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Benzoic Acid And O-Toluic Acid Lab Report

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The specific purpose of this experiment is to determine the composition of vapor and liquid phases for different mixtures of a pair of volatile liquids using refractive values and distillation techniques involving the construction of two different types of phase diagrams. Moreover, these different phase diagram might be analyzed and compared individually in order to have a better understanding about the multiple types of phase equilibrium and phase change that occurs. For the procedure, the two components are benzoic acid and o-toluic acid. The first step of this experiment is to accomplish the part A: run samples A1 to A5 and B1 to B5. For this step, place a beaker of silicon oil on top of a hot plate until the temperature reaches 135 +/- …show more content…

Firstly, measure the refractive index of water five times and then measure for each of the pure liquids (toluene and cyclohexane). After that prepare 9 mixtures of toluene and cyclohexane carrying their volume fractions from 10 to 90 percent in increments of 10 percent using 10.0 mL volumetric flasks. The last step is to read the temperature in the thermometer. Then, determine the the boiling point for toluene and for cyclohexane. Finally, complete the part C: for this part, the composition of vapor and liquid phases of toluene-cyclohexane mixtures. From the done experiment result were successfully obtained regardless some errors. The resulting liquid-vapor phase diagram for toluene and cyclohexane vs. temperature demonstrates that as the temperature increases, the components leave the liquid phase reaching the vapor phase. For this plot, the equilibrium region is the the region enclosed by the two curves (liquid and vapor). The 40% o-toluic acid phase diagram has an equation with negative slope indicating that all the components are in solid phase: y = -0.1236x + …show more content…

To take the refractive index, ten different mixtures were prepared in which each of them contains different cyclohexane and toluene concentration in increments (total volume of mixture 10 mL). After that, the corrected refractive index in found in order to plot the refractive index vs. mole fraction of toluene; the equation from this plot will allow the calculation of toluene’s molar fraction in the distilled mixture. After this calculation, the remaining molar fraction of toluene (gas phase) is used to plot Liquid - vapor phase diagram for toluene and cyclohexane vs. temperature (fig.1). This plot contains two curves representing two phases – vapor and liquid; the region between liquid and vapor curve is the equilibrium region (liquid and vapor). From the vapor phase diagram for toluene and cyclohexane vs. temperature, it might be concluded that as the temperature increases, the components change their phase from liquid to vapor phase (Fig. 1). The refractive indices values obtained for toluene and for cyclohexane are accurate since their values is closed to the known value and the percent of error is very small. The values for the temperature boiling point are precise. Factor such as the not correct reading of the temperature might be one of the reason for the fond error. In this case, the lever

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Next, about 10 mL of both solutions, Red 40 and Blue 1, were added to a small beaker. The concentration of the stock solution were recorded, 52.1 ppm for Red 40 and 16.6 ppm for Blue 1. Then, using the volumetric pipette, 5 mL of each solution was transferred into a 10 mL volumetric flask, labelled either R1 or B1. Deionized water was added into the flask using a pipette until the solution level reached a line which indicated 10 mL. A cap for the flask was inserted and the flask was invented a few times to completely mix the solution. Then, the volumetric pipette was rinsed with fresh deionized water and

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Using the data from the first two columns, an x-y scatterplot graph was created. Analyzing the graph, a set of points that formed a linear curve were identified, and the plot of the graph was reduced to these points. This is the initial cooling curve. A second series was then added to the graph, with points that correspond to the interval when t-butyl alcohol was freezing. A trendline was then created for each of the series to obtain the equation of the line and r values.

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Introduction: In this assignment, I will be doing two experimentations on examining the impact of temperature on the Alka-Seltzer’s response time. The first experimentation that I will be doing involves some water that is room temperature. The second experimentation that I will be doing involves some water that is very hot. If I want to be able to figure out the impact of the temperature on water, I will have to document the time it will take for the Alka-Seltzer to go into solution.

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After performing the investigation, it was concluded that each of the seven liquids will have different evaporation rates based upon strength and type of their intermolecular force. This is supported by (Figure 1.), in which Distilled Water contained the slowest rate of evaporation at 0.00686 degrees Celsius per second, therefore having the strongest intermolecular force because of its hydrogen bond. Pentane had the fastest rate of evaporation, as shown in (Figure 1.), at 0.349 degrees Celsius per second because it consisted of the weakest intermolecular force, a london dispersion bond. This evidence was not only supported through the experiment in which my group performed, but it was also supported by claims made by other groups who performed the same experiment. Overall, the molecular shape and the intermolecular bond type affects the rate of evaporation in liquids, causing each liquid to evaporate at its own specific

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(2005) states that all molecules have different boiling points, this is due to the intermolecular forces between the atoms. Therefore, the more intense the intermolecular force is the higher the boiling point, and the lower intensity, the lower the boiling point. This paper aims to discusses the order of the boiling points of 3-methyl-1-butanol and 3-methylbutanal, 1-Hexanol and 1-Pentanol, examining the differences between them. (De Marco et al. 2014). Results Table 1.

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Introduction Distillation is a specific technique of separating mixtures based on differences in propensity to vaporize of components in a boiling liquid mixture (Palleros, 2000). Distillation is a physical separation process, which does not involve chemical reaction and used for purification of liquids which do not undergo decomposition at their boiling point. There are several types of distillation including simple distillation, fractional distillation, vacuum distillation and steam distillation (ibid.). The type of used distillation depends on the nature of the liquid and the nature of impurities present in it. During this practical two types of distillation were performed: simple and fractional distillation.

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