Reaction : CO2+H2O → H2CO3 Technique : I will prepare a bowl that can fit 1000cc water. Then measure the initial temperature of the water using Pasco sensor first. Then, I will use insulated gloves to put one dry ice every 30 seconds and see the temperature change. I will do this continuously until 300 seconds then I stop. Variable : Control - Water, 1000cc Independent - Dry ice amount, 1-10 Dependent - Temperature Background Information: Dry ice is frozen carbon dioxide, Co2, which can make lots of fascinating experiment.
This was done by taking small amounts of the unknown acid. It was then placed into capillary tubes and inserted into the Bibby Sterilin Device. Starting with a high plateau to find a quick melting point and then proceeding to find an actual melting point. The next experiment that aided in finding more characterizations of unknown #2651145-PLF13 was equivalent weight. In order to find the equivalent weight a titration of the unknown acid had to be conducted.
It was also stated by Professor Bob Prior that “it is possible for salt to hurt an enzyme due to the fact that salt can change the polarity of certain parts of an enzyme.” Over time, salt tends to denature certain enzymes, making them less efficient catalysts. This is one of the key reasons that our hypothesis states tha salt will cause the enzyme to be less effectual. Our lab group felt compelled to find an answer. We used Morton's Sea Salt in our experiment because the Morton Company has been in the salt business for over 160 years. They have a very informative website in which we were able to resource valuable information on the differences of sea and table salt (Mortonsalt.com).
In this experiment, the freezing point for the solvent biphenyl will be determined theoretically and experimentally, as well as the verification of the freezing point depression equation for a solvent/solute mixture. Represented by the equation kf=RTf2MΔHf , the freezing point depression will be constant for a solvent despite whether a solute is involved in the experiment. The freezing point equation can later be used to calculate the temperature the solvent freezes represented by the equation, ΔTf=-ikfnsolutemsolvent . The freezing point of the solvent containing a nonvolatile electrolyte will be equal to the addition of the freezing point depression to temperature of the pure solvent and will always be lower than the freezing point of the pure solution. Because the freezing point depression is a colligative property, the higher the concentration of
The linear regression model could also be use to approximate the heat of solution. Where finding the heat of solution could be important is when we are trying to figure out the enthalpy change of a solution. Procedure The procedures for this experiment were followed as those printed on pages 221-223 of the manual, experiment number 36 (see references). Deviations in this experiment from the what was printed in the procedure was that Microsoft excel was needed to make the graph instead of using the graph paper provided at the end of the experiment. Data and Results The first eight graphs show the relationship between the temperature of the solution and the nature log of each specific molal concentration.
Using a thin-layer chromatography, or TLC, the position in which molecules stop advancing upwards could be observed. By applying the TLC method to this experiment, different traveling distances of a certain chemical, with changing salt concentrations of water, can be measured. In this investigation, however, sheets of tissue papers were dipped into salt water with different concentrations and soaked until the water traveled to the top, so the method was different from the TLC experiment. Consequently, the volume of liquid absorbed will likely not change with different salt concentrations since every time the paper will be dipped into the solution until it completely absorbed water, each time in the same manner. Moreover, the mass of solution absorbed will increase because the density of the solution increases with increasing concentration.
Testing Saccharides Saccharides, which are also known as carbohydrates, are the most essential biomolecule for the human body. Carbohydrates are what run the body to function. Saccharides help your brain and nervous system to function properly. What we were testing in both experiments was to see if there was a presence of saccharides. More specifically in these experiments, we tested if there were reducing sugars with the Benedicts reagent in the first experiment and if there were starches present with Lugol’s solution in the second experiment.
The Depression of Frozen Point The boiling point and the freezing point both refer to colligative properties; in other words, the individuality of each particle is not as significant as the number of dissolved particles in a solution. In a solution, the boiling point increases and the freezing point decreases when the concentration of particles increases; this means that the change in normal boiling point as well as freezing point of water is connected to the increase of particles. Throughout the experiment, calculating the freezing point depression constant of solvent was a significant process. Observing the co-relation between the sugar concentration and freezing point was important too. In addition, the freezing point of the same solution for sugar and salt was compared.
As for endothermic the reactions pulls in energy and makes it cold to touch. The other experiment measured the pH level in the reaction. The reaction consisted of sodium hydroxide and hydrochloric acid also to see at which point the reaction becomes neutralized. Neutralization is a reaction between an acid and a base forming a salt and water even tho you can’t see the salt due to the salt dissolving into the solution and the pH level of the reaction around level 7 and has a green sometimes yellow colour when the universal indicator is added. The neutralization gap shows how small the gap is to make the reaction neutral.
The consecutive evaporations and condensations allow for the separation and purification of compounds with similar boiling points. Boiling points are directly proportional to pressure; therefore as the pressure is decreased the boiling point will also decrease. Compounds with very high boiling points can be distilled much easier if a vacuum is applied. Vacuum distillation is a common technique which allows for the distillation of high boiling compounds under mild conditions. Both the simple and fractional distillation apparatus can be performed under vacuum by attaching the vacuum line to the fume hood vented adapter near the collection