Melting point Essays

Introduction: The melting point of a pure substance is a characteristic that is physically consistent with each specific substance. When a substance is impure, it causes the melting point to decrease and the range of the melting point to increase. In order to identify a pure substance, it must be purified in order to get an accurate melting point estimation. Purification can be done through crystallization. Crystallization is one of the simplest and most effecting ways to purify a solid. The procedure

Thus, the hypothesis that when salt is sprinkled on ice, a brine is made with the surface of the water, which lowers the freezing temperature of water and starts melting the ice that the brine is in contact with. Compare results with info found in research. Site sources. Consider sources of uncertainty in your measurements. This is an important result as it shows that table salt helps ice cubes melt faster, which

The Identity of the unknown, in this case unknown A, was determined to be acetyl salicylic acid. This was determined by comparing the melting points of the purified unknown crystals to the crude unknown. The known melting point range for acetyl salicylic acid is 135°C -136°C. The Unknown’s melting point was slightly off at 128.6°C - 132°C. This can be due to impurities of the crystals during the purification process. There were a few steps in the experiment that may have contributed to impurities

The phenomenon of freezing point depression has many practical uses. The radiator fluid in an automobile is a mixture of water and ethylene glycol (antifreeze). As a result of freezing point depression, radiators do not freeze in winter (unless it is extremely cold, e.g. −30 to −40 °C (−22 to −40 °F)). Road salting takes advantage of this effect to lower the freezing point of the ice it is placed on. Lowering the freezing point allows the street ice to melt at lower temperatures, preventing the accumulation

mixture was separated into its pure benzocaine and benzoic acid portions. This could be proven by matching the melting points of the substituents obtained at the end of the lab to the average melting points found in several chemistry databases. In other words, the melting points of the purified benzocaine and benzoic acid compounds (93.2˚C and 131˚C, respectively) reflect a similar melting points to the documented 89˚C and 122.41˚C of the pure compounds found in nature. Although, the results was collected

are extremely important in this operation. Water’s freezing point is 32 degrees Fahrenheit or 0 degrees Celsius.  As some may not be aware of, this temperature is only accurate with pure water. If other particles and substances were added to the water, the freezing point would no longer be the same. So, how does salt alter a solution when it is dissolved into water?        When dealing with homemade ice cream “change phase”, “freezing point-depression”, and “temperature” are extremely important words

Sophia Vines Honors Chemistry Period 3 Group 1 September 30, 2016 Topic: Ice Melting Alternatives Background Research Since salt is an effective way to melt ice that is harmful to the environment, the objective of this experiment is to find a more eco-friendly alternative. For this experiment, the scientist will find out how effective sugar and fertilizer are at melting ice compared to table salt. The independent variable is the different de-icing agent (salt, sugar and fertilizer.) The dependent

parts of alum through a series of tests. We also were able to conclude whether or not the substance was alum after all. The testing of the alum, AlK(SO4)2, was able to conclude the melting point of alum, to determine whether sulfate was present in alum, and the water of hydration in the alum crystals. The melting point of alum was measured to be 92.5℃. This was tested by taking the alum and crushing it into a powder which was put into a capillary tube. The capillary tube was conjoined with a thermometer

charge) is attracted to the oxygen part of the water molecule and the chloride (which has a negative charge) is attracted to the hydrogen part of the water molecule. This prevents hydrogen bonding so it prevents re-freezing. Since more water is melting and less is re-freezing, more heat is being absorbed from the surroundings and less is being released into the surroundings. Therefore, the surroundings get colder. Experiments have shown that adding salt to ice water can make

determine this, one must compare a multitude of factors. In this lab, the freezing point depression of water, enthalpy of dissolution, cost, and environmental impact will be discussed. A large factor in how effective a substance is as a deicer is it’s ability to decrease the freezing point of water. If the freezing point of water can be lowered, the outside temperature must be much colder to reach this new freezing point, resulting in less ice on the roads. These results a somewhat inaccurate due to

