It used mass, temperature, length, volume, density, and making a dilute solution. I learned the importance as well as the difficulty of making proper measurements in a lab setting. If one measurement is off, it will throw the entire equation off. This will give either incorrect or inaccurate results.

One milliliter of 6.00-M phosphoric acid was placed into a 125-mL Erlenmeyer flask using a volumetric pipette. Using a slightly larger pipette, six milliliters of 3.00-M sodium hydroxide was transferred into a 50-mL beaker. Then a disposable pipette was used to slowly mix the sodium hydroxide into the phosphoric acid while the solution was swirled around. Then both the beaker and flask were rinsed with 2-mL of deionized water and set aside. A clean and dry evaporating dish was weighed with watch glass on a scale. Then the solution was poured into the dish and the watch glass was placed on top. The solution was then heated with a Bunsen burner to allow for the water to boil off to reveal a dry white solid. After the dish cooled to room temperature it was once again weighed and the new mass was recorded.

Using the direct weighing and weighing by difference methods to find weight and mass of chemicals and compounds.

Used parafilm to cover the top of the Erlenmeyer flask to ensure no evaporation occurred

Abstract: This experiment served to analyze the densities of eight different substances by placing them within a container in the order of their perceived densities. From our results, we were able to determine that there was less mass per unit of volume for the items on the upper layers of the column compared to the denser items that constituted the base. The substances were ordered in the graduated cylinder (from top to bottom) from least dense to most dense. According to our table, dish soap was denser than whole milk, but yet it floated on top. This

First a 500 mL beaker was filled with little temperature water and then placed on the base of the Buretrol stand. A piece of magnesium ribbon was obtained and the weights of this ribbon was taken and recorded. There after a string also a certain length was wound around this magnesium ribbon. Next 100 mL gas measuring tube was partially filled wi an approximate amount of hydrochloric acid. The rest of the gas measuring tube was completely filled with water. Thereafter the string with the magnesium ribbon was suspended inside the

Zero-out the balance and place an empty evaporating dish on the scale. Weigh and record the mass.

For the experimental procedures I unscrewed the lids of both the polymer vial and the water vial, I poured the water rapidly into the bottle with the polymer. The water must be poured rapidly

During the experiment, a total of two beakers were used: one that contained the hot water bath and one that held the ice water for the ice bath. Two separate graduated cylinders were used as well: one to measure and

Mass = (Mass of Cool Flask Assembly After Heating) – (Original Mass of Flask Assembly)

This experiment consists of four methods, of measuring and weighing room temperature water using the different devices, each method repeated five times. Method one is to

Then, a10µL pipette was equipped with the appropriate tip, and the volume was set to 1µL. The pipette was then immersed in the DI water and used to draw the set volume and deliver it to the weighing boat. The mass was recorded. This process was repeated for four more aliquots of 1µL of water, and the cumulative weight was recorded. After that, the weighing boat was removed from the balance, dried, placed back, and the balance was tared again to read 0g. Now the volume was set to 9µL by adjusting the micropipette knob, and 5 cumulative weights of 9µL aliquots of water were measured. The entire process was repeated for a second trial. Moreover, the 2-trial cumulative weighing process for the small and large volumes was repeated using the 100µL pipette (with 10µL for small volume and 90µL for large volume), and yet again for the 1000µL pipette (with 100µL for small volume and 900µL for large volume). Note that the disposable plastic tip was changed any time there was residual water droplets trapped inside. Finally, the temperature of the water was measured by the

Instead of using a 500mL volumetric flask a 1L volumetric flask was used. This made calculations that required Liters (L) easier as the numbers could be carried without doing any math. This also made the experiment more accurate. Even though the absolute uncertainty increased so did the volume of the container, this meant that

In experiment number two, take an Erlenmeyer flask form the shelf and place it on the workbench and close it. Then add 1.5atm of butane gas to the flask and note that the volume of the flask is 150mL (the gas occupies the entire volume of the flask.) Next take a syringe from the materials shelf and place it in the flask and record the new volume of both the flask and the syringe. After recording the data in the lab notes take the flask and place it in a constant temperature bath at 40 degrees Celsius. Record the temperature (in degrees Kelvin) and the volume of the flask added to the volume of the syringe in the lab notes. Next change the temperature of the