A variety of extraction methods were employed in order to separate a strong acid, a weak acid, a strong base and neutral compound from solution. This is possible due to the presence of different functional groups in the organic mixture, which each provide distinct chemical properties. These individual properties are what allow the extraction of each compound. How these properties pertain to solubility is key to the separation of these compounds. Originally, the four-component mixture was placed in a flask and dissolved in an ether solution. The first step to this experiment was separating the strong acid from the rest of the solution. After being transported to a separatory funnel, saturated NaHCO3 was added to the ether solution. CO2 was subsequently removed from the mixture by shaking the contained mixture, then releasing the …show more content…
This was done by carrying out the same procedure outlined above, just using NaOH instead of NaHCO3. The resulting liquid was labeled NaOH Extract, and set aside. Similarly, the base was extracted with the same technique, using HCl instead of NaHCO3. This solution was labeled HCl Extract, and set aside. Following the aforementioned procedure, the neutral compound was to be isolated from the ether solution. Moved to a clean flask, the ether solution was introduced to anhydrous sodium sulfate. After letting the mixture sit for about 10 minutes, the mixture was decanted into a new beaker. The ether in this final mixture was allowed to evaporate, leaving behind the neutral compound. Percent recovery was recorded and the compound was transported to a vial. Then, the weak acid was isolated from the NaOH extract. After cooling the mixture, HCl was pipetted into the flask, neutralizing the NaOH. This enabled the, now precipitated, weak acid to be filtered out of the solution. After vacuum filtration was used to remove the solid acid, percent recovery was recorded, and the weak acid was moved to a
The purpose of this experiment was to learn and preform an acid-base extraction technique to separate organic compounds successfully and obtaining amounts of each component in the mixture. In this experiment, the separation will be done by separatory funnel preforming on two liquids that are immiscible from two layers when added together. The individual components of Phensuprin (Acetylsalicylic acid, Acetanilide, and Sucrose as a filler) was separated based upon their solubility and reactivity, and the amount of each component in the mixture was obtained. Also, the purity of each component will be determined by the melting point of the component.
Experiment: First prepared a well plate with the appropriate amounts of distilled water, HCl, and Na2S2O3 in each well according to the lab manual. The well where the reaction
In this experiment, a mixture of three substances (benzoic acid, 2-naphthol, and 1-4 dimethoxybenzene) will be separated based off acidity strength using the liquid-liquid extraction technique through a separatory funnel. Benzoic acid and 2-napthol will be converted into ionic salts when reacting with their appropriate bases (sodium bicarbonate and sodium hydroxide). Both ionic salts will then form solids through the addition of acidic HCl. Neutral 1,4 – dimethoxybenzene forms a solid through the evaporation of ether. Each compound will then be purified through recrystallization, using the processes of dissolving the solid in either water or methanol, and isolating the solid through vacuum filtration. After a week of evaporation, the compounds will then be examined for both
The objective of this experiment was to perform extraction. This is a separation and purification technique, based on different solubility of compounds in immiscible solvent mixtures. Extraction is conducted by shaking the solution with the solvent, until two layers are formed. One layer can then be separated from the other. If the separation does not happen in one try, multiple attempts may be needed.
