Separation Of Mixtures Essay

Gather materials (beaker, 100 milliliters of copper chloride, graduated cylinder, funnel, 2 centimeter by 15 centimeter aluminum foil strip, goggles, gloves, apron, hydrochloric acid, and a spoon to push down the aluminum foil so that it doesn’t rise up and drip copper chloride down the side) 2. Pour 100 milliliters of copper chloride into the graduated cylinder to measure it 3. Pour the copper chloride into the beaker or leave it in the graduated cylinder (whichever you want to conduct the experiment in) 4. Fold the tin foil in half the long way so that you have 1 centimeter by 15 centimeter strip of aluminum foil 5. Curl it into a coil/spring 6.

when the pH is 7, allow the solution to cool to room temperature. f. Add about 50 ml water to the solution and stir it. Filter the pale blue precipitate in a Buchner funnel.it is observed that the mixture filters slowly, the way to solve the little problem is to stir the precipitate with 50 ml more water. Wash the precipitate with water followed with alcohol. Place the mixture in a petri dish and let it dry in an oven at 140 ˚C for six hours.

There is one mole of OH- in the solution since NaOH goes to Na+ and OH-. Trial 1: 25.65mL NaOH x 0.100mol/1000mL = 2.57 x 10-3 mol NaOH = 2.57 x 10-3 mol HA = 2.57 x 10-3 mol H+. The equivalent mass is 0.356g Acid / 2.57 x 10-3 mol H+ = 139g/mol H+ Trial 2: 49.57mL NaOH x 0.100 mol / 1000 mL = 4.96 x 10-3 mol NaOH = 4.96 x 10-3 mol HA = 4.96 x 10-3 mol H+. The equivalent mass is 0.644g Acid / 4.96 x 10-3 mol H+ = 130.g/mol H+ Average =

The appearance after this period resulted in another color change back to white. The crucible, lid, and hydrated copper sulfate was weighed again to calculate the mass of water lost by dehydration (described in table 1.3). This was done by subtracting the final mass by the initial mass of the crucible, lid, and compound. The mass of the crucible would remain unchanged while the mass of the compound would be altered. This trial was repeated 3 times and 1 extra set of data was taken from 2 separate groups to include

Using method 2, the product appear as white crystals. Given that the yellow color remain throughout the product in method 2, too much aldehyde was added. It was predicted that this was the source of error because aldehyde was a yellow liquid. In this experiment, 293 mg of aldehyde was weighted for method 1 instead of 250 mg and.

We used a Buchner funnel to collect benzocaine. We used three 10 ml of water to wash the product. After the product was dry, we weighed, calculate the percent yield and determined the melting point of the product.

This experiment was to weigh the magnesium then wrap it with copper and to put it in a beaker with full of water in order to get the hydrogen gas. In the first trial the reaction happened real quick, this could be due to over using magnesium and it could have been improved by using less magnesium. But the rest two trials, they were pretty much ok. The figure shows that, ratio between H2 and Mg is 1:1 which means that there are equal molecules in both of them. Since the answer has to be four significant figure, the average molar mass of magnesium is 23.85

Dry the evaporating dish. Wait for the dish to cool off then weigh it with the product. Mass of copper wire .2654 g Sodium Hydroxide 45mL Sulfuric Acid 25mL Zinc 3.0g Hydrochloric acid 15mL Methanol 10mL Acetone 10mL Calculations

sp3 O-H stretch, about 3200-2500 cm-1 (b, m); sp3 C-H stretch, 2991-2868 cm-1 (sh, m); sp2 =C-H stretch, 3100-3000 cm-1 (sh, w); sp2 C =

The purpose of the K_a determination of an unknown weak acid lab was to use titration in order to determine the K_a for an unknown solid weak acid knowing only its molar mass. The previous laboratory experiment was performed in order to determine whether titration or dilution would yield more accurate K_a. It was determined that titration yielded more accurate results. This lab was performed by taking a sample of solid weak acid and dissolving it in water before titrating with the strong base NaOH. Titration is a technique in which a reagent of known concentration is slowly added to an unknown solution in order to calculate the concentration of the unknown.

50 μL of these dilution solutions were separated on the TLC plate coated with SNISG. The plate was developed with petroleum ether: ethyl acetate (4:1) and the movement of solvent was usually controlled at 1 cm from the upper edge. After completion, the plate was dried until no solvent smell remained. It was sprayed with an ethanol solution containing 10% sulfuric acid, and heated at an infra-red drier until obvious color came up, as shown in Fig.2 (B.ab). Simultaneously, the amount of silver nitrate in the impact of isolative effect was investigated with the sample procedure, as shown in Fig.2

value*100%. When it came to the results, the calculated percent error was 6.65% for sand, 0.60% for wood,1.57% for plastic, 3.13% for metal,

One sample had 250ng of plasmid A as well but with no enzymes added. All the digestions tubes were incubated at 37℃ for 30 minutes. After incubation, 5μL of loading buffer (30% glycerol, 10 mM Tris-HCl, pH 8, 1 mM EDTA, 0.025% bromophenol blue) was added to each sample. 50 ml of molten agarose (1% agarose boiled and cooled to 55℃ with added SYBRsafe) was poured into the casting tray for gel electrophoresis.

Problem: How can you separate beads, iron, salt, and sand into four piles of separate substances? Hypothesis: Materials: Mixture (Beads, Iron, Salt, Sand) Digital Scale 8 Dixie Cups as Containers(a,b,c,d,e,f,g,h) Plastic Wrap 1 short box Clear packing tape

The purpose of this lab is to use the Diels-Alder reaction to combine anthracene and maleic anhydride. Named after its two founders the Diels-Alder reaction is the addition of a conjugated diene (electron rich compound) with a dienophile (electron poor compound). (1) These compounds will be combined using [4+2] cycloaddition, where the numbers 4 and 2 come from the number of π electrons that are used in each compound to synthesize the product. (2) This experiment comes at the cost of losing two π bonds to form two new sigma (σ) bonds in the cyclic compound. (2)