Fractional Distillation and its comparison to a control simple distillation was the main focus of this lab. The theory behind fractional distillation is fundamentally the separation of compounds. In this experiment we used cyclohexane and toluene as our compounds. Fractional distillation is used when the boiling points of two compounds are within close range to each other. Toluene and cyclohexane have a boiling point difference of 30 degrees Celsius.
In a solution of FeSO4, solution of .02 KMnO4 was added until the combination of the solution turned pink. The change of the color pink indicates that the reaction is complete. The process that was undergone with FeSO4 and KMnO4 is called titration. In chemistry, titration is a procedure used to determine the molarity of two or more solutions. Molarity is the number of moles in a compound in a solution over the number of liter in the solution.
The eudiometer will show the displacement of the water in volume of CO2. Hypothesis: I predict that the greater the concentration of hydrochloric acid, the greater the rate of reaction and so more carbon dioxide will be produced in the same time period than at lower concentrations. I predict this because there will be more collisions between the calcium carbonate and hydrochloric acid. Variable Factors Reasons Control 1.Time duration of experiment 2. Mass of Marble Chips 3.Surface Area of Marble Chips 4..
Once calculated, these results can be analyzed and will either validate or refute my hypothesis. Introduction (Library Research): Ascorbic acid (vitamin C) is found in orange juice. In this experiment, orange juice made from the concentrate was measured for decreases/increases of off-flavours (furfural and α-terpineol) and for decreases/increases of ascorbic acid. Sodium hydroxide (NaOH) as well as hydrochloric acid (HCl) were added during separate trials to change the PH in the orange juice. An increase of PH from 3.2 to 4.2 enabled the protection of ascorbic acid levels, without increasing the levels of other enzymes.
They work best at room temperature around 36-40 C. Introduction For this experiment, I will be looking at how the change in temperature affects the rate of reaction. If the temperature is too high or too low in the water bath the enzymes active site will denature. The best temperature is 37 degrees because this is the natural body temperature which is also called the optimum temperature so the reaction will take place faster. Method * Firstly you have to label a test tube with the temperature that you will be investigating. * Secondly you have to add five drops of phenolphthalein the test tube which you are using.
The acceptable change in the temperature was ± 0.05 ºC. The amount of CO2 produced was kept the same through having the same distance of 5 cm in the manometer tube, as only the same amount of CO2 would move through that distance. The time has been measured since agreed level in the manometer tube was reached, in order to avoid the paralax effect. Mass of sugar and solution was controlled by using weighting machine and by keeping the same mass of each solution for different yeast concentration. Apparatus: • Yeast (20g) • Sugar (8 g) • Water (52 g= 52 cm3) • Termometer (0-110 ºC ±0.05 ºC) • Weighting machine (±0.05 g) • Razor blade • Boiling tubes (20.0±0.5 cm3) • Stand, bosses and clamps • Manometer tube • Clip
Then by writing a balanced chemical equation and using the titration formula, Nb+Ma+Va=Na+MbVb , the molarity is able to be determined. Procedure: 1) Using the graduated cylinder add 10.0 mL of water into the Erlenmeyer flask. 2) Add 5.0 mL of HCl into the flask using another graduated cylinder because acid goes into water when mixing them. 3) Add three drops of phenolphthalein indicator into the flask. 4) Swirl the flask in circular movements to mix the substances.
The system was heated for 4-5 hr under vacuum at 200°C and then cooled down to the temperature (50°C) where we want to perform the adsorption study. Small doses of test gases consecutively introduced to the system and gradually increased up to 50 Torr until an equilibrium pressure was reached. Then the obtained differential heats of the test gases adsorption were recorded as a function of its coverage. Further, the manifold degassed under vacuum for almost 30 minutes; adsorption was conducted in the same manner. Finally, the number and strength of active surface are obtained from the difference between the adsorbed gases from the first and second
When we increase the temperature of the Hydrochloric acid (HCl) the reaction will be quicker, more gas will be formed in a short amount of time. Because increasing the temperature, the particles move faster the ions have more kinetic energy, causing more collisions. Which will increase the reaction. As the temperature decrease the reaction rate will decrease because the particles have less thermal energy, will travel slower, less collision with other particles as a result of this the reaction rate will be lower. Similarly when the Calcium Carbonate (CaCO3) is broken down into powder the rate of reaction will increase.
Introduction A titration was carried out in this experiment to find the concentration of hydrochloric acid is an unknown solution. The aim of this experiment is to determine the number of moles of sodium hydroxide in hydrochloric acid and then to determine the number of moles of sodium hydroxide present in gastric juices. Titration, or volumetric analysis, is a common laboratory procedure for the analysis of substances and solutions. In a titration, the analyst determines the volume of a solution, called a titrant, that reacts exactly with a known weight or volume of another substance. This reaction is carried out by adding a solution of reactant hydrochloric acid from a burette to a solution of sodium hydroxide until just sufficient of hydrochloric acid has been added to react with all of the sodium hydroxide.