Solubility is the property of a solid, liquid or gaseous chemical solute to dissolve in a solid, liquid or gaseous solvent to form a solution [1]. The solubility of a particular substance is dependent on the physical and chemical properties of both the solute and solvent [1]. The temperature, pressure and pH of the solution also has an effect on the solubility. The extent of the solubility of a certain solute in a particular solvent is measured as saturation, where adding more solute will not increase the concentration of the solution and will precipitate the excess in the solution.
Phase transfer reagents are used to facilitate movement of a reactant from one phase to another [2]. For example, from the aqueous phase to the organic phase.
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The two compounds that showed benzoic acid as soluble was acetone and ethanol and benzoic acid did not appear to be soluble in hexanes or water. Acetone dissolved the benzoic acid at both room temperature and increased temperature, while benzoic acid in ethanol was only slightly soluble at room temperature and completely soluble at increased temperature. Acetone is a ketone, which is a carbon chain with an oxygen attached to it [1]. Ethanol is an alcohol; it is an ethyl group with a hydroxyl group attached to it [1]. Water is a covalent compound and hexanes is an alkane with a mixture of isomers of carbon-6. When comparing the functional groups and structures of the different solvents, the ethanol and acetone contain non-polar carbon chains with polar branches, while water is a completely polar molecule and hexanes contains no dipole moments. The non-polar carbon chains of the acetone and ethanol interact with the aromatic ring of the benzoic acid and dissolve the compound. The benzoic acid dissolved in acetone easier because the polar atom is in the center of the carbon chain rather than the side. The ethanol required heating because the increased kinetic energy of the solvent molecules broke apart the bonds of the solute easier. Ethanol would be the best for recrystallizing benzoic acid because you want a solvent in which the solute is insoluble at room temperature and soluble at high temperatures. The benzoic acid can be dissolved at high temperatures and slowly precipitated out to leave impurities in the solvent, resulting in pure benzoic
barbier reaction: In a 50 mL round bottom flask that had a reflux condenser attachment, saturated ammonium chloride (5 mL), THF (1 mL), zinc powder (0.4 g), benzaldehyde (0.500 mL, 0.5225 g, 4.92 mmol), and allyl bromide (0.470 mL, 0.6533 g, 5.40 mmol) were charged with stir bar and stirred at room temperature for 45 minutes. Diethyl ether (10 mL) was added to the reaction mixture and stirred. The mixture was gravity filtered into a beaker that was topped with a watchglass. The filtrate was transferred to a separatory funnel and the organic layer was extracted with deionized water (10 mL) and diethyl ether (15 mL). The organic layer was placed into an Erlenmeyer flask and the aqueous layer was placed into a beaker, which was extracted with
The reaction performed in this experiment was bromination of an alkene, using trans-Cinnamic acid, Pyridinium Tribromide, and Glacial Acetic Acid.
The actual melting point of benzoic acid is known to be 122.4°C. Also, looking at Table1, the percent yield is shown to be 44.9%. The percent yield is how much product was recovered after the reaction was carried out. The percent yield can be used to explain why the melting point observed in the experiment didn’t match the known melting point. Obtained melting points are generally lower than the literature value melting points of a substance due to the number of impurities present in the obtained product. The percent yield of 44.9%, validates that the product could have had some impurities present, and thus the lower melting
When making an organic compound, it is important to separate the compound from other compounds to make it as pure as possible, this is called crystallization.
This occurs when special carrier proteins carry solutes dissolved in the water across the membrane by using active transport. When the concentration gradient can not allow travel from one side of the membrane to the other fast enough for the cell’s nutritional needs, then facilitated diffusion is used. The transport protein is specialized for the solute it is carrying, just as enzymes are specialized for their substrate. The transport protein can be
Prediction: Draw a sketch to show the shape of the curve you expect for the solubility of a typical solid dissolving in water at different temperatures. Plot solubility on the y-axis and temperature on the x-axis.
