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Compare The Solubility Of Two Different Solutes

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Various solids and liquids were immersed in solvents, ranging from water to TTE, in order to observe the solubility of the given solutes in each solvent. Each solute was placed in 3 different test tubes filled with water, ethanol and TTE. In part one of the lab, 2 small crystals of iodine, nonpolar solutes, were added to 5 ml of water, ethanol and TTE. Upon our observation iodine did not dissolve in all three solvents and instead produced a dark reddish-orange colour and magenta colour in ethanol and TTE respectively. The same procedure done to the 2 small iodine crystals was repeated with the 2 small ammonium chloride crystals, polar solutes. Unlike iodine, ammonium chloride dissolved in almost every solute completely. The only exception was that it did not dissolve fully in ethanol and left behind a powdery …show more content…

Our last experiment involved investigating the solubility of an unknown solid. The unknown substance did not dissolve in most of the solvents with the exception of water. The solubility of the unknown substance leads me to conclude that the substance is polar, however it is as polar as water thus indicating that it is more polar than ethanol and TTE. With our noted observations, we came to the general conclusion that the solubility of a substance is determined by how similar the polarities of the solute and the solvent it is immersed in. For instance, iodine remained in its solid form in water and dissolved slightly in TTE. This indicates that TTE has a polarity more similar to iodine than that of water hence why the iodine’s stronger pull by the molecules of TTE allowed it to dissolve slightly better. Similarly, ammonium chloride was able to dissolve easier in water than TTE. Water is a more polar substance than TTE and created a stronger attraction between the polar molecules of ammonium

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To begin, the solubility of the unknown compound in water was tested. If the compound is soluble in water, it can be inferred that it is either a polar covalent or ionic compound.

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Sodium chloride forms an ionic intermolecular force, and silicon dioxide and octane both form a London dispersion force. Each compound behaves differently in water. Sodium chloride is soluble in water, and silica and mineral oil are not. This is because of the idea that likes dissolve like. Water forms a polar intermolecular force, and when ionic molecules enter it, they dissolve because the water molecules are more attracted to the ions rather than other water molecules.

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This result indicates that for every milliliter of water, .2 grams of the compound was dissolved; the science behind the test is that water is added in increments to determine how many mililiters of polar water molecules are necessary to break apart the polar or ionic bonds in a certain amount of solute. A Litmus paper pH test of the compound dissolved in water revealed that the solution had a pH of 7. This indicated that the solution of water and dissolved compound was neutral, or neither basic nor acidic5. The result of this test is in agreement with the identified compound because there are no OH- cations or H+ anions in KCl.

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In this experiment we investigated the physical and chemical properties of cis-butenedioic (maleic acid) and trans-butenedioic (fumeric acid) isomers. We used pH paper to determine the difference in pH between the two, water to determine the solubility of each and added a magnesium strip to each in order to determine the reactivity of each isomer. The results that we determined by this experiment is that Maleic acid is more acidic, pH of 1, than Fumeric acid, pH of 2; we found that Maleic acid was more soluble than Fumeric acid considering that the Fumeric acid did not dissolve in the water at all noticeable; Maleic acid had a much high reactivity with the Magnesium strip showing a large amount of bubbling when it was added while Fumeric acid

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Abstract: The purpose of this lab was to separate hexane and toluene from a mixture by collecting fractions of both hexane and toluene through simple distillation. Because hexane and toluene have different boiling points they distill at different times and can be separated easily. We found the refractive index by putting our collected fractions in a refractometer. Once we knew the refractive index we could figure out the percentage of both hexane and toluene in the solution. The first fraction was collected from 66°C to 70°C the temperature then dropped and the rose to 98°C and the second fraction was collected from 98°C - 100°C.

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Properties of Substances Express Lab 1)The purpose of this lab was to compare the physical properties of different types of solids and how the properties of solids are determined by their intermolecular forces and their intramolecular bonds. Then we were to classify each type of solid as either ionic, metallic, non-polar molecular, polar molecular, or network. Paraffin wax classified as a non-polar molecular, Silicon dioxide was classifies as a network, Sodium chloride was classified as ionic, Sucrose was classified as polar molecular and Tin was classified as metallic. (2)The intermolecular forces that are present in Paraffin wax are dispersion forces, because it is non-polar and carries a negative charge. Followed by Sucrose that has

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Salt does dissolve in water. But, there is a maximum limit of concentration that salt can have. When the salt concentration reaches its limit, the salty water has become saturated, meaning that the salt content in the water is so concentrated, there is not enough water left to dissolve the rest of the salt. And this would be the only time salt would not dissolve in water. When salt goes into water, the water will cause the sodium and chloride atoms from the salt to pull away and make the salt crystals begin to pull apart.

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Properties of Ionic and Covalent Substances Lab Report Introduction The purpose of this lab was to determine which of the following substances: wax, sugar, and salt, are an ionic compound and which are a covalent compound. In order to accurately digest the experiments results, definitions of each relating factor were researched, leading to the following information: ionic compounds are positive and negatively charged ions that experience attraction to each other and pull together in a cluster of ionic bonds; they are the strongest compound, are separated in high temperatures, and can be separated by polar water molecules. A covalent compound is formed when two or more nonmetal atoms share valence electrons; covalent compounds are also categorized into two sections: polar covalent and nonpolar covalent. Furthermore, polar covalent compounds dissolve in water, while nonpolar covalent compounds do not.

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Using a thin-layer chromatography, or TLC, the position in which molecules stop advancing upwards could be observed. By applying the TLC method to this experiment, different traveling distances of a certain chemical, with changing salt concentrations of water, can be measured. In this investigation, however, sheets of tissue papers were dipped into salt water with different concentrations and soaked until the water traveled to the top, so the method was different from the TLC experiment. Consequently, the volume of liquid absorbed will likely not change with different salt concentrations since every time the paper will be dipped into the solution until it completely absorbed water, each time in the same manner. Moreover, the mass of solution absorbed will increase because the density of the solution increases with increasing concentration.

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This has been criticized due to the fact that not simplest solvents, however also different capacity co-formers as well as the active substance itself can be drinks at ambient temperature (e.g. valproic acid9,10). It consequently appears to be of

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Introduction Solubility is a chemical property that is measured in terms of the maximum amount of solute dissolved in a solvent at equilibrium. The resulting solution is called saturated solution. For example when a sample of sodium chloride solution in water is heated the behavior of the reaction is endothermic obstructing exothermic behavior. Another relationship that can be said about solubility is that the solubility of a solid substance increases as the temperature increases. The solubility of solutes is dependent on temperature.

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