Separation of a Solid Mixture Purpose In this experiment I will become familiar with the separation of mixtures of solids. I will also learn separation techniques based on the chemical properties of a substance. Procedure I first measured my weighing dish to find out its mass. I then poured the mixture into the weighing dish and found out the mass of the mixture. I then poured the mixture on to a solid white piece of paper.
Record this mass on your date sheet. If a very hot crucible is put on an electronic balance, the balance can be ruined. 5. Put about 5.00 g of sodium hydrogen carbonate in the cool crucible. Once again using the electronic balance, record the mass of the crucible plus baking soda accurately on your data sheet.
First, we had to calculate how many grams of copper (II) sulfate we needed to form 100 mL of a 0.200 M solution of copper (II) sulfate. We determined that we needed to use 4.994g of copper (II) sulfate to make the solution. We added distilled water to the 4.994g of copper (II) sulfate in a beaker until it reached 100 mL. Then we put the beaker on a hot plate and added a magnetic stirrer. We determined that the mass of zinc necessary to completely react with the copper (II) ions in the solution was 1.308g.
Ref: Lesson #3 The spontaneous elevation or depression of a liquid in fine hair like tubes. 5. How does capillary action affect the dye penetrant during the inspection process? Ref: Lesson #3 After the dye penetrant is applied, and excess penetrant is removed, you apply the developer. The developer, according to capillary action, forces the penetrant out of the defected area, making the defect visible.
Record the initial temperature of the liquid in the calorimeter. Watch the thermometer until maximum temperature is achieved. Weigh out 2.0g of NaOH pellets. Record the temperature of the distilled water in the calorimeter until the temperature is constant then add all of the pellets at once. Gently stir the pellets until the acid is dissolved by shaking the the apparatus.
To get the right result for solution reaction to occur, it is base on the measuring liquid for each solution. You need to pour the right amount of each solution so you can determine the result of solution reaction (product) will occurs accurately. If you pour your solution (liquid) into a beaker not at the right point than you can’t find the result of solution reaction (product) accurately. You need to put a lid on top of a weighing bottle because you don’t want your solution to spill out and other stuff (oil, dirt, sweat) will get into a weighing bottle that can cause the mass is not accurate and not
So, qwater = qmetal Using the formula qmetal = m × c × ΔT, calculate the specific heat of the metal. Use the data from your experiment for the metal in your calculation. Part II: Calculate the energy change (q) of the surroundings (water) using the enthalpy equation qwater = m × c × ΔT. We can assume that the specific heat capacity of water is 4.18 J / (g × °C) and the density of water is 1.00 g/mL. Show ALL your work.
| The variables must be controlled so the experiment is a fair test otherwise the experiment is not accurate. | 3.2 Equipment list -2m Hydrochloric Acid - 100mL beaker - Mylanta tablet -Stopwatch - Water - Bunsen burner -Gas -Tongs -Matches (light Bunsen burner) -Tongs 3.3 Safety Assessment See Risk Assessment sheet for safety hazards 3.4 Method - 20mL of Hydrochloric Acid was poured into a beaker - The 1st tablet was placed into the HCL and the time from star to finish
This experiment will help the researcher understand the effect that home solutions such as salt and sugar have on waters freezing point. The plan of the project plan is to start off by collecting all the materials needed in order to complete the experiment, next step to come up with a hypothesis, after creating a hypothesis a procedure must be used to carry out the experiment. After completing the experiment the last step would be to create a graph using the results from the experiment. Research was done in order to find does the amount of salt and sugar effects the freezing point of water? The concept of freezing point depression is helpful in applications where water needs to be kept in a liquid state.
The main uses include: to determine the number of components in a mixture, to determine the identity of 2 substances, to monitor progress of a reaction and to determine effectiveness of purification. This technique involves placing sample onto the end of a sheet of glass or plastic that is coated with an adsorbent, this is called the stationary phase. After it is then placed into a solvent chamber containing a volatile solvent and covered, this is called the mobile phase. Via capillary action, the solvent pulls the components on the plate upward. The two most common adsorbents: alumina (Al2O3) which when anhydrous, alumina is more active and will adsorb substances more strongly.