Flask Synthesis Lab Report

I. LIQUID - Identification of an Unknown Liquid: Using the physical properties of Solubility, Density, and Boiling Point.

We then created an ice bath using a 250mL Erlenmeyer beaker. The 50 mL Erlenmeyer beaker was then labeled as “Acid Extract”, and was placed in the

In the third stage of this experiment, the density of a liquid was determined and compared to known standards. A 100ml beaker was filled to about half-full with room-temperature distilled water. The temperature of the water in ◦C was recorded in order to compare to known standards later. A 50ml beaker was then weighed on a scale in order to determine mass and recorded. A sample of the distilled water with an exact volume of 10ml was then placed in the 50ml beaker using a volumetric pipette. The 50ml beaker with the 10ml of water was then weighed again and the initial mass of the beaker was subtracted from this mass to obtain the mass of the 10ml of water. With the volume and the mass of the water now known, density was calculated using d = m/V and recorded in g/ml. This process was then repeated to check for precision and compared to standard values to check for accuracy. Standard values were obtained from CRC Handbook, 88th Ed.

Corresponding to the previous experiment, this week’s experiment measures the participants’ ability to conduct basic, fundamental laboratory procedures. These procedures revolve around scientific measurements of volume, mass, and density. Unlike last week’s activity, this week’s experiment had a few modifications. In addition to distilled water, saltwater and an unknown substance were added. There was a total of five substances to choose from; Hexane, Methanol, Ethyl acetate, Ethylene glycol, and Dichloromethane. Part C, the unknown liquid number was four, which the average density was 0.789 gmL-1, and from looking at the chart the unknown identity was methanol. Part A, the temperature of the water was 20 oC, which was in front of the class,

In this experiment, 0.31 g (2.87 mmol) of 2-methylphenol was suspended in a 10 mL Erlenmeyer flask along with 1 mL of water and a stir bar. The flask was clamped onto a hotplate/stirrer and turned on so that the stir bar would turn freely. Based on the amount of 2-methylphenol, 0.957 mL (0.00287 mmol) NaOH was calculated and collected in a syringe. The NaOH was then added to the 2-methylphenol solution and allowed to mix completely. In another 10 mL Erlenmeyer flask, 0.34 g (2.92 mmol) of sodium chloroacetate was calculated based on the amount of 2-methylphenol and placed into the flask along with 1 mL of water. The sodium chloroacetate solution was mixed until dissolved. The sodium chloroacetate solution was poured into the 2-methylphenol and NaOH solution after it was fully dissolved using a microscale funnel.

To find the density, we divided the mass by the volume (which we found by using water displacement) for both our boiling chips and the ones we had in the lab. We also tested the effect on boiling water using 4 flasks of the same amount of water. 2 flasks contained the same amount of boiling chips, we used two flasks to prove that boiling chips always had a

Question: Will changing the water temperature affect how quickly a gummi bear dissolves in water? Hypothesis: If the temperature of the water is warmer, then the gummi bear will decrease more quickly in size than compared to cooler temperatures. Materials: Gather the following materials including: •safety equipment including: goggles, gloves, and apron •two 25 mL beakers •one graduated cylinder •one thermometer •one hot plate •8 red gummi bears from the same brand •20 mL of normal tap water in each beaker •one balance measured in grams •forceps •paper towels Procedure: 1.Gather all the materials listed above. 2.Include data tables in your experiment by doing two trials.

Trial 1: A dish was filled with approximately 2 cm water and a candle mounted on clay was place in it. The candle was lit and a jar was placed over top of the candle so that it was resting on the dish. When the flame went out the water level inside the jar was measured. This process was repeated three times.

The objective of this experiment is to see how safe bottled and tap water is to drink based on what is in the water; specifically the contaminants and the pH balance of the water. As well as if the temperature of the environment that the water is placed in affects the pH balance of the water along with if bacteria is grown due to the condition it is in. Water is one of the most important things in life, being as it is known as the universal solvent, and humans and many other animals need it to survive. Along with water, the balance of pH is also extremely important in the maintenance of any organism 's life, including the lives of humans. Temperature is known to affect the speed of movements of ions within a solution. There are specific

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.

We suspended the flask at a slight angle, up to its neck in the water bath, making certain that the water never touched the foil cap. To suspend a thermometer in the water we rolled a piece of napkin paper, and used a clamp to supported to the apparatus, making certain that the thermometer bulb didn’t touch the bottom of the beaker. We turned on the heating plate, and boiled the water in the water bath. We waited for the whole unknown liquid to vaporize, and recorded the water-bath temperature. As soon as the liquid completely vaporized, we removed the clamp-flask assembly from the water bath.

It would be difficult to keep the temperature constant for this amount of time so we put the boiling tube with the bathing solution into a beaker of water at the required temperature. This insulted the bathing solution so that it stayed at the right temperature for the full 2 minutes. Some groups did not do this so over the 2 minutes the temperature was not exact. If the bathing solution was not at the correct temperature the results may not be as reliable. Using an electronic thermostatic water bath would keep the temperature of the bathing solution constant during the 2 minutes and therefore the results would be more reliable.

First, using a glass cup, 100.0g of filtered water in room temperature was measured. Filtered water was used so that the mineral content of water is always constant, and also the temperature is kept the same since water temperature affects rate of evaporation and how much the solvent gets dissolved in water. Then, 5.0g, 10.0g, 15.0g, or 20.0g of table salt (coarse salt, 粗塩) was put in and stirred until completely

“Molar Mass of a Volatile Organic Liquid” lab is focused on determining the unknown substances correct label. During the lab, 3 separate Erlenmeyer flasks were filled with the same unknown clear colourless solution #3 from the back of the lab located under the fume hood. In each of the beakers it was observed to ensure that only 2ml of the unknown solvent was placed into each of the Erlenmeyer flasks. Once the unknown solvents were prepared, the hot water baths are needed to be observed to ensure that 200mL or enough distilled water was placed to fully encapsulate the Erlenmeyer flask. Both of the flasks were placed in the water at approximately the same time. After about 10 minutes, it was witnessed that the water has come to a boil due to

Twenty Invokana tablets were weighed and the average weight was calculated. Accurately sample equivalent to 10 mg of canaglifozin was weighed and transferred into a 100 ml volumetric flask.10 milliliters of methanol was added and sonicated to dissolve it completely and volume was made up to the mark with the diluent. It was mixed well and filtered through 0.45 mm filter. Further 0.1 ml was pipette out of the above stock solution into a 10 ml volumetric flask, diluted up to the mark with diluent and filtered through 0.45 mm filter. An aliquot (20µl) of this solution was injected into HPLC system. Peak area of canagliflozin was measured for the