ubility * 1 To measure the molar solubility of a sparingly soluble salt in water. * 2 To prepare a calibration curve based on complex ion formation for absorbance enhancement. * 3 To calculate the solubility product constant (Ksp) of a sparingly soluble salt from its molar solubility. * 4 To confirm the common ion effect on the molar solubility of a sparingly soluble salt. Introduction In previous introductory chemistry courses‚ you learned some basic solubility rules that are
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Self Heating Food and Drink Cans Heater meals – originally developed for military use – are ready-made self-heating meal packs. They can be heated in many ways – by pressing a button on the packaging‚ unwrapping and shaking the pack‚ or pouring the contents of one bag into another and waiting for a few minutes – all of which use exothermic chemical reactions. These meals can be used to motivate students to study such reactions relatively safely and without the use of a burner. Plus there is the
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concentration of CaCO3 obtained was 1034 ppm‚ with a standard deviation of 2.4495. The results indicate that the unknown solution can be considered as hard water. Introduction The hardness of water is defined in terms of its cation content‚ which includes calcium‚ magnesium‚ iron‚ zinc‚ and other polyvalent metal ions. These metal ions interfere with the use of the water for many applications. For example‚ these ions diminish the effectiveness of soap and detergent for cleansing operations; they diminish
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antacid for hyperchlorhydria • for intestinal toxemia CALCIUM-CONTAINING ANTACIDS • dependent upon their basic properties • raise stomach pH to 7 • constipating • found in combinations with magnesium antacids 1. CALCIUM CARBONATE • precipitated chalk • fast action • found in combinations with Mg antacids • in Lozenges and Oral suspension 2. TRIBASIC CALCIUM PHOSPHATE • Precipitated Calcium Phosphate‚ Tertiary Calcium
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Indiana University. (2010). Retrieved March 8‚ 2012‚ from Indiana University: http://www.indiana.edu/~nimsmsf/P215/p215notes/LabManual/Lab12.pdf Lehninger‚ A Schonheyder‚ F.‚ & Volqvartz‚ K. (2008). On the Activation of Pancreatic Lipase by Calcium Chloride at Varying pH. Acta Physiologica Scandinavica ‚ 62-69. Tortora‚ G. J.‚ & Anagnostakos‚ N. P. (1990). Principles of Anatomy and Physiology. New York: Harper & Row‚ Publishers.
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EXPERIMENT 13： Extraction: Extraction with acid and alkali Objective 1. To recover the benzoic acid and p-dichlorobenzene from its mixture from its mixture by using acid-alkali extraction. 2. To determine the percentage recovery and melting point of the recovered benzoic acid and p-dichlorobenzene. Introduction Acid-base extraction is a process which purifying the acids and bases from mixtures based on their chemical properties. Acid-base extraction is performed to isolate the compounds and natural
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of calcium from the sarcoplasmic reticulum. Calcium is what activates the contractile mechanism‚ causing the muscle fiber to shorten (Rodriguez‚ et al. 2913). Calcium (Ca2+) channel blockers are components of several drugs such as those for high blood pressure and migraines. Therefor it is important to understand what adverse effects calcium channel blockers can have on muscle contractions because it can be dangerous if someone is operating heavy machinery while under the effects of a calcium channel
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test the gases‚ otherwise you can use the standard set up) The limestone cycle: 1. Burn the limestone chip/ limestone powder in a test tube in a Bunsen flame → calcium oxide 2. Put calcium oxide in water → calcium hydroxide solution + left over limestone 3. Filter the leftover limestone 4. Blow bubbles using a straw into the calcium hydroxide solution → limestone Flame colors: (I copied a table from the internet because it isn’t in the book‚ the ones in red I’m pretty sure you have to know‚
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objects known as “scum”. Calcium ions are typically the most common contributing factor for water hardness so this experiment uses CaCO3 (Calcium Carbonate) to analyze the hardness of an unknown sample. A scale of water hardness identifies “soft” water with a value less than 60 ppm (parts per million) and “hard” water with a value more than 200 ppm. 3 mL of ammonia/ammonium chloride buffer (pH 10) is added to the mixture prior to the titration to capture the calcium metal ions so the indicator
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Energetics Worksheet 1. Calculate a value for the Lattice Energy of Calcium Chloride from the following data. Draw energy cycles Std. Enthalpy of Formation of CaCl2 = - 795 kJ/ mol Std. enthalpy of atomisation of calcium = + 177 kJ/mol Std. enthalpy of atomisation of Chlorine = +121 kJ/mol 1st ionisation energy of calcium = +590 kJ/mol 2nd ionisation energy of calcium = +1100 kJ/mol Electron Affinity of chlorine = -364 kJ/mol 2. Draw Born-Haber cycles and calculate the L.E. of Cu2O and CuO
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