Free Erlenmeyer flask Essays and Papers

Demo #1: Two Erlenmeyer flasks, 500mL and 250mL, two peeled hard-boiled eggs, water, and a square burner. The larger flask is taken off the heat after the water started boiling, and an egg was placed on the opening of the flask. The egg is then slowly being sucked into the flask until it plops into the water. The same steps were taken with the 2nd 250mL flask however, the entire egg didn’t make it into the flask; it broke in half. The pressure of the air inside the flask increases and the oxygen

beaker filled halfway with water. The bath was then sat on a hot plate and lest to boil. 2g of salicylic acid was placed in a 125 mL Erlenmeyer flask with 3 mL of acetic anhydride, and 3 drops of concentrated sulfuric acid. The solutions were mixed and placed in the boiling water bath. The solution was left in the boiling bath for 30 minutes. The 125 mL Erlenmeyer flask was removed and placed on the side to cool to room temperature. Once cooled the solution was placed into a 150 mL Beaker that was filled

Part A Procedures Observations 1. Put 400 mL of tap water into a beaker. Heat it on a hot plate until it starts to boil. 2. Put a rubber-stopper assembly into a 125 mL Erlenmeyer flask. Twist the stopper into the flask's neck until it is tightly secured. Connect the connector and the gas pressure sensor valve, then twist in a clockwise motion. Prevent gas leakage by covering the stopper and flask's top with parafilm. Twist the white valve until it is perpendicular to the valve stem in order to

was poured inside the Erlenmeyer flask. Weight of the container with this solution was 103 g. The flask was closed with a stopper (cork?) and the total weight increased to 103.161 g. 0.25 g of Zinc was added to the solution. The maximum temperature was observed at 26.5° C with the final weight of the container at 103.411 g. The same steps were repeated while adding 25 g of Zink to the solution and resulted in explosion while performed in a closed flask. Meanwhile, when the flask was not closed, 25 g

The objective of this experiment was to perform extraction. This is a separation and purification technique, based on different solubility of compounds in immiscible solvent mixtures. Extraction is conducted by shaking the solution with the solvent, until two layers are formed. One layer can then be separated from the other. If the separation does not happen in one try, multiple attempts may be needed. The experiment was conducted in three parts: Part A of the experiment consisted of extracting

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

Burette • Three 250ml Erlenmeyer flasks • 10ml pipette and pipette bulb • Wash bottle • Funnel • Retort stand and clamps Procedure: 1. Clamp the 50ml burette to the retorted stand and add the sodium hydroxide solution (base) using a funnel. 2. Clean one of the Erlenmeyer flasks using a wash bottle and add 10ml of Acid “A” into it. Use the pipette to accurately measure 10ml before adding it to the flask. 3. Add 2-3 drops of phenolphthalein indicator into to the Erlenmeyer flask containing the Acid

and then twice with approximately 5 mL of ~0.25 M NaOH solution (Fisher Scientific, Certified ACS Pellets, S318-3). A 125 mL Erlenmeyer flask (Fischer) was obtained and 0.999 g of potassium hydrogen phthalate (KHP, C8H5KO4) (Acros Organics, 99+%, Code: 417955000, Lot: A0358893) was added. A precision balance

Analysis of a Household Acid: Titrating Vinegar” by the Department of Chemistry at APSU. The first procedure requires one 10mL volumetric pipette, one 50mL buret, two small beakers, one labeled “vinegar” and the other labeled “NaOH”, three 250mL Erlenmeyer flasks, labeled one, two and three, and one large beaker for waste collection. Collect 50mL of vinegar in the beaker labeled “vinegar” and record the brand and listed concentration of vinegar. Then collect about 60mL of NaOH in the beaker labeled “NaOH”

NaOH solution created from part one and the initial volume was noted. Next, 0.7g of KHP was obtained and placed in an Erlenmeyer flask where it was mixed and dissolved with 25mL of deionized water. After the KHP finished dissolving 4 drops of indicator, phenolphthalein, was added to it. Lastly, the titration was conducted by added the solution from the burette into the Erlenmeyer flask until the solution turned pink for approximately 15 seconds, which indicated neutrality. Once the solution turned pink

added water again, stirred, and pipetted the top layer into an erlenmeyer flask. Used a spatula to scoop anhydrous sodium sulfate into the cyclohexane mixture until it no longer stuck together at the bottom of the flask. Set up and ran the vacuum filter. Concentrating the sample- Once all of the cyclohexane was filtered into the round bottom flask, removed and connected it to the rotary evaporator and allowed evaporation until the flask fully dried.

