Solubility Of Hexane Lab Report

Take two test tubes, label each test tube according to solvent. Add 1 mL of distilled deionized water to the first test tube and 1 mL of ethanol to the second test tube. Next, add 1 mL of the unknown liquid to each test tube, shake for a small period of time, and observe patiently. During this observation, you will be able to determine whether the two liquids mix completely, slightly, or not at all. If the two liquids mix completely, then you should be able to see one liquid mixed together without a visible line indicating two different substances. This means the two liquids are considered soluble. If the two liquids

Prior to beginning the experiment, it is important to understand a few different concepts such as the distinguishing physical properties of a chemical substance and how these physical properties can be analyzed. Physical properties of a chemical substance include water solubility and melting point, both of which are used to pursue identification of the unknown component of Panacetin. Water solubility is a distinct physical feature of chemical substances that can lead to an increase or decrease in product recovered. For example, the water solubility of the two possible unknowns, acetanilide or phenacetin, are different in opposite temperature spectrums. Acetanilide’s cold water solubility is 0.54 grams/100 mL of water, whereas the substance’s boiling water solubility is 5.0 grams/100 mL of water.

Our testable question was, what is the effect of different liquids on the dissolving rate of the alka seltzer. To answer this question we dissolved alka seltzer in three different liquids, and recorded the data we found. After testing water three times

As indicated in Table 1, each of the given substances for this lab were soluble in ethyl acetate. However, the solubility results varied based on the structure of each tested compound. 4-bromoacetanilide and fluorene are both insoluble within solvents of HCl and NaOH. Fluorene will stay soluble within the organic layer since its is a purely made of carbon and hydrogen. 4-bromoacetanilide will act similarly given its nonpolarity from balanced branches and lack of acid/basic characteristics. 4-nitroaniline and 2,5-dichloroaniline travel solubly into the HCl/H2O solvent when added to the separatory funnel, yet form a precipitate after a highly concentrated NaOH is added. Both 4-nitroaniline and 2,5-dichloroaniline are slightly basic organic compounds, and when an acid (HCl) is added a proton will transferred to make them ionic. In their ionic state, both compounds become water-soluble. When NaOH is added to 4-nitroaniline and 2,5-dichloroaniline, it removes the proton causing the compounds to become insoluble in water once again. The same concept can be applied in an opposite fashion to the acid organic compounds of 3-chlorobenzoic acid and resorcinol; both become water-soluble when they lose a proton after mixed with NaOH. They go back to their water insolubility if you add an acid to donate a proton back to 3-chlorobenzoic acid and resorcinol. Therefore, after completing this lab,

Samples of benzophenone, malonic acid, and biphenyl were each tested with water, methyl alcohol, and hexane. Benzophenone was insoluble in water as it is nonpolar while water is highly polar. Benzophenone was soluble in methyl alcohol, dissolving in 15 seconds, because methyl alcohol is intermediately polar as benzophenone is nonpolar. Methyl alcohol is polar but not as much as water. Thus, the nonpolar benzophenone was soluble in methyl alcohol. Benzophenone was partially soluble in hexane because hexane is nonpolar as is benzophenone. Thus, benzophenone was dissolved in hexane. Malonic acid was soluble in water because both malonic acid and water are polar. It took 25 seconds for malonic acid to dissolve in water. Malonic acid was soluble in methyl alcohol because malonic acid is polar and methyl alcohol is intermediately polar, allowing malonic acid to dissolve in the methanol in 15 seconds. Malonic acid was insoluble in hexane because hexane is nonpolar while malonic acid is polar. Biphenyl was insoluble in water as water is highly polar whilst biphenyl is nonpolar. Biphenyl was partially soluble in methanol which is intermediately polar whilst biphenyl is nonpolar, allowing it to dissolve a little. Biphenyl was soluble in hexane because both biphenyl and hexane are nonpolar molecules. Biphenyl dissolved in hexane in 10 seconds.

6. The solubility of the solids were tested using a micro tray, by placing them in water and oil to observe their polarity,

Substance A and B were weighed; Substance A weighed 0.502 g and substance B weighed 0.503 g. Both substances were put into two different test tube with approximately 8 ml of DI water into the test tub. Substance A and B were stirred and B dissolved while A did not. This shows that B is soluble in water compared to A. Thus, shows that B is soluble in water than A. The reason why B is soluble in water is because it has a higher dipole moment than A. With a higher dipole moment, it shows that it is soluble in water since it is polar and the bonds were easily broken.

Ionic compounds are soluble in water to a certain point depending on the compound. The level of solubility changes among different compounds. Some ionic compounds can completely dissolve in water and appear to be a homogeneous mixture. Although, some ionic compounds dissolve very little, and could be considered insoluble, since it does not dissolve fully. Depending on the compound, the level of solubility can be high or low. However, ionic compounds could dissolve to a certain degree. If the solution appears to be a heterogeneous mixture, many may assume through visual representation that it may be insoluble. As stated previously, the smallest amount of solubility should be considered. To confirm whether or not the substance is soluble, observe the efficiency when conducting electricity. Due to practical reasons, the slightest solubility could be considered insoluble by people.

After the initial mixture has refluxed, 9.11 grams of benzophenone was dissolved in 100 mL of anhydrous ether in a beaker and was then transferred into the separatory on the reflux apparatus. This solution was then added to the Grignard reagent at a drop wise rate while stirring. After the benzophenone was added, the mixture was then refluxed for 15 minutes on a heating mantle.

The experiment recrystallization was divided into two parts. In the first part, the purpose was to find the solubility of the four compounds, anthracite, resorcinol, benzoic acid, and 4-amino-1-napthalenesulfuric acid using three different solvents, water, toluene, and n hexane. Further, Phthalic acid and benzoin were recrystallized.

The purpose of this lab was to study colligative properties. These properties are properties that are affected when a solute is added to a solvent. Thus, the amount is important, not the actual type of substance, for the colligative properties. A couple types of this property are the freezing point and boiling point of a substance. (1)

Practically insoluble in ethanol, ethanol (95%), ether and water, slightly soluble in benzene and warm ethanol (95%)

In week one we performed a qualitative solubility test of our fats and oils, synthesized our soaps and detergents, and performed a solubility test and lathering test for the soaps and detergents. We wanted to test the solubility of our starting materials of the soap making process to understand the properties of the materials. In our initial solubility test of the starting materials, we found that most of the materials were insoluble. As you can see in Table 2.0, olive oil and vegetable oil were only soluble in toluene and the shortening and lard were only partially soluble in acetone. In order to understand the solubility of the soaps and detergents, after our synthesis and filtration, we performed a qualitative solubility test with each of

1. Obtain a sample of the mixture. The mixture you will separate contains three components: NaCl, NH4Cl, and SiO2. Their separation will be accomplished by heating the mixture to sub-lime the NH4Cl, extracting the NaCl with water, and drying the remaining SiO2.

Solubility:- Slightly soluble in 5% w/v sodium hydroxide solution; practically insoluble in water, dilute acids, and most organic solvents.