Brass Alloy Lab Report

The purpose of this lab is to figure out the mass percentage of copper in a penny. Furthermore, by doing this lab we will practice using a spectrophotometer and review the names of equipment such as volumetric glassware, pipets, and volumetric flasks.

Due to this fact, the concentration of copper in the solution is able to be calculated by using light absorbance. Since zinc doesn’t absorb any light, we are able to deduce that the greater the absorbance, the greater the concentration of copper.

In this gummy bear lab, the goal was to see the movement of water in cells depending on the concentration of solutes in the environment. The control group was the type of water used. The research question for this experiment was, how does concentration of solute in the environment affect water movement in cells? The hypothesis thought of for this question was that the salt water would enlarge the gummy bear the most. The distilled water would not enlarge the gummy bear as much as the salt water.

The purpose of this experiment is to distinguish the relationships between reactants and products, in addition to expanding on concepts such as single displacement reactions, mole ratio values, moles to mass, theoretical yields, limiting reactants, excess, stoichiometric relationships and percentage errors.

Washing of the copper is necessary in this experiment to separate the iron from the copper and make sure the iron is not counted in the mass of the copper.

The Copper Cycle is a popular experiment used to determine if an element, in this instance, copper, reverts to its elemental form after a chain of reactions. This experiment is very dangerous because of the reactions between the strong acids and bases. In this experiment I performed a series of reactions starting with copper metal and nitric acid to form copper (II) nitrate. Then I reacted copper and several other solutions such as, sodium hydroxide, sulfuric acid, ammonium hydroxide, and hydrochloric acid to form precipitates. In conclusion my percent recovery

Copper is a naturally occurring element that can be found in all plants and animals. A certain amount of copper is necessary for health, and the human body has developed a way to maintain the proper level of copper in it (Minnesota). Even so, large concentrations of copper, and general long-term exposure, can have a negative impact on the body. Symptoms include stomachaches, vomiting, diarrhea, liver and kidney damage, and even death (Lenntech). Exposure to copper comes from many areas, but the most common one is through the water. Copper is commonly found in plumbing pipes, which can lead to high levels of copper in drinking water and fresh water sources due to erosion. Lakes and streams are also treated with copper to prevent algae overgrowth (Group).

To complete the research a scientist went out to the Delaware River three different times at 6 different locations (Shi, Allen & Grassi, 1998). He collected the water and brought it back to the lab to be tested (Shi et al., 1998). The research method that was used was sampling and collecting data to see if the river has a high rate of copper in it (Shi et al., 1998). The results of the journal were also conclusive. Data was shown that when the water went through treatment plants or through sewers the water would come out with more copper than without going through these places (Shi et al., 1998). In the long run, the water is safe depending on where and when you collect the water for use (Shi et al.,

When the tip of the rod touched the pH paper, the color of the pH paper became blue.

Purpose: The purpose of this experiment was to observe the many physical and chemical properties of copper as it undergoes a series of chemical reactions. Throughout this process, one would also need to acknowledge that even though the law of conservation of matter/mass suggests that one should expect to recover the same amount of copper as one started with, inevitable sources of error alter the results and produce different outcomes. The possible sources of error that led to a gain or loss in copper are demonstrated in the calculation of percent yield (percent yield= (actual yield/theoretical yield) x 100.

Examine a piece of nichrome wire. On the data sheet, record the color and the luster of the metal. Use a forceps to hold the wire in the flame of your burner for about two minutes (recall where the hottest part of the flame is located). Describe the appearance of the wire while held in the hottest part of the flame. Allow the wire to cool and reexamine it. From your observations, determine if there was a physical or a chemical change. Give specific reasons for your conclusions. Save the nichrome wire for step #2.

This experiment was conducted under conditions described by Williamson, 2003. To begin, approximately 150 mg of cyclohexanone was placed into a vial. In a separate 10 x 100 mL reaction tube, 1.0 mL of HNO3 was added by pipette, along with a pre-weighed boiling chip. The reaction tube containing the nitric acid was clamped into a sand bath under the fume hood and heated at a low setting. One drop of cyclohexanone was careful added to the nitric acid. The presence of a brown oxide indicated that the reaction had begun, at which point the reaction tube was removed from the sand bath.

3 because this is the maximum absorbance for the iron (III) ion. The Beer's Law Plot that was graphed came out to be linear with an equation of:

The copper in this experiment was the least corroded, as was predicted. When the metals are compared to mild steel, the standard of comparison, all of them performed better, so they would all make better tanks according to the results of this experiment. The practical applications of this would be using copper to make the tanks under gas stations. For further experimentation one could investigate the discrepancy in the mild steel between trials 1 and 2. One could also investigate the effect of oxidation on how well the metals would work. There is also the possibility of investigating which metal would be the most cost effective. Another investigation that could be done would be seeing if the surface area of the samples would affect the corrosion of the

Using the same process, the equilibrium concentration of Fe3+ and SCN- in each mixture will also be calculated. After finding the equilibrium constants, the mean and standard deviation of each cuvet will be recorded using basic equations. For finding the mean, we will take the sum of all of the equilibrium concentrations and divide that by the total number of values. The standard deviation and mean can be more easily calculated by entering the data into excel and using their standard formulas.