The freezing point for tert-butanol in literature is 78 F, or approximately 25 C, which is quite close to what was observed, as stated in the Freezing Points Table. (NOAA, 2016). The molarity of the additive substance could be calculated by taking the moles used and diving by the volume of the solvent. So for benzoic acid, there would be two different values. For the first, the moles could be calculated by dividing the grams used by the molar mass of benzoic acid, 122.123. (NIH, 2016). .3/122

The suspense helped drive it along. Karen Rhodes said “The suspense as gripping; Will he get the fire built in time? Will he live?” The suspense never dies down at all, it keeps building up. However, it’s not noticeable to the point of cheesy horror film. The most suspenseful it gets is when the dog refuses to get close to him and the story says “He was losing in his battle with the frost.” The sentences afterwards lose the suspense since there is nothing the man can do to survive

THE MPEMBA EFFECT Erin Splaine Deerfield School Grade 8 Abstract The reason for this experiment was to find a faster way to freeze water by simply changing the temperature. The way this was accomplished was by heating an amount of water while leaving an equivalent amount at room temperature, then freezing both amounts of water and determining which freezes first. The heated water ended up freezing completely first, even though the cooler water started to freeze first. These findings tell us that

Hill provided. We recorded our results and found that ice melt faster on block A ( Aluminium) than block B ( Plastic). We were soon put with the question, “ Why does ice melt faster on block A?”. We believe that explanation number 3 from “The Ice Melting Blocks Problem” gives an answer to the question. Our answer says, “ The ice melts faster on block A because block A is a good conductor. Although block A is colder than block B, it is still warmer than the ice. As cold moves into block A, the ice

I believe the ice melts faster on the metal block because it gives off more thermal energy than the plastic block; although the metal block is formed more kinetic energy than the plastic block, even when the metal block ‘feels colder’. Common sense dictates that the cold thing is supposed to sustain the ice block for a longer time, just like your refrigerator does. So why does the opposite happen? The temperature of the metal block is presumed to be colder than the plastic block, but in reality,

My research topic for this science fair is: Does Ice melt faster in water, coke, apple juice? I was interested in this topic because it would cool to know what drink would have the biggest effect on the ice. During research I fould out that ice melts at a temperature of 32 degrees farhenhiet. Pressure can also alter the amount of time it takes for an ice cube to melt. It would be interesting to see what type of impact that these drinks would have. During my experiment I hope to find that out

Purpose: The purpose of this experiment was to determine the molar mass of unknown #43 using the derived freezing point depression. To obtain the freezing point depression, t-butyl alcohol was placed in a cold-water bath and frozen solid for a total of two runs. Then, unknown #43 was dissolved in t-butyl alcohol and placed in a cold-water bath until frozen solid. This process was repeated for a total of three runs, with the first two runs containing half of the unknown, and the last run containing

The melting point of the experimentally synthesized Aspirin product was found to be between 126-129 ˚C. This temperature range of initial to final melting point has a small and sharp temperature range of only 3˚C, which is within the acceptable limits of the 128-137˚C1 literature value for Aspirin (Acetylsalicylic Acid/2-acetoxybenzoic acid), if located slightly toward the beginning of the literature melting temperature range. Therefore, the narrow melting point range, which falls within the standard

solid was left to dry over the weekend. The following lab period the solid was weighed (0.0483 g) and percent yield was calculated (65.5%) with the limiting reagent being tetraphenylcyclopentadienone. The melting point was determined. The first melting point was 204-204.9 °C and the second melting point was 215.6-215.9°C. Finally, an infrared spectroscopy was obtained for the

become electrically neutral. Salt causes freezing point depression when combined with ice. In order for salt to begin the melting process, it must come in contact with water. Fortunately, a thin film of water can generally be found on top of ice and snow. As the top layer of water tries to freeze the salt gets in the way. The total number of water molecules captured by the ice per second goes down, therefore the rate of freezing goes down. The melting occurs faster than the freezing because it is not