alkalinity of the unknown soda ash sample was determined by titrating it with standard HCl solution. After three trials‚ the researchers obtained an average percent alkalinity of 33.20% that resulted to a percent error of 12.63%. The percentage of carbonate and bicarbonate of the same unknown soda ash sample was also determined in the experiment‚ following the same procedures and using the same titrant that is the standard HCl solution; however‚ this time‚ the researchers made use of a pH meter. Subsequently
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than if all of the Panacetin was dissolved in the dichloromethane. (b) Failing to mix the aqueous and organic layers thoroughly during the NaHCO3 extraction would lead to little to no production of aspirin precipitate. The aqueous layer contains sodium hydroxide and water‚ whereas the organic layer contains the dichloromethane‚ aspirin‚ and the unknown. If the HCl has nothing to react with in the aqueous layer following mixing (i.e.‚ sodium acetylsalicylate)‚ then little to no solid aspirin will be
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a laboratory method in which the endpoint of a reaction is determined quantitatively. In this experiment‚ the amount of soda ash present in a sample was determined and the alkalinity reported as it was titrated using HCl as the titrant. Also‚ the percentage amount of Na2CO3 and NaHCO3 present in the sample was determined at the end of the experiment. Introduction Soda Ash (Na2CO3) or sodium carbonate is commonly used as a cleaning agent and known as “washing soda”. It was found to be alkali
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yield versus the theoretical yield of NaCl when HCl is titrated into Na2CO3 and NaHCO3. When 0.15g of both NaHCO3 and Na2CO3 are titrated with HCl‚ then 0.165g of NaCl should form from the NaHCO3‚ and 0.104g of NaCl should form from the 0.15g of Na2CO3. Procedure: Weigh 2 samples of 0.15g of dried unknown each‚ and dissolve each into 50mL of distilled water. Add 0.5 to 1mL of bromocresol green indicator until the solution turns blue. Titrate the HCl until it turns green. Gently heat and boil out
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Chemistry 104: Analysis of Commercial Antacid Tablets Hydrochloric acid (HCl) is one of the substances found in gastric juices secreted by the lining of the stomach. HCl is needed by the enzyme pepsin to catalyze the digestion of proteins in the food we eat. Heartburn is a symptom that results when the stomach produces too much acid (hyperacidity). Antacids are bases used to neutralize the acid that causes heartburn. Despite the many commercial brand‚ almost all antacids act on excess stomach
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Experiment # 4: Analysis of Soda Ash Experiment # 5: Volumetric Analysis of a Carbonate – Bicarbonate Mixture Submitted by: Eugenio December 2012 Department of Chemical Engineering University of Santo Tomas España‚ Manila Abstract Soda ash is the common name for sodium carbonate (NaCO3)‚ a chemical salt derived from carbonic acid. It is frequently used in manufacturing‚ industry‚ and in domestic chores. Glass production is one of the primary industrial uses for sodium carbonate. It is also
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The procedure for this lab are as follows below: Part 1 of 2 NaHCO3 reacted with HCl: The mass of the flask was recorded. 2.0 +/- 0.2 grams of NaHCO3 was added to the flask. The mass of NaHCO3 + flask was then recorded. Before moving on to step 3‚ the mass of NaHCO3 was calculated. Then the theoretical yield of NaCl was determined. This was the hypothesis. 30 mL of hydrochloric acid should be obtained. HCl was slowly added to NaHCO3‚ drop by drop. The reactants should not splatter out of the
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observe the reaction of NaHCO3 and HCl. Students will draw the Lewis Electron Dot Diagrams of Na+ and Cl-. Students will site examples of how to identify an ionic compound. Materials: Materials include 6M of HCl and NaHCO3 ‚ a 100 milliliter (mL) beaker‚ a 10 mL graduated cylinder‚ a dropper‚ phenol red indicator‚ distilled water‚ a hot plate‚ a balance‚ a magnifying glass‚ and beaker tongs. Procedure: First‚ measure the mass of a 100 mL beaker. Then‚ add 0.5 grams of NaHCO3 and 15 mL of distilled
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and is isolated: CO2(g) + NH3(g) + H2O(l) + Na+ (aq) + Cl! (aq) ==> NaHCO3(s) + NH4+ (aq) Cl! (aq) (1) When heated to 300 °C‚ the sodium hydrogen carbonate decomposes to form sodium carbonate‚ carbon dioxide‚ and water. 2 NaHCO3(s) ==> Na2 CO3(s) + CO2(g) + H2 O(g) (2) The crude product obtained from this thermal decomposition is called soda ash‚ which is primarily Na2 CO3 ‚ although it also contains unreacted NaHCO3 and other impurities. The total acid neutralizing capacity of a soda
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measure the mass of the solid reactant NaHCO3 and that of the solid products‚ NaCl. The experimental determination of these relative masses will enable you to determine their relative number of moles. As a result of your observations and calculations‚ you will determine the mass and mole relationships-the reacting ratios-of the solid reactants and products. The ratios of mass and moles are important in kitchen chemistry also. In some recipes‚ baking soda‚ NaHCO3‚ is used to cause a cake to “rise”
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