CHAPTER 1
Introduction
1.1 Introduction to the Physical Chemistry Laboratory
The physical chemistry laboratory is intended to acquaint the students with the practice of experimental physical chemistry. Considerable effort has been made in linking the experiments with the topics of theory lectures.
Learning objectives: To familiarize the students with a number of the techniques to be used in laboratory. To give them some basis for judging the reliability of data. To develop the habit of keeping the laboratory record. To understand the interconnection between experimental foundation and underlying theoretical principles and to appreciate the limitations inherent in both theoretical treatments and experimental measurements. To gain familiarity
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1.1) to be employed in the measurements are accurate and within the definite limits. The limit of accuracy is differing in the case of different instruments and apparatus. Since the apparatus for the determination of weight and of volume are those most generally concerned, in chemical or physico-chemical measurements, we shall first consider the methods of calibrating them. Determination of Weight
The determination of the mass or weight of a body is one of the most fundamental of physical measurements. In chemical analysis, the determination of weight of a body is not a matter of great difficulty for weighing about 100g with an accuracy of one part in one hundred thousand. Thus, in weighing glassware’s or other material, the difference in weight, due to the handling, the manner of drying the apparatus, etc., may sometimes amount to at least several tenths of a milligram, while the accuracy of the balance itself might quite well allow of the weight being determined to less than one-tenth of a
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Fill the burette with water. Make sure the tip is free of bubbles. Drain into a waste beaker until it is at, or just below, the zero mark. Allow 10-20 seconds for drainage. Make an initial reading to a precision of at least 0.01ml. Test for tightness of the stopcock by allowing the burette to stand for 5 minutes and then re-reading the volume. There should be no noticeable change in the reading. Once the tightness of the stopcock is assured, refill the burette and again drain into a waste until it is at, or just below, the zero mark. Allow for drainage. Touch the tip of the burette to the wall of the waste beaker to remove the pendent drop of water. Make a volume
Introduction The purpose of this Lab was to identify the density of the unidentified object and determine what substance the unidentified object given by the teacher was. The density calculated in the experiment will stay the same because the density of the unidentified object will stay constant. The Independent Variable of this experiment was the calculated density and the unidentified object given. The Dependant Variable for this experiment was the density.
Repeat steps 1-10 for two more trials. Conclusion: 1. I chose to compare temperature and amount of reactants in my experiments. I chose these because I thought they would reveal the the most drastic time differences. I also chose these factors because I had prior knowledge of them before I even started chemistry.
Now, they are ready to start the lab. The empty crucible is weighed by and the weight was recorded. Then the students used a disposable pipet and put close to 4.0 grams of their milk sample in their crucible on the scale. The crucible was then placed back on
Three trials were done. All three trials were done the same way. In trial one, the weigh boat was first zeroed on the scale. Five grams of the white unknown mixture was measured on to the weigh boat.
Procedure and Observations To begin the lab, first all the correct equipment and materials had to be collected
It required the diluted 2MHCl. 120mL of this HCl was added to the calorimeter, which got covered by the lid and the probe was inserted. A watch glass was weighed again, first without MgO, then with 1.0g MgO. After 3-4 readings were collected, the MgO was added and stirred constantly. The watch glass was weighed then again. Weight measurements were recorded.
3mL of the liquid in each of the vials were added into cuvettes and measured in the spectrophotometer. Before each time point the photo spectrometer was zeroed using a cuvette with 3mL of distilled water. If any of the results were considered unusual the machine was zeroed again and the sample was retested. The results from the spectrophotometer test were recorded in a table. The experiment was repeated six times to gain a sample size of six.
Introduction The intent of this experiment is to understand how hot and cold water interact with each other by combining clear hot water and black ice cold water. I hope to learn more about how hot and cold water interact with each other. As of now, I know that cold water is denser than hot water. Knowing this I formed my hypothesis.
= 10^-3 M = 1,000 mL Here C1,C2; are the first and second concentrations of solution V1 and V2 ; are the required and current volumes. The impeller turned on and DDA, and tap water left to be mixed properly with water for 2 minutes. Approximately 150 grams of quartz added into the solution.
These small errors may be arised as a result of temperature. Because the accurate mesuring process took much time and during this time the temperature of water was decreasing. Among two methods the density bottle gives more accurate measurement of the volume, resulting in more accurate determination of density. One of disadvantages of hydrometer is that hydrometer has Operator dependent readings, therefore has limited accuracy. Morever, for measuring the density using hydrometer large sample volume is required.
Stop the timer as soon as the reaction has stopped taking place and no remaining tablet is visible. Record the data. Empty out the beaker and water. Repeat steps 18-26 three more times, until four trials have been completed in total.
11) After you have prepared the dilutions, clean the outsides of the cuvettes with a paper towel. 12) Place the blank tube (tube 0) in the spectrophotometer. Since distilled water has no color it will not absorb any light so the absorbance number would be zero and this done to test the absorbance scale on the Spectrophotometer for the purpose of having it calibrated correctly. 13) Set the spectrometer to a wavelength of 530 nanometers. 14) Place the cuvettes (numbers 1-6) with the appropriate substance and record it’s reading in the data table.
In the separating funnel, the liquid was left on the retort stand for ten minutes to settle. The cover of the separating funnel was removed.
I. Introduction This experiment uses calorimetry to measure the specific heat of a metal. Calorimetry is used to observe and measure heat flow between two substances. The heat flow is measured as it travels from a higher temperature to a lower one. Specific heat is an amount of heat required to raise the temperature of one gram of anything one degree Celsius. Specific heat is calculated using several equations using the base equation: q=mc∆T II.
That caused a new initial reading of NaOH on the burette (see Table1 & 2). The drops were caused because the burette was not tightened enough at the bottom to avoid it from being hard to release the basic solution for titrating the acid. The volume of the acid used for each titration was 25ml. The volume of the solution was then calculated by subtracting the initial volume from the final volume. We then calculated the average volume at each temperature.