Law of Conservation of Mass

Use a glass beaker to pour an adequate amount of the liquid substance and use the pipette from the glass beaker.

In the experiment, What Goes Around Comes Around, the element copper was put through a series of chemical changes to observe whether or not the final copper precipitate had the same mass as the initial mass of the copper. The purpose of this lab is to prove the Law of Conservation of Mass, which states that mass cannot be created nor destroyed. In the experiment, if the final mass of the copper precipitate is equal to the initial mass of copper, this law is proven because the copper was not destroyed in the chemical reactions nor was it created. Copper was first combined with the compounds nitric acid(HNO3), water(H2O), and sodium hydroxide(NaOH). This mixture was first chemically separated using heat to boil out the water. The aqueous solution

The two most obvious formation of the precipitate were the combinations with the MgSO4. The MgSO4 and NH3 solution became very opaque and the MgSO4 and Na2CO3 turned from liquid to a full solid white substance. The Na2CO3 and CH3COOH did not have as strong of a reaction, however, the precipitates were able to be visualized with in the clear

Describe a fourth scenario in which either the “Law of Conservation of Matter” or the “Law of Conservation of Energy” could be observed. Using as many sentences as needed, describe how an experiment could be set up to further explore your recorded observation. The goal is to show understanding of the concepts in the lesson.

Copied the observations table in our notebook. Then recorded the mass of the beaker using the balance and wrote down the measured mass in the observation

Fill a test tube about 1/3 full with cold tap water for use in step 34.

3. When two solutions combine and a solid substance is formed, this solid is called a precipitate. In your experiments, if the clear reactant solutions you combined together formed a cloudy product, then a precipitate (solid substance) was formed. Describe the precipitates (according to color and clarity) and the substances that formed them. (18

5.Position gas collecting hose so it runs from reaction vessel through gas collecting box to opening of the graduated cylinder. The idea is that any gas coming through the tube will rise in the graduated cylinder and displace the water in it.

4.Measure 35mL of warm water and add them into each of the 4 test tubes at about roughly the same time. It is essential that the water is warm. Do not seal the test tube.

the stopcock to release the pressure. Close the stopcock, shake the funnel several times, and again release the pressure through the stopcock (see Technique 12, Section

1.) Transfer the distillate to separatory funnel. Fluid didn’t seem very clear but sufficient to finish our lab on time.

Anton Lavoisier proved the law of conservation of matter. His experiments on the nature of chemical reactions showed that matter is neither gained nor lost in a chemical reaction. His findings indicated that the mass of the reactants in a chemical reaction is always the same as the mass of the products. Ernest Rutherford used the gold foil experiment and concluded that the atom is made mostly of empty space and has a positively charged center called the

a) Transfer pipette was obtained. The pipette was cleaned because distilled water does not drain uniformly. A cleaning solution or detergent was used to clean the pipette.

2. Calculate the mass of the reaction mixture in each reaction first by determining the volume of the solution and then assuming that the density of the solution is the same as pure water (1.0g/ml). Show work here and record your answer in Data Table 2.

3. Place about 3g of the mixture into the evaporating dish and carefully weigh it to the nearest 0.01g with the top loading scale and record its mass on the data sheet.