Composition of Potassium Chlorate

In the hood, place the copper wire in 10mL of nitric acid and wait for it to dissolve. Afterwards, add 100mL of deionized water to the solution and boil the solution, so all the nitrogen oxides are removed. Place the solution to a 250.0mL volumetric flask and add deionized water to the flask until the solution is 250.0mL. When the solution in the flask is at 250.0mL place the solution in a clean plastic bottle. Now cut a penny into four pieces, and measure the mass of all the pieces together. Go back to the hood, and place the pieces of the penny into a 250mL beaker. Afterwards, add 20mL of concentrated hydrochloric acid. Wait for the hydrochloric acid to dissolve the zinc core. When the zinc has dissolved, filter the solution through the filter paper, and place the copper metal pieces into a clean 150mL beaker. In the hood, place 4mL of concentrated nitric acid in the beaker, and when the copper dissolves add, one drop at a time, 30mL of 6 M ammonium hydroxide to neutralize the nitric acid. Transfer the copper/ammonia solution to a 100.00mL volumetric flask. Prepare four different calibration

First I will set up the apparatus as show above. I will add 1.5 grams

The first step that needed to be done in this experiment was adding hydrochloric acid (HCl)

1 litmus paper, red - in bag 2"x 3", Copper (II) Carbonate in Vial, 1/2 Full

Using elemental analysis to determine the percent mass composition of each element in a compound is the first step in creating an empirical formula. There are many different types of elemental analysis, but in this experiment gravitational analysis and Beer’s Law are used. Elemental analysis is first used to find the moles of each element, then converted to mass, and then the percent mass of the element in the product is found (2).

Turn on the gas burner and bring it a low heat, only to the point that there is a blue flame. Carefully push the gas burner under the crucible and heat for around two minutes in order to properly rid the crucible of any bacterias or other impurities that may affect the lab.

Finally, place the 96 well plates in a CO2 incubator (37ºC) for 24 hours and read on a florescent

The wet, crude product was placed into the 50 mL Erlenmeyer flask. Small amounts of CaCl2 were added to dry the solution. The flask was sealed and the mixture was swirled and left to settle. Once

2. Measure out 25 to 45 grams of one of the four metals on the trough. This may require several "clicks."

To begin, we formulated a method in which each unknown substance and compound were compared to find their molar relationships. In the experiment we calculated the molar mass of every compound by determining the amount of moles per gram in each element using the periodic table and then added them together. We then

Heat crucible and lid to redness, cool it, and determine and record its mass to the nearest 0.01 g. 2. Place powdered hydrate in the crucible, but leave it slightly ajar. 3. Gently heat the covered crucible to avoid spattering. When there is no further tendency to spatter, strongly heat the crucible for about 5 minutes.

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.

First we placed the evaporating dish on the wire to preheat for 3 mins. Next, we used tongs to transfer the evaporating dish and allowed 5 mins to cool and took the mass afterwards. After that, we added approximately 2g of MgSO4 crystals to the evaporating dish and found the mass. We then placed the dish on the burner for 10 mins, allowed it to cool found the mass. Next, we heated the dish again for 7 mins, allowed it to cool and found the mass. Lastly we burned until there was a constant

1. 10 drops of 1 M K2CrO4 was added to the solution and stirred for about 10 minutes.

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.