The Solubility of Potassium Nitrate Introduction The purpose of this experiment was to observe how temperature affected the solubility of solid potassium nitrate that was put in different solvents. The temperature was not the other thing that was being varied to observe the solubility of potassium nitrate, the amount solute was also varied and the kinds of solvents in this experiment were varied. The nature of each solvent changes due to the common ion effect which is basically means that the concentration of a soluble salt is reduced if there is a common ion with that salt. Also potassium nitrate solubility in basic and acidic places was also determined, to see if it affected the temperature. The moles of KNO3 s/ Kg solvent were needed to calculate the correct molal concentration.
* Then you will have to put the test tube in a water bath and leave it until the contents reach the same temperature as the water bath. * Then you will have to take the thermometer from the test tube and put a glass rod into it instead. * After this you will have to use a 2cm syringe to measure out 1cm of lipase to the beaker in the water for the temperature you are investigating. * Then add the lipase to the test
My hypothesis for the experiment was that the optimum temperature for catalase to function is 98.6o F because this is the optimum temperature for the human body. The optimum pH level for the catalase function is 7 because the human’s optimum pH is 7. Materials and Methods Forceps Test Tubes Raw Liver Hydrogen Peroxide Test Tube Rack Gloves Goggles Pipette Waste Beaker Beakers Hot Plate Ice Bath Thermometer The procedure that we used to do the normal catalase activity was that we first transferred 2 ml of hydrogen peroxide solution into a clean test tube. Next we took
Acid Base Titration Purpose: The purpose is to calculate the molarity of a NaOH solution by titrating the base with 5mL of standard HCl solution in each trial. By adding the base with unknown molarity to the acid with 0.10M the molarity of NaOH can be calculated. The base, NaOH, helps bring the pH of the acid, HCl, closer to seven, which neutralizes it. When using the buret the amount of NaOH used is able to be determined. Then by writing a balanced chemical equation and using the titration formula, Nb+Ma+Va=Na+MbVb , the molarity is able to be determined.
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.
ii. Materials & Methods: First, testing the enzyme specificity. Obtain three test tubes and mark them at the 1 cm and 5 cm levels. First tube: fill it to the first mark with catalase buffered at pH 7.0, the optimum pH for catalase. Then fill the second mark with hydrogen peroxide.
3. Since dealing with enzymes, it was important to choose well the different temperatures for the experiment – for example, not making all five temperatures high because then it would not take effect. Observation during the experiment After the digestion of the gelatines was completed, the silver salts on the film peace chipped off and left a clear piece of film. The silver salts that had fallen were left as a black substance that remained at the bottom of the test tube. The Effect of Temperature Increase on the Digestion rate of Gelatine by Trypsin by the time taken for the silver salts on the exposed film pieces (in trypsin solution) to fall off, leaving clear film pieces: Temperature of the 2% trypsin solution (°C) ±0.5 | Time taken for film pieces to become clear (seconds) ±0.7 – Trial 1 | Time taken for film pieces to become clear (seconds) ±0.7 – Trial 2 | 25 | 186.6 | 184.7 | 35 | 150.0
Determination of Freezing Point and Verification of Freezing Point Depression for a Mixture by Linah Richer Partners: Maike Blakely CHM317 Preformed: Nov. 8th, 2013 Report: Nov. 19th, 2013 Abstract: The purpose of this experiment is to determine the freezing point of the solvent, biphenyl, and verify the freezing point depression equation ΔTf=-ikfnsolutemsolvent. The addition of solute will lower the vapor pressure of the solvent/solute mixture resulting in the lowering of the freezing point for the mixture solution. The experiment resulted in the experimental difference in the two trial freezing points to be 0.08 K leading to a calculated change in temperature freezing to be -1.92 E -5 K, and an overall decrease in temperature freezing of the solute/solvent solution compared to the pure solvent solution. Introduction: Experimentally it is understood that the addition of a nonvolatile solute to a solvent will lower the vapor pressure, raise the boiling point and lower the freezing point. 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.
Gravimetric Determination of Sulfate Purpose The purpose of this lab is to determine the percentage of sulfate in the hydrate by precipitating the sulfate as barium sulfate. Materials Filler paper Sodium sulfate Graduated cylinder Bunsen burner Watch glass Beakers (250 mL, 400 mL) Rubber bulb Graduated pipette Beaker tongs Funnel Filter Paper Sodium Sulfate Drying oven Wash bottle Stirring rod Silver nitrate Hydrochloric acid Distilled water Small test tube Procedures First, .4861 grams of sodium sulfate was placed into a clean 400mL beaker. Exactly 200mL of water and 1mL of HCl was added to the same beaker. A watch glass was placed on the beaker and the solution was heated using the Bunsen burner to a gentle boil. The watch glass was removed with the beaker tongs.
In this experiment we are going to measure the solubility of KNO3 in water at various temperatures. Results can be reported in different ways ranging from grams or salt dissolving in a milliliter of water to grams of salt in 100 mL of H2O In general, systems tend to go to a state of disorder or to a state of greater entropy. During the dissolving process, the particles of the solid become randomly distributed through the solvent in sharp contrast to their orderly arrangement in the solid state. Ion the solid state there are strong forces holding these particles together. In order to dissolve the solid, energy must be expended to overcome these forces.