Powders Lab Report

The reactants in our lab were aluminum foil and copper chloride solution. The products were aluminum chloride and copper. A change in properties demonstrates that a chemical reaction occurred. One property that changed was the colors. Initially the aluminum foil was a shiny silver, and the copper chloride was a green-blue liquid. After we placed the aluminum into the copper chloride solution, the liquid clouded up a lot and turned to a light grayish hue. There were solid pieces produced that were a dark reddish color. This change in color shows that there must have

When we placed the aluminum foil in copper chloride, a chemical reaction occurred. Before the reaction took place we had aluminum foil and copper chloride as our reactants. After the reaction happened, the products were aluminum chloride and copper. After the foil was placed in the copper chloride, the color of the aluminum foil had changed from a shiny silver, to a deep red. Also, the color of the copper chloride changed from a light blue to a murky green. At the start, there was aluminum and copper chloride. During the reaction, the aluminum and copper chloride atoms rearranged to form aluminum chloride and copper as two separate substances, also being different substances than the ones that we started out with. A chemical reaction is when

The absorbance was set to 0 Abs while the spectrometer was set to ʎmax (from Part A). In Part B, 1.00 ml of the solution was mixed with the Blue dye in the beaker and half-way covered with a cuvette. Concurrently, the Spectronic 20 was blanked with water. The processes detailed above were repeated, each at a time. The absorbance values were recorded for 11 minutes.

I think that these properties were not tested because it would have taken much longer to check the mass, and boiling point. Testing for the scent of each of the powders may haven’t been much of a help as they probably all smell very similar. Also, we don’t have a stove top in the science classroom so checking the boiling point would be difficult. Another reason as to why that we didn’t check mass is because it would have been difficult to get the exact same amount of each substance for the measurements would be accurate. Finally, all those physical properties would result in quantitative measurements and we didn’t include any other quantitative measurements in this

1. What type of macroscopic evidence for chemical change did you observe during this experiment? Give at least three different examples.

In order to do this experiment we had to prepare by buying our supplies, and follow some safety steps. We had to use some safety gloves when handling soda ash because if we ate after handling it we could of gotten very sick. Also any supplies that came in any contact with the soda ash couldn’t be used for food after. Also we had to buy different types of fabric, cut them into 20 by 20 cm squares and label them. We had to buy some dye in order to find out how each fabric reacted to it. We used three squares of each of out five fabrics, our fabrics were cotton, linen, poly cotton, polyester, and nylon. Then you had to wash them in the washing machine for approximately thirty- eight minutes, with one fourth cup of Tide Simply fresh and Clean detergent, Then the materials dried over night, for the best results.

When sodium was added to water, the sodium melted to form a ball that moved around on the surface of water rapidly and hydrogen gas was produced. Because of the amount of heat liberated during this exothermic reaction, the hydrogen gas ignited the sodium with an orange flame while floating on the water. Also, when potassium was put onto the water, the observation was similar to how sodium reacted towards water. The metal was also set on fire, with sparks and a lilac flame. But, in the case of speed of tarnishing between the two elements, potassium was faster than sodium. It dissolves completely in water quicker than sodium.

In the “Blast Off” lab, we had launched a foam rocket into the air by pumping air into a nozzle, shooting the rocket up, and then recording the time from launch to when it hit the ground. I have learned and now understand the mechanics of kinetic and potential energy.

In this lab, the hypothesis, if a chemical reaction occurs, there will be signs of a chemical change such as a change in temperature, color, and/or smell, was accepted. In each experiment, clear signs of a chemical reaction were observed. In chemical reaction #1, we put drops of vinegar onto a small pile of baking soda. The baking soda and vinegar produced bubbles of gas right as the first drop hit the baking soda, which is a clear sign that there was a chemical change occurring. This can be classified as a double replacement chemical reaction. In chemical reaction #2, a visible color transformation was seen when the ammonia was added to the grape juice. Although in some cases a basic color change could be a physical change, the vinegar chemically

The purpose of the “Titration of the Unknown Acid” lab is to determine how much of a given material known as concentration is in a substance or mixture. In this lab, the student also learns the technique of using titration. The concentration of the acid we used in class will be sampled with a standardize solution such as sodium hydroxide with an environmentally indicator to show the physical change of color that occurs to the solution by the acid. The equipment necessary for the titration experiment follows: 0.1M NaOH, Acid solution, Anthocyanin (which is found in red cabbage leaves) indicator, Burets, Ethanol 95% and DI water. First Professor Greenberg assign a labeled unknown acid solution, then we recorded the solution’s identity and bottle code. Next, we obtained an Erlenmeyer flask for the titration. Rinse it with DI water. Next we are to dispense from the buret at least mL of the designated acid into the flask. Record the initial and final volume readings on the buret in laboratory notebook data table. Next we add 20mL of deionized water and anthocyanin indicator drop

In this experiment we took an original mixture and split into three components. By decanting and dissolving materials we were able to find the percentages of each material in the original mixture. From the results we found Sand and NaCl to be the majority of the mixture, however in reference to the Law of Conservation of Mass, we found a slight discrepancy in the final results.

Solubility is the property of a solute to dissolve in a solvent to form a solution. Pouring and mixing the powders in water will test their solubility. A highly soluble powder will dissolve in the water without leaving an traces of solid powder. A less soluble powder would somewhat dissolve, but remains of the powder would gather on the bottom of the container.

The purpose of this experiment was to see if altering the ingredients of a bath bomb affected the effervescent when placed in water. When a bath bomb is submerged in water the ingredients caused it to fizz, releasing a scent and changing the color of the water. This bath bomb experiment requires two recipes. The first recipe which was labelled as “normal”, contained less cornstarch than the other recipe. In addition to the “normal” recipe, the other recipe was labelled “extra” because it contains more cornstarch. During this process, by adding or subtracting ingredients the fizziness of the bath bomb changed. If more cornstarch is added to the recipe, the bath bomb will not fizz as much when placed in water. This is because the cornstarch

During the Tang Dynasty in China, around 850 AD, alchemists working on making a concoction to make human beings immortal, accidentally created Gun Powder that they called “huo yao”. This was a mixture of Saltpetre (Potassium Nitrate), Charcoal and Sulphur that was gradually tuned in a ratio of 75%, 15% and 10% respectively. The Chinese employed this newly invented mixture in arrows, primitive grenades and mines to terrorise the Mongols as early as 904 AD. They tried to conceal this invention but eventually the secret formula was exported via the Silk Route to India, Middle East and Europe, leading to new weapons being introduced (Szczepanski).

In this experiment, chemical reactions take place in cells and are responsible for all the actions of organisms. Chemical reactions can consume energy (endergonic) or release energy (exergonic). Together, these reactions make up an organism 's metabolism. The chemicals taking part in these reactions are called metabolites.