Title: Separation of a Mixture of Solids Purpose: To learn about separating solids and how this happens. By separating the solids one will be able to tell the difference between a mixture and a pure substance. Procedure: Four main steps. Separating the iron from the mixture with a magnet. Separate the sand by boiling water and pouring the water off, then move on to separating the Benzoic acid using filter paper.
Procedure: Weigh out the mixture, and then use different techniques to separate them from each other. Using the magnet to separate out iron filings, boiling the substance to separate out the sand, and filtration paper to separate the salt and benzoic acid. Once substances are separated and dried, weigh them out to receive a total amount. III. Experimental Data: The original weight of the mixture before separation was 4.6g.
6- Place only the edge of the Q-tip at the top the Flame. 7- Remove it when you see the of light being given off to avoid burning the Q-tip. 8- Clean up procedure: Discard used Q-tips to the bin, cover back compounds and put them up in a safe place, pour away distilled water in the sink, disconnect the Bunsen burner and clean it if stained,clean the lab test surroundings with paper towel to ensure no stain is left, wash your hands remove your goggles only when all equipments have been placed in safe places. Compound | Flame Colour Observation | 1 LiNO3
In order to remove the iron filings I will use the iron bar since it the composition of iron will be picked up by the magnet. Then I will bring the water to a boil in order to only remove the sand. After, I will use the ice bath to remove the benzoic acid. After removing all other solids I will be left with only the sodium chloride in the water. Results: Please see attached the final results and questions to go with Lab #3.
You can go to the web for flow chart examples. Flow Chart: (3 pts) Based on the physical properties (solubility, density, melting point, etc.) of sand, NaCl (table salt), benzoic acid, and iron filings, prepare a flow chart for the experimental procedure for this experiment and include it in your report in the table on page 2. Then you will be ready to follow the experimental procedures as described in the lab manual. If you make any changes to the experimental procedures, please record these changes below: Flowchart: (complete before
Ailsa Cottam 28.10.13 Separating salt and sand. Introduction In this experiment students were asked to separate a mixture of salt and sand, illustrating the fundamental means of separating a mixture of an insoluble material from one which is soluble. Aims/Hypothesis Students were asked to perform an experiment into the separation of a mixture of salt and sand, identifying the calculations of both sand and salt once going through the separation process. The separation techniques that were used in the lab were Evaporation and Filtration. Materials Protective Glasses | Beaker (250ml) | Stirring rod | Filter funnel | Filter paper | Evaporating basin | Bunsen burner | Heat resistant mat | Tripod | Gauze | Sand | Salt | Matches | | | Method After collecting all the materials needed for the experiment, the students were asked to weigh a mixture of sand and salt (5g) into a 250ml beaker.
Title Page Experiment Title: Experiment 4: Qualitative Analysis of Cations III – Mg2+, Ca2+, Fe3+, Ba2+. Aim To determine the presence of the cation II , Mn2+, Ni2+, Fe3+, (Fe2+), Al3+, Zn2+ by using separation method to confirm the presence of cation II in the test solution. Procedure Please refer to the laboratory manual page 30-31. Results Procedure Number and Ion | Test Reagent or Technique | Evidence of Chemical Change | Chemical(s) Responsible for Observation | Equation(s) for Observed Reaction | 1 | Centrifuge the solution. | A brown precipitate was formed.
About 3mL of the wash water is collected in a small test tube. A few drops of 0.1M silver nitrate solution is added to the water to test for the presences of Cl- ions. Lastly the filter paper was placed in the dry oven to dry completely and then weighted. Calculations and observations were made and recorded. Observations The
Then you will fill a BURETTE with sodium hydroxide (a base) that has a known concentration. Because all the reactants and products in this reaction are colourless, an INDICATOR DYE is added to the sulphuric acid to let us know when all the acid present has been EXACTLY NEUTRALIZED by adding base. Finally, the sodium hydroxide in the burette is added to the acid/indicator solution until the indicator changes colour. (An indicator dye is a chemical that has a different colour in an acid and a base.) PROCEDURE 1.