Method Prior to the experiment, the LabQuest must be set up and the conductivity probe must be calibrated. Calibrate the conductivity probe connected to a LabQuest using a solution of known conductivity. In this experiment, a solution with a conductivity of 1000 μS/cm was used. Choose “Calibrate” from the menu and choose “Calibrate Now”. Then submerge the conductivity probe into the standard solution and type in the known value of the solution; 1000 in this case. Then, wait for the voltage to stabilize and press “Keep”. Exit by pressing “OK” when this process is done. Set the data collection method on the LabQuest to “events with entry”. In order to titrate the phosphoric acid, the following method was used. Using a pipette, transfer 60ml …show more content…
Start the titration and keep titrating in 0.5ml intervals until the graph shows the end point. Transfer the data from the LabQuest to a computer using a USB key and then open the file to select the values which is used to obtain the graph below. Pipette 20ml of the phosphoric acid into an Erlenmeyer flask and add 3 drops of Thymol blue indicator. Perform a titration using NaOH solution. Repeat the experiment. The cola drinks were titrated using the following method: Prepare the beverage in a 250ml volumetric flask. Use a funnel to facilitate the process. Place the beaker on a hot plate so that it boils and place a watch glass on top to prevent the carbon dioxide from the atmosphere getting dissolved in the cola. Once the cola starts to boil, continue to boil it for another 10 minutes so that the carbon dioxide is removed. When the cola has finished boiling, cool it in an ice bath and pour the cola back in the volumetric flask and use distilled water to fill the flask to compensate for the evaporated water. Using a volumetric pipette, transfer 60ml of the cola to a beaker and put the magnetic stirrer in the beaker. Submerge the conductivity probe in the cola. Fill up the burette with NaOH …show more content…
If a large amount of the indicator was added, it was possible to slightly distinguish the color. However, this wasn’t clear enough to properly distinguish the end point of the
Question3: Experiment 3 The unknown acid sample was 1 • Monoprotic Acid Trails Initial NaOH solution (mL) final NaOH solution (mL) The volume of NaOH to titrate the acid (mL) Amount of Unknown Acid sample 1 (g) The moles of the Unknown Acid (mol) Molar mass of the Unknown Acid (g/mol) A 3.38 28.31 24.93 0.150 0.0026 57.69 B 0.18 29.32 29.14 0.175 0.0029
2. Add 8cm³ of sodium carbonate to each tube using a measuring cylinder. 3. Measure out the strontium nitrate for each boiling tube and add it (boiling tube 1 contains 1cm³, test tube 2 contains 2cm³ and so on). 4.
The purpose of this lab was to be able to use physical characteristics to determine the identity of an unknown compound. The data from this experiment classified aluminum as metallic; ascorbic acid, paraffin, palmitic acid, sucrose, graphite, and water as molecular; sodium chloride as ionic. In order to determine this, 3 tests were conducted. The first test was to test the conductivity of each substance at room temperature. In this test, only graphite and aluminum conducted.
This disproved my hypothesis that Powerade would have the most electrolytes and proved that orange juice contains more and would be better for hydration. It answered my investigative question of which liquid would have the most electrolytes with orange juice coming in first place, Powerade in second place and tap water in last place. I would like to improve the experiment by adding in more variables such as more substances to test and testing at different temperatures to see if the temperature has an effect on the conductivity. I also feel that I would like to get more copper wire to change it after each trial as I think the oxidation of the copper wire caused my later readings to fluctuate and perhaps be inaccurate. I therefore conclude that orange juice proved to be the most conductive and that the oxidation o the copper wires caused some of the later readings to fluctuate but overall I feel that the results were accurate.
For this I needed to first obtain deionized water. I cleaned my large graduated cylinder and got 20 + or - 2 mL of deionized water. I then added this water to the beaker that contained the mixture I created from the last step of the experiment. I also gathered 2 boiling stones and added them to the mixture of the last step. I placed the beaker on a hot plate and heated it up to 130 degrees Celsius.
The quantitative solubility of the unknown compound was determined to be 29/100ml. The known solubility of sodium sulfate is 28.11g/100mL water. Using the found solubility to compare to the known solubility of sodium sulfate. This solution created in the solubility test, the conductivity of the unknown compound was tested using an Ohmmeter to measure the resistance of the solution. Resistance is the measure of a substances ability to conduct
Weighed 1 gram of NaC2H3O2 and mixed it with ionized water. Boiled 12 mL of 1.0M Acetic Acid added into a beaker containing the sodium carbonate on a hot plate until all the liquid is evaporated
The mass of an 11 dram vial was taken before and after it was filled with 15 mL of distilled water, resulting in a mass of 29.9667 grams without the distilled water and 44.7771 grams with the distilled water. The looped wire was inserted into the 11 dram vial, to be used for stirring. The 11 dram vial was then submerged into the ice bath, and the Vernier temperature probe was immersed into the 11 dram vial. Once the temperature of the distilled water reached 10°C, the temperature was recorded every 10 seconds. After the data was collected, the 11 dram vial was brought back to room temperature.
Place the conductance sensor into the tap water and record the current in mA. Tap the conductance sensor onto a paper towel and then dip in into the three distilled water rinses. Place the sensor in the sports drink and measure the current. Record the current in units of mA.
15) After each cuvette was tested, place the distilled water sample (Cuvette zero) to reset the spectrometer and to ensure that the scale is calibrated and repeat for each cuvette test. Data/Results: Tube Number Concentration Of CoCL2 (Mg/ML) CoCL2 Stock (ML) Distilled Water (ML) Spectrometry Reading at
INTRODUCTION The purpose of this lab is to practice the use of the scientific method, the series of steps in which scientific data is collected through observation and experimentation. The secondary purpose of this lab is to discover the issue that dominantly interests the students at Nova High School. HYPOTHESIS
Practical I: Acid-base equilibrium & pH of solutions Aims/Objectives: 1. To determine the pH range where the indicator changes colour. 2. To identify the suitable indicators for different titrations. 3.
Preparation of Working Electrode. Carbon fiber is used as the conducted electrode for this experiment. Cut two long stripes of carbon fiber into 8 shorter stripes around the same length. The chart shows the length, width and area of each of the eight carbon fiber pieces.
Regional Elections The concept of democratic elections remains the same internationally, nationally, and regionally, however the means to collect qualitative data can vary. Regional elections are viewed as a subordinate process compared to national elections, however, their impact for their area remains just as significant (Jeffery & Hough, 2003). The voting behavior is immensely different regionally as certain areas have values engraved in a respective area (Jeffery & Hough, 2003). In comparison to larger scale elections regional values may be dissolved in the greater span on the state or nation view.
II. METHODOLOGY In order to perform this experiment, the students will need a distillation set-up with a connector receiver, an iron ring and stand, a Bunsen burner, a wire gauze, a 250mL round bottom flask, a graduated cylinder, a thermometer, one or two boiling chips, an alcoholic beverage, masking tape, an ice bath, a stirring rod, and, optionally, food coloring. It is imporatnt to avoid playing with the apparatus and equipment so as to avoid breakage and injuries, especially since fire is being dealt with in this experiment.