Separate the sand by boiling water and pouring the water off, then move on to separating the Benzoic acid using filter paper. Lastly separate the salt out by allowing the water to evaporate from the solution. Data Tables: Data Table 1: Experiment Data | | Grams | Percent of mixture | Iron filings | 1.5g | 24.6% | Sand | 1.6g | 26.2% | Table salt | 1.8g | 29.5% | Benzoic acid | 1.2g | 19.7% | Total | 6.1g | 100% | Questions: A. I proposed the magnet would remove the iron from the mixture. I thought the sand might be removed by filtration. I thought distillation would remove the salt.
One student did not stir the mixture before decanting the water a. This error could cause the percent of sand calculated to be too high. When the mixture is stirred it allows for the sand and salt to separate away from each other enough for the salt to be dissolved and the sand to sink to the bottom. If it is not stirred correctly the salt may not fully dissolve leaving it mixed with the weight of the sand you are using to calculate the percent. b.
In order to remove the iron filings I will use the iron bar since it the composition of iron will be picked up by the magnet. Then I will bring the water to a boil in order to only remove the sand. After, I will use the ice bath to remove the benzoic acid. After removing all other solids I will be left with only the sodium chloride in the water. Results: Please see attached the final results and questions to go with Lab #3.
It was also because we had to take two measurements (one for diameter another for height)...which could possibly create more mistakes. Furthermore, you need to multiply diameter and height to get to the volume, so any one of those reading had a mistake, the error would compound and get worse. The same is not true with measuring with graduated cylinder, which is just a one shot reading. If that reading is off a bit, it won't impact the density as much 2- Did you find that density was intensive or extensive? Explain A- It was intensive.
If you have a mixture of tennis balls and marbles (not pure substances by the way), it would be easy to separate the mixture. However, it is more difficult to separate a sand (also not a pure substance) and salt mixture. Even with very good tweezers and a magnifying glass, it would be extremely tedious. You could take advantage of the fact that salt dissolves in water and sand does not. To separate iron powder from an iron and sand mixture you can take advantage of the magnetic properties of iron and separate the mixture.
Experimental Data: The original weight of the mixture before separation was 4.6g. After separation the weights were as follows Grams Percent of mixture Iron Filings 1.4g 33% Sand 1.2g 28% Table Salt 0.8g 18% Benzoic acid 0.9g 21% TOTAL 4.3g 100% IV. Observations: The easiest part of this experiment was separating out the iron filings. With the magnet they separated out pretty easily. When almost boiling the sand, salt, and benzoic acid it didn’t seem like it was working.
LIQUID-LIQUID EXTRACTION OF BENZOIC ACID J Wright Organic Chem Lab 1 Tuesday 1:40-5 Ian Stubbs LIQUID-LIQUID EXTRACTION OF BENZOIC ACID PURPOSE: The purpose of this experiment was to extract benzoic acid from an aqueous of benzoic acid using methylene chloride, use liquid-liquid extraction to calculate the distribution coefficient of benzoic acid and to determine whether a single extraction or multiple extractions are more efficient. Add in the table of physical constants. See the attachment for the lab format. PROCEDURE: Gather a two stock solution that includes; 0.02M of sodium hydroxide (NaOH) aqueous solution and 0.02M of benzoic acid aqueous solution. For a single extraction, use a 50mL graduated cylinder and measure out 50mL of the benzoic acid solution into a 125mL separatory funnel.
The slit acted as the only means of escape for the particles. The slit was pointed at the think gold foil. The foil was set up a short distance from the source, and in a line with the opening in the lead block. using the foil as the center, they took a long strip of material that was coated with zinc sulfide and set it up in an almost complete circle. Then they turned off the light.
| Gravimetric Determination Nickel in Steel | | 10/15/2013 Fall 2013 | | Objective The purpose of the laboratory is to determine the percentage of nickel (Ni) in the steel alloy. Introduction There are numerous types of steel alloys with different chemical compositions and weights. Some steels are simple in composition, like a steel with 99% iron (Fe) and only 1% carbon (C). However, there are other steels that vary greatly in composition. For the laboratory an unknown steel was used and the nickel content was determined using a gravimetric method and by exploiting the chemical properties of the compounds and solutions.
When the solution is acidified during diazotization to form nitrous acid, the sulfanilic acid is precipitated out of solution as a finely divided solid, which is immediately diazotized. The finely divided diazonium salt is allowed to react immediately with dimethlaniline in the solution in which it was precipitated. Mechanism Diazotization: [pic] Diazo Coupling: Methyl orange is often used as an acid-base indicator. In solutions that are more basic than pH 4.4, methyl orange exists almost entirely as the yellow negative ion. In solutions that are more acidic than pH 3.2, it is protonated to form a red dipolar ion.