Balance Lab Title: Get familiar with a Centigram Balance Purpose: The purpose of this lab was to use the Centigram Balance and the Electronic Balance to measure the weight in grams of a copper slug, a 100ml Beaker, and an unknown substance. The experiment was to help me get familiar with the weighing of certain materials and the different types of weighing, including direct weighing and weighing by difference. Materials: 2 Copper slugs, 2 100ml Glass Beaker, 2 Centigram Balances, 2 Electronic Balances, 2 unknown weights. Method: First, measure the copper slug using the centigram balance, then put the slug inside of a 100ml Beaker and measure its weight and record the value in the table below. Then measure the Beaker by itself and calculate the weight of the slug by difference.
Procedure Centigram balance- direct weighing technique 1) Obtain the centigram balance 2) Add the copper slug to the balance 3) Record the mass of the cooper slug in (g) 4) Retain scale and slug for future use. Centigram balance- weighing by difference 1) Obtain the centigram balance 2) Obtain a 100mL beaker. 3) Put the beaker on the scale and record the mass in (g) 4) Transfer the copper slug from the first part of the experiment to the beaker 5) Weight and record the mass of the beaker & slug. 6) Subtract the mass of the beaker from the mass of the beaker & slug. 7) Record the mass of the copper slug in (g) 8) Retain the beaker and slug for future use.
* Place a weighing paper on the balance. Press down on the bar again, waiting untill the scale zeros out, showing “g” for grams to the far right of the display screen on the balance. * Place the specified amount of chemical on the weighing paper, on top of the pan. * Record the number on the scale; this is the weight of the chemical in grams. 3.
Introduction: Thyme contains a surprising amount of iron compounds. This experiment enables us to determine the amount of iron(II) present in dried thyme by means of a redox reaction. Method: 1. Weigh accurately about 1g of dried thyme and put into a 250cm3 beaker. Record the mass of thyme used.
Let’s experiment and observe Whether these ions will have a reaction or indeed soluble in water. Experimental Procedure Let’s begin this experiment by obtaining a 100ml beaker from our equipment tool bar list, then we are going to add 50ml(s) of Potassium Chromate 1M solution to that beaker, The next step we are going to add another ionic compound of 50ml of Lead (11) nitrate 1M into the same beaker as the Potassium Chromate. As we observe the beaker, we notice a reaction has occurred and a precipitate has formed and settled on the bottom of the beaker. The next step is we are going to filter the resulting precipitate into a 250 ml Erlenmeyer Flask with a Buchner funnel. Now that we have filtered the precipitate, we will then place the resulting precipitate into a test tube to measure the weight.
12. Place a paper towel over the drain, pour the content of the well plate, throw the paper towel and rinse the well plate. DATA, OBSERVATIONS, AND CALCULATIONS: Data Table: Oxidation - Reduction | | Reactions | Mg in Na2SO4 | Bubbles | Zn in MgSO4 | Small bubbles | Pb in Zn(NO3)2 | Dark lead changed into lighter color | Pb in FeCl3 | Changed the lead into slight green yellow | Fe in CuSO4 | Changed the iron into orange color | Note: I added more than 10 drops to make sure that the pieces are well covered. QUESTIONS: A. Based on your observations make an activity series of the metals used.
iLab 1: Separation of a Saltwater Solution Devry University BIOS135 Professor Subbhalakshmi, Dhalladoo 11/01/14 Introduction The purpose of this lab experiment was, to practice using the scientific method and separate a mixture of salt and water based on the physical properties of each component. I will examine more closely the physical properties of matter. To do this procedure we must evaporate the water and leave behind the salt from the solution. In 103c the water evaporates and behind left is the salt. From this information, the percentage of salt verses water ions can be determined Ions are also produced in the liquid or solid state when salts interact with solvents (for example, water) to produce "solvated ions," which are more stable, for reasons involving a combination of energy and entropy changes as the ions move away from each other to interact with the liquid.
10. Repeat the procedure for a second metal. Analysis: Our data | Trial #1 | Trial | Mass of zinc | 1.99g | 4.01g | Mass of water in Calorimeter | 45g | 45g | Temp. of water in Calorimeter | 20°C | 21°C | Temp. of boiling water | 100°C | 100°C | Peak temp.
Experimental Procedure: 250 mL of the copper solution was made by creating 100 mL of the solution, reacting CuO with HNO3, and then diluting to the mark of 250 mL. Using this stock solution, different concentrations were made and placed in the sprectrometer for observation. The absorbances and transmittances were recorded for use when identifying the amount of the color-absorbing copper ions later. A graph was plotted of Absorbance v. Molar Concentration easily see the results of the experiment. Pre-Lab Questions: 1.
The major findings were that crude oil has a specific boiling point. And gasoline is the first to be distilled then kerosene and then in the end the lubricating oils. Procedure From the Equipment menu, select Distillation Equipment. Obtain the 100 mL Round Bottom Flask. Now right-click on the flask, and select Heating Mantel from Distillation Equipment then, Right-click on the flask, and select Distillation Head from Distillation Equipment last, Right-click on the flask, and select Condenser from Distillation Equipment.