As shown in Fig. 5, the final pH of the NaClO-NH3 solution after simultaneous removal are 5.4, 6.9, 7.2, 7.5, 8.5, 9.6, 10.7, 11.5 and 12.8 with respect to the initial pH of 5, 6, 7, 8, 9, 10, 11, 12 and 13, from which, an interesting law can be concluded as that if the initial pH is an acidic, the final pH is slightly increased; but if the initial pH is an alkaline, the final pH is declined. NaClO-NH3 is macromolecule compounds with a large inter surface area. It contains abundant functional groups such as hydroxyl (OH), carboxyl (COO), quinone, amino (–NH2), etc, which determines that NaClO-NH3 is a salt of strong base and weak acid, as well the ionization equilibrium and hydrolytic equilibrium would be complicated. When the pH of the NaClO-NH3 solution was acidic, the functional groups such as OH, COO and NH2- would react with H+ to generate the NH3 sediment, resulting in a decrease of inter surface area owing to the block and a great loss of NaClO-NH3, then the NOx removal as well as the duration time was decreased. As for the increase of the final pH in the acidic conditions, this was a result of the consumption of H+ by NaClO. The decrease of the
Apparatus: * 1 measuring cylinder * 1 test tube * 1 stop clock * A large gelatine cube containing indicator and NaOH * Hydrochloric acid ranging from 1-3 molars * A scalpel Diagram: Method: * Take the large gelatine cube and cut into 15 equal pieces * Place on piece of the cube into the test tube * Measure out 10mls of HCl in the measuring cylinder * Pour the HCl into the test tube with the gelatine cube and start the clock * Time how long it takes for the pink colour inside the gelatine cube to completely disappear * You will also notice that the cube dissolves slightly * Record your results and repeat this same process 3 times for each molar of acid: § 1 molar § 1.5 molar § 2 molar
The advantage of these compounds is they all look vastly different and telling them apart from one another and see if they are disappearing was no problem. This was used this to advantage right away; added water to compounds and saw, as predicted, the NaCl become soluble while the other two compounds remained insoluble. This is where the hypothesized NaHCO3 would dissolve the Acetanilide. Initially frustrated by failure as the solvent failed to perform as predicted, but noticed the M-Toluic Acid rise to the top of the solution, rather than starting over improvisational thought arose and manual separation of the M-Toluic Acid off the top of the solution proved quite successful. Then dried both compounds and weighed them. A parallel experiment using acetone in place of NaHCO3 was also being performed. This dipolar aprotic solvent would have been ideal in this experiment as M-Toluic Acid was soluble in it at a raised temperature but because of time constraints (and high moral after finding 98.8% accuracy) the path was abandoned.
Base being Baking Soda, or Sodium Bicarbonate, and the acid being Vinegar, or Acetic Acid for a control. I measured 10 ml. of Vinegar, dumped that into a two inch high glass jar, and wrote down the pH level. Then I measured o...
Acid-Base Titration I. Abstract The purpose of the laboratory experiment was to determine equivalence. points, pKa, and pKb points for a strong acid, HCl, titrated with a. strong base, NaOH using a drop by drop approach in order to determine. completely accurate data. The data for this laboratory experiment is as follows.
Materials and Methods: An ion exchange chromatography column was obtained and set up for purification with the addition of 0.5 ml ion exchange matrix. 1 ml
Acid-base liquid-liquid extraction was done to separate the individual components of Excedrin so that caffeine could be extracted. Acid base liquid-liquid extraction works by converting an acid or base to the alternate form by adding a strong acid or base, which allows it to become more polar and move between solvents. The solvents can then be extracted off, allowing for the individual components to be extracted. This is important for organic chemists, because being able to separate components allows for reactions to take
Initially, before any NaOH is added, the pH of H2C2O4 .2H2O is low because it contains mainly H3O+. The starting pH will, however, be higher for a weak acid, like H2C2O4 .2H2O, than for a strong acid. As NaOH is added, H3O+ is slowly used by OH- because of dissociation of NaOH. The analyte remains acidic but the pH starts to increase as more NaOH is added.
Neutralization Experiment AIM:- To investigate how heat is given out in neutralizing sodium hydroxide (NaOH) using different concentrations of Hydrochloric Acid. Background Information:- Substances that neutralize acids are called alkalis. An acid is a substance that forms hydrogen ions (H+ ) when placed in water. It can also be described as a proton donor as it provides H+ ions. An example of an acid is hydrochloric acid (HCl), Sulphuric acid (H2SO4) etc.
The drug ingredients used in drug manufacture are usually aqueous salts that are prepared using strongly acidic or basic hydroxy-acids salts and counter ions, which possess a h...
The purpose of this experiment is to use our knowledge from previous experiments to determine the exact concentration of a 0.1M sodium hydroxide solution by titration (Lab Guide pg.141).