the crude sample, and a 98% yield of naphthalene and benzoic acid, which is great as far as results go. It means enough hydrochloric acid, HCl, was added for the conjugate acid, benzoic acid, of the base, benzoate that was in the aqueous layer Erlenmeyer flask before the addition of the acid. The separation of naphthalene and benzoic acid seemed successful as far as turnout of product came. Out of the 1.00 g of crude sample started with, 0.40 g of naphthalene was recovered and 0.58 g of benzoic acid

This was repeated two more times for a total of three flasks. A flask was placed on a hot plate and heated until it was at 80 C. As the solution was heated a burette was filled with a KMno4 solution. After the solution was at the required heat a magnetic stir bar was added to create a whirlpool. The KMno4 was then titrated into the solution until the heated solution turned light pink in color. This process was repeated for the two other flasks. The average molarity was then found for the kMno4

and placed in a pre-weighed 25 mL round bottom flask, along with 2.5 mL of glacial acetic acid and a magnetic stir bar. Then the reaction apparatus was assembled, the dry tube was charged with conc. sodium bi sulfate, the 25 mL round bottom was attached to the apparatus, and 5 mL of Br2/HBr mixture was obtained and placed in the round bottom. The reaction took place for 20 minutes. An orange liquid was obtained and placed in a 125 mL Erlenmeyer flask along with 25 mL of water and 2.5 mL of conc. Sodium

The Effect of Sodium Thosulphate Solution on the Rate of Its Reaction with Hydrochloric Acid Aim To find out how the concentration of sodium thiosulphate solution affects the rate of its reaction with hydrochloric acid. Prediction I predict that the higher the concentration of Sodium Thiosulphate solution the faster it will react with the hydrochloric acid. Firstly for a reaction to take place the particles must collide and secondly collide with enough energy to break and make new

The Rate of Reaction between Thiosulphate and Hydrochloric Acid Equipment: pen, paper, 2 measuring cylinders, conical flasks, 2 beakers, HLC, Na2SO4, stop clock. Method: What I am going to do is draw a cross on the paper with the pen then get10cm3 of Na2SO4 and 50cm3 of HCL and put in separate beakers. Then put the Na2SO4 in the conical flask, which is placed on the cross on the paper. Then I will add the HCL to the Na2SO4 and start the stop clock. I will stop the clock when I

0020) mol L-1. The amount of sodium carbonate in the conical flask from A-E was 0.113 g, 0.195 g, 0.1368 g, 0.1872 g and 0.1898 g respectively. Results: To obtain a concentration value for the HCl a solution of (0.1008 ± 0.0020) mol L-1 HCl was titrated with Na2CO3 with methyl orange to give a

Marble Chips Experiment Pilot Aim: To investigate how the concentration of hydrochloric acid affect the speed of reaction with marble chips. Prediction: I predict that the more hydrochloric acid there is the faster the chemical reaction. I also predict that the more dilute the acid is (the more water there is with the acid) the slower the chemical reaction. Hypothesis: I predicted what I did because the more concentrated the hydrochloric acid is the more energy there will be and

conical flask when we perform the experiment because the chemical fumes are pungent and are not good to breath in. Method. We are going to measure the rate of reaction by how fast or slowly the mix of chemicals and water goes cloudy by placing a piece of paper with a cross on it underneath the conical flask and all agreeing when it has disappeared from sight. In this experiment we will need to use the following: Equipment Use Stop clock To time the experiment Conical flask To

Hydrochloric Acid of 3 different concentrations as following 2 molar, 0.5 molar and 0.1 molar. In order to calculate the results must be within 0.05cm3 of each other. Apparatus Burette Volumetric Pipette Beakers Conical Flasks Volumetric Flasks Funnel Clamp Stand White Tile Fair Test For a fair test I will have to make sure that I change the equipment for each test so that the residue of the last test doesn't alter my results and also I must use the same amounts