ffect of temperature on solubility
Introduction
The solubility of a substance is defined as its ability to dissolve. There are some factors that alter solubility, such as pressure and the type of solvent, but will temperature affect the solubility of a substance? The investigation problem is to identify whether or not the temperature of a substance affects its ability to dissolve in another substance. Understanding solubility and the processes that undergo is very important, this is due to the important role that it plays in our daily life as well as in the human body. When it comes to oral ingestion, especially in drug delivery, it is profitable since it permits to deliver the medicine throughout the system in order to gain positive and desired responses. Meanwhile it is seen in the human body, it is also manifested while doing household cleaning and in automoviles. That’s why it is essential to recognize and know what is solubility in order to be able to control, manipulate, and enhance it as well as get informed of how life works by depending on water and chemical reactions.
Theoretical Framework
According to Rogers (2000), the solubility of a substance is a property that states the amount that will dissolve in a certain amount of solvent. In other words, solubility refers to a substance’s ability to dissolve. When the substance is dissolving, we refer to the solvent as the substance in which the solute is being dissolved, and to the solute, which is the substance that is being dissolved. Solubility may depend and change according to its temperature, most of the times solubility of liquids and solids tends to increase as the temperature increases. Oppositely to that, as temperature increases, the solubility of the gases dec...
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Paragraph 2: It is believed that as the temperature of the water increases the time it will take for the tablet to dissolve will decrease. This is believed since the temperature there will be more energy allowing the particles to get together and form a reaction allowing the ta...
The temperature probe was placed into the test tube and recorded the temperature of the freezing solution using Logger Pro software. The test tube was held against the inner glass of the ice bath beaker so the test tube was visible to see when the solution froze over. Once the freezing point was measured, the temperature stopped being monitored and the data was recorded. The steps mentioned above for finding the freezing point, also known as ΔTf, was replicated for the 0.0, 0.4, and 0.6 concentrations. To find the freezing point depression, the equation ΔTf = imKf was used. The molality (m) of each solution was then calculated dividing moles of solute by kilograms of solvent, and the Kf value for magnesium chloride is known to be -1.86. Since magnesium chloride breaks down into three ions in deionized water, it was concluded that the Van’t Hoff factor couldn’t exceed three. For better accuracy, the experiment explained above for finding the freezing point depression and Van’t Hoff factor was re-conducted exactly the same to determine more accurate results. Again, the molality of each solution was calculated, and a graph expressing the change in freezing temperature verses molality
In this lab, lab 4.3 Comparing the Concentrations of Saturated Solutions, we set out to find and compare the solubilities of two solids in water. In addition, we tested if solubility is a characteristic property of a solid in a given liquid. This lab allowed us to test and use a reliable way to measure the solubility of a solid. This lab can be replicated for any solid with the same procedure, thus it gives us a method to calculate solubility. The two solids we tested in this experiment were NaCl (Sodium Chloride) and NaNO3 (Sodium Nitrate).
We started by testing the time it takes for sugar cubes to dissolve in boiling water. We boiled the water to 100℃ and then dropped four sugar cubes in, each cube took exactly 1:03 to dissolve. After testing the boiling water we switched the beakers, which we kept the same size and filled it with room temperature water. We made the room temperature 22℃ and then dropped four new sugar cubes in, this time it took the cubes precisely 4:52 to dissolve, so lastly we tested cold water temperature. Again switching
Performing this experiment, we used the technique called Acid-Base extraction to isolate Eugenol, which is one of the main ingredients of clove oil. Acid-Base extraction is the most efficient method for isolating organic component; it is efficient because it purifies the acid and base mixture based on their chemical identities. We have seen throughout this experiment that acid and base play an important role, when it comes to solubility in water. Our basic knowledge of acid and base is acid is a proton donor and base is a proton acceptor. This ideology helps us to understand why organic compounds are not soluble in water. When compounds tend to be insoluble, we have to use acid and base reaction, to change its solubility. The changes that occurred
Hypothesis: The Alka Seltzer will dissolve fastest in hot water and slowest in cold water.
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.
soluble. In other words, any way ap person gets it in his or her body, it will
Methanol, acetone, dichloromethane, toluene, and hexanes were tested for their miscibility with water. Methanol and acetone were found to be miscible with water, and dichloromethane, toluene, and hexanes were immiscible. Two layers—one organic and one aqueous—were observed each time an immiscible solvent was combined with water. Dichloromethane was observed as the bottom layer, and toluene and hexanes were observed as the top layers when added to test tubes of water. In Table 1 below, density, boiling point, and miscibility with water are shown for the organic solvents used in this experiment.1
Size and stability: Liquid formulation can be bulky, difficult to transport and store.1 During storage under the stated conditions, it’s necessary that oral solutions are not subject to precipitation, fast sedimentation, caking or formation of lump.2 They have poor stability compare to solid dosage form formulation due to hydrolysis.1 Therefore, it’s important to optimize the active ingredient stability in liquid formulation including those prepared from powder or granules.2
Craig, D. Q. (2002). Pharmaceutical Applications of Micro-Thermal Analysis. Journal of Pharmaceutical Science, 91(5), 1201-1213.
The heat of solution is the enthalpy change associated with the process of a solute dissolving in a solvent. With an ionic compound dissolving in water, the overall energy change is the result of two processes (the energy required to to break the ionic bonds between the ions in the lattice structure, and the energy released when the free ions form dipole attractive forces with the water molecules). Heats of solution are generally measured in an insulated container, called a calorimeter. The process of the dissolving solute either adds or subtracts heat from the solution. The amount of enthalpy change can be determined by using the equation, q=m•C•∆T, with the specific heat of the solution generally being the same as that of water, 4.18 J/g•C°.
Electrical conductivity refers to a substances ability to carry moving electrons (conduct electricity). In order to do so, there must be a supply of delocalised electrons. While in a solid state, ionic substances can not conduct electricity as there are no delocalised electrons or free/mobile ions to act as charge carriers. In an aqueous ionic solution, the H2O molecules break apart the crystal lattice structure of the ionic substance into individual ions, surrounding each ion in a jacket of hydration. Below is the equation that describes the dissociation of NaCl when in H2O solvent.
1-Butanol with intermediate polarity was soluble in both highly polar water and non polar hexane as 1-butanol can be either polar or non polar compound. 1-Butanol was polar based on the general rule of thumb stated that each polar group will allow up to 4 carbons to be soluble in water. Also, 1-butanol can be non polar due to their carbon chains, which are attracted to the non polarity of the hexane.
Water is the most important substance in our evolution and our daily lives. Without water,