the+effect+of+temperature+on+sodium+chloride


 * __ Abstract: __**
 * THE EFFECT OF TEMPERATURE ON SODIUM CHLORIDE. Cameron Mattics, Ross Baker.** The purpose of this experiment was to help understand the effect of temperature on sodium chloride in a salt garden. Four different samples were created with the same procedure and place in four separate locations where the temperatures were all different. The oven was approximately 47 C, room temperature 22 C, refrigerator 5 C, and the freezer was -21 C. The four samples were monitored over a four day period and the procedure required and addition of 2 table spoons of sodium chloride every day for three days helping to absorb the liquid and accelerate the evaporation process. On the first and third day 2 table spoon of water and two table spoons of bluing were required. The oven sample formed crystal all over the bowl, the crystals were thin and white with a bluer appetence the close the crystals were to the sponge. The crystals that formed at room temperature had a square structure, much more apparent then the sample in the oven, the crystal never became white and flaky like the ones in the oven. Both the refrigerator and freezer sample have little to no crystal growth at all. A second room temperature sample was created to double- check the results, and sure enough the square shaped crystals formed again. Sodium chloride created large crystal when the evaporation rate is higher, like in the oven compared to the refrigerator sample. The sodium chloride can not crystallize when the water in the bowl and in the bluing freezes or is hovering around 0 C the freezing temperature of water. The results showed that the higher the temperature the more crystal growth and the lower the temperature the fewer the crystals developed. ||
 * THE EFFECT OF TEMPERATURE ON SODIUM CHLORIDE. Cameron Mattics, Ross Baker.** The purpose of this experiment was to help understand the effect of temperature on sodium chloride in a salt garden. Four different samples were created with the same procedure and place in four separate locations where the temperatures were all different. The oven was approximately 47 C, room temperature 22 C, refrigerator 5 C, and the freezer was -21 C. The four samples were monitored over a four day period and the procedure required and addition of 2 table spoons of sodium chloride every day for three days helping to absorb the liquid and accelerate the evaporation process. On the first and third day 2 table spoon of water and two table spoons of bluing were required. The oven sample formed crystal all over the bowl, the crystals were thin and white with a bluer appetence the close the crystals were to the sponge. The crystals that formed at room temperature had a square structure, much more apparent then the sample in the oven, the crystal never became white and flaky like the ones in the oven. Both the refrigerator and freezer sample have little to no crystal growth at all. A second room temperature sample was created to double- check the results, and sure enough the square shaped crystals formed again. Sodium chloride created large crystal when the evaporation rate is higher, like in the oven compared to the refrigerator sample. The sodium chloride can not crystallize when the water in the bowl and in the bluing freezes or is hovering around 0 C the freezing temperature of water. The results showed that the higher the temperature the more crystal growth and the lower the temperature the fewer the crystals developed. ||

**__ Fabrication of Large Binary Colloidal Crystals With a NaCl Structure __** This experiment investigated the crystallization of binary colloidal crystals with a NaCl structure that could be manipulated by using external forces. The external forces used were gravity, electric fields, epitaxial templates, and dielectrophoretic compression. The gravity leads to a slower crystallization process. NaCl crystals contain two different size spheres the small partials have an octahedral hole and the larger has a tetrahedral hole. The crystallization of NaCl begins growth by following the homogeneous crystallization pattern, by stacking from larger to smaller particles, from the bottom up. Next, the heterogeneous crystallization begins to stacking from the bottom up again. The homogeneous and heterogeneous crystallization creates a parallel plane throughout the crystals. This pattern of arranging the sodium and chlorine partials in an alternating pattern that creates square crystals. Although there is an order to the alignment of the partials, there also is randomness to the stacking sequence. The randomness meant that the NaCl was not a pure compound and consisted of other materials. From the experiment it was concluded that the NaCl was stable in the approximate size and ratio.

September 22, 2009. PNAS. (Fabrication of Large Binary Colloidal Crystals with a NaCl structure). __[]__ (Accessed January 8, 2010)

Light blue crystals formed in the bottom of the bowl The whitest crystals were the one that formed the farthest from the bluing. Square shaped crystals formed around the sponge and on top as well The crystals are thin and flaky toward the outer edge of the bowl The crystal are thicker closer to the sponge and the source of the sodium chloride || Similar square shaped crystals formed None of the crystals are white and flaky The crystals are very thick and are dark blue like the color of the bluing || Since there is less salt the number of crystals is significantly less but the crystals still resemble the square structure The crystals have a bluish tint to them but the are mostly white || Some of the crystals worked their way up the side of the bowl but very few crystals formed The crystals on the side of the bowl are white and don’t appear to have any blue coloring || The sodium chloride looks no different then when it was added ||
 * || Observations: ||
 * Oven: 47 C || White crystals formed on the extremities of the bowl and on the edges of the bowl
 * Room temperature # 1: 22 C || Dark blue crystal formed only on the bottom of the bowl
 * Room Temperature # 2: 22 C || Crystals had formed in the pours of the sponge and around it as well
 * Refrigerator: 5 C || The crystals was present under and around the sponge
 * Freezer: -21 C || The liquid froze in the bowl