Salt Separation Lab Report

The purpose of this lab was to determine the limiting reactant in a mixture of to soluble salts and the percent composition of each substance in a salt mixture.

There are various techniques to separate a mixture of compounds from each other. One of the commonly used way to isolate compounds from a mixture of two compounds is called extraction. This method of extracting two compounds from each other relies on the different solubility of the compounds in two different solvents.

The purpose of this particular lab was to experiment and identify the chemical and physical changes throughout the experiment.

Three grams of a mixture containing Benzoic Acid and Naphthalene was obtained and placed in 100 ml beaker and added 30 ml of ethyl acetate for dissolving the mixture. A small amount (1-2 drops) of this mixture was separated into a test tube. This test tube was covered and labelled as “M” (mixture). This was set to the side and used the following week for the second part of lab. The content in the beaker was then transferred into separatory funnel. 10 ml of 1 M NaOH added to the content and placed the stopper in the funnel. In the hood separatory funnel was gently shaken for approximately one minute and vent the air out for five seconds. We repeated the same process in the same manner one more time by adding 10ml of 1M NaOH.

The volume and the boiling point of each collected sample was recorded in a table (for Fractions A, B, and C). The data in the table was converted into a graph (both of which are attached to the back of the report). There is, like in all experiments, an ideal set of data. In this experiment, if the distillation for the unknown mixture (which has two compounds) was done properly, the temperature vs. volume graph should show two plateaus for temperature. (See hand drawn graph attached on back). We look at the plateau temperatures because they are essential to find out what the unknown compounds are. This is because the plateau temperatures show us the boiling point ranges for the unknown compounds. In addition, as shown in the table and calculations attached to back, the volume of the collected sample can be utilized to figure out a ratio of the compounds. But, of course, since ideal and pure samples were not collected, the ratios that are calculated are just estimates. There is one plateau for the boiling point of both lower and higher boiling point compounds. The lower boiling point plateau comes first. The transition phase that occurs between the first and second plateaus was collected. This transition phase represented the mixture of the two compounds in the experiment. If the experiment yielded ideal results, sample A would show to be consisted of primarily the lower boiling point compound. This would be the case up to the point when the temperature is raised to match the boiling point of the higher boiling point compound. The compound is sample C. During the experiment this sample was gathered in a falcon tube. But there is some error in my results. Some of the reasons why there was error in the experiment are stated. I boiled Fraction A for too long, the boiling rate was too high, or a combination of these errors occurred. If the boiling rate is too fast, the side arm will heat up as the

Because salt dissolves in water, we added water to the salt and sand mixture. Sand is insoluble in water making the sand not dissolve. The mixture containing of sand and salt water was then filtered with filter paper. The filter paper allowed the salt water to pass through because it is a liquid while not allowing sand to pass through because it is a solid. The salt water was then collected in a pre-weighed 250-mL (67.88 gram) beaker while the sand and filter paper was put in a pre-weighed (52.02 gram) 100-mL beaker. The water was then evaporated because we left both beakers to dry overnight.

The purpose of this lab is to separate a mixture and determine the percentages of each of the ingredients. Each substance will have a different boiling point due to its intrinsic properties and from that, we will be able to determine the purity of different products as we evaporate off the next level of product.

Table 2: Consists of color extract taken from a red cabbage for a natural indicator. The pH reading that was measured by using the pH meter and the result of the pH reading to determine whether the solution was acidic or basic.

After reading the lab instructions - but before starting the lab - record your best “educated guess” about what will happen in the experiment. What hypothesis can you generate about the effect of adding salt to water?

In Rosemary Jolly's class, students performed the hot plate procedure in order to evaporate the water from the unknown hydrate.  The equipment that the students used were two 100-mL beakers, an analytical balance, a hot plate, and a clean glass rod to stir the substance.  Students obtained about 1 or 2 g of the unknown hydrate into one of their 100-mL beakers.  They determined the combined mass of the sample and the beaker.  After doing this, they placed the beaker onto a hot plate that was on a medium setting.  Using the glass rod, students stirred their beakers in order for all of the unknown hydrate to melt until a dry powder appeared.  Once the dry powder appeared in the beakers, the students took their beakers off of the hot plate in order to cool to room temperature.  They placed the beakers on an analytical balance to record the mass of the beaker and residue.  This information was used later in the experiment to find the number of moles of water per formula weight unit of magnesium sulfate.  Students repeated the procedure with their second 100-mL beaker.  Once the second trial was completed, they used their data to determine the average number of moles of water present in the magnesium sulfate

Corresponding to the previous experiment, this week’s experiment measures the participants’ ability to conduct basic, fundamental laboratory procedures. These procedures revolve around scientific measurements of volume, mass, and density. Unlike last week’s activity, this week’s experiment had a few modifications. In addition to distilled water, saltwater and an unknown substance were added. There was a total of five substances to choose from; Hexane, Methanol, Ethyl acetate, Ethylene glycol, and Dichloromethane. Part C, the unknown liquid number was four, which the average density was 0.789 gmL-1, and from looking at the chart the unknown identity was methanol. Part A, the temperature of the water was 20 oC, which was in front of the class,

The purpose of this separation of a mixture lab is to give students the challenge of figuring out how to separate a provided mixture, and following through with their procedure. The mixture is composed of salt, sand, poppy seeds, and iron filings, and all of these components should be separated and dried as well as possible by the end of the lab.

This is done through a change in temperature. Over time, two objects that are in direct contact will

The hypothesis stated that, firstly, the materials could be sifted through the sieve. Secondly, the iron filings could be separated from the mixture. Thirdly, that the salt would be removed from the mixture, through dissolving and evaporation. Fourthly, the polystyrene beads could be removed in the dissolved mixture. Finally, the salt mixture could be separated, using evaporation. The reason why iron filings come first is because magnetism is a quick and easy method to separate the iron filings, meaning that it could be separated straight away, so it’s out of the way. The salt is dissolved next because the rest of the mixture in insoluble, meaning it is unable to be dissolved in water. Dissolving salt, here, means that the other

The hyphotesis created for this experiement was accurate. Each element received a different reaction for each of the tests. No test had a similar outcome for both Iron or Sulfur. The reaction always proved to be quite different and even the oposite. Iron reacted to magnet, mixed with the substances while Sulfur did not react with the magnet nor did it mix with either water or M Hydrochloric Acid. This experient however could have had a couple of mistakes. The measurments werent exact ones. It would be impossible to do so everytime and the amount of substance or elements would always be a little off.