Ensure gloves are worn at all times when handling strong acids and bases within the experiment of the preparation of benzocaine. 4-aminobenzoic acid (3.0g, 0.022 moles) was suspended into a dry round-bottomed flask (100cm3) followed by methylated sprits (20 cm3). Taking extra care the concentrated sulphuric acid of (3.0 cm3, 0.031 moles) was added. Immediately after the condenser was fitted on, and the components in the flask were swirled gently to mix components. It should be ensured that the reactants of the concentrated sulphuric acid and the 4-aminobenzoic acid were not clustered in the ground glass joint between the condenser itself and the flask. In order to heat the mixture to a boiling point, a heating mantle was used and then further left for gently refluxing for a constituent time of forty minutes. After the duration of the consistent forty minutes the rou...
The same procedure was done using 10ml of CV and 20ml of sodium hydroxide, both separately diluted to 50ml and added in a large beaker. The absorbance was recorded. In the last trial, 10ml of CV, 10ml of NaOH were diluted to 50ml. Before adding the two mixtures, 1ml of soap was added to the NaOH solution and then poured into a large beaker, along with the CV. Absorbance was recorded and the materials
In order to separate the mixture of fluorene, o-toluic acid, and 1, 4-dibromobenzene, the previously learned techniques of extraction and crystallization are needed to perform the experiment. First, 10.0 mL of diethyl ether would be added to the mixture in a centrifuge tube (1) and shaken until the mixture completely dissolved (2). Diethyl ether is the best solvent for dissolving the mixture, because though it is a polar molecule, its ethyl groups make it a nonpolar solvent. The compounds, fluorene and 1, 4-dibromobenzene, are also nonpolar; therefore, it would be easier for it to be dissolved in this organic solvent.
The solvent should be easily removed from the purified product, not react with the target substances, and should only dissolve the target substance near it’s boiling point, but none at freezing. A successful recrystallization uses minimum amount of solvent, and cools the solution slowly, if done to fast, many impurities will be left in the crystals. Using the correct solvent, in this case ice water and ethyl acetate, the impurities in the compound can be dissolved to obtain just the pure compound. A mixed solvent was used to control the solubility of the product. The product is soluble in ethanol an insoluble in water. Adding water reduced solubility and saturates the solution and then the crystals
When a miscible salt is completely dissolved in liquid solvent to dissociate positive and negative charged ions, then this mixture is called liquid electrolyte.
Benzoic acid does not dissolved in water unless the water is hot because the non polar hydrocarbon part outweighs the effect of polar –COOH part as non polar part was hydrophobic. So there was no hydrogen bonding took place and it was insoluble as the final result. Meanwhile, for ethyl 4-aminobenzoate not mixing with water due to greater chain of carbons in amino group makes it less polar than benzoic acid.
Titration is a technological process in which a solution, known as a titrant, is slowly and carefully added from a burrette into a fixed volume of another solution (known as the sample). In an acid-base titration an acid neutralizes a base or vice versa. This process is maintained untill the reaction between the titrant and the sample (acid and the base) is judged to be complete. The reaction is judged to be complete when the endpoint is reached. An endpoint in a titration analysis is referred to as the point at which no more titrant is added due to an observable colour change of an indicator. Indicators can be used to find an endpoint because they change colour when the pH of a solution changes and an endpoint in a titration is an empirical approximation of the equivalence point, which is the point of major pH change in the titration sample due to the fact that equal chemical amounts of reactants have been combined at that point. All indicators have a pH range, which is the range of pH values at which the colour of the indicator changes. Thus
The first step is choosing a suitable recrystallization solvent. This step is crucial when it comes to executing a successful recrystallization experiment. Solubility comes into play when choosing a proper solvent. When choosing a solvent, its polarity must be similar to the compound that will be purified, in this case, the compound acetanilide. The principle of “like dissolves like” can be used to understand this simple concept.
Water hardness is the amount of calcium and magnesium dissolved in water. When water passes through ground or rocks for example limestone the calcium and magnesium is dissolved into the water thus producing hard water. Water hardness does not easily give good lather with soap. There are two types of hardness, temporary and permanent. Temporary hardness is caused by dissolved calcium and magnesium bicarbonates. Boiling the water can soften temporary hardness, by boiling, it converts the bicarbonates into insoluble carbonates. Magnesium sulphates that are very soluble and calcium sulphates that are slightly soluble cause permanent hardness. Permanent hardness cannot be precipitated.