solutions and Standardizing Acid and Base solutions Objectives: The objective of this experiment is: 1- To prepare two primary standard solutions‚ KHP and Na2CO3 2- To standardize a sodium hydroxide solution using the prepared primary standard KHP. 3- To standardize a hydrochloric acid solution using the prepared primary standard Na2CO3. 4- To calculate the concentration of an unknown acid or base. Introduction A primary standard is a standard that is accurate enough that it is not calibrated
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April 7th‚ 2015 Section- 109 Investigating Stoichiometry with Sodium Salts of Carbonic Acid Introduction- This experiment is intended to help find a better understanding of chemical stoichiometry through titrations of NaHCO3 and NA2CO3 with HCl. A chemical reaction is a process that involves rearrangement of the molecular or ionic structure of a substance‚ as opposed to a change in physical form in a nuclear reaction. Titration is when a measured amount of solution of unknown volume
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PREPARATION OF A STANDARD ACID SOLUTION NAME: ADDISON JOSHUA HUGHES ID: 1511907 EXPERIMENT: A.2.2.3.
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drop or two of the indicator. • Slowly add small amount of sodium carbonate until it changes color. • Measure out the initial and remaining mass of Na2CO3 of solution D. Data/Table HCI 0.5M Vol HC sol A Remaining mass of Na2CO3 HCI 0.25M Vol B Remaining Mass of Na2CO3 HCI 0.3M Vol C Remaining Mass of Na2CO3 HCI unknown Vol D Remaining Mass of Na2CO3 10 mL 0.28 g 10 mL 0.23 g 10 mL 0.21 g 25 mL 0.72g 15 mL 0.49 g 15 mL 0.42 g 15 mL 0.32 g 20 mL 0.60 g 20 mL 0.49 g 20 mL 0.46 g 30 mL 0.90 g 30
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CHM 3880 Fall 2011 Partner: Edwin Gay Abstract The PH at each point during the titration of sodium carbonate unknown sample was determined. An Unknown sample of Na2CO3 was titrated with a standard HCL solution. In addition to titration‚ the pH at each point of titration was measured using PH meter. The % of the unknown Na2CO3 was 25.83% Introduction1 The purpose of this experiment was to determine the actual pH at each point during the titration of a sodium carbonate unknown with the use
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In step1‚ one set up x as a mass of NaHCO3 in the original mixture. Thus‚ equation that shows that the total mass of NaHCO3 and Na2CO3 is 2.00g. In the second step‚ by using gravimetric analysis‚ one converts x into the mass of Na2CO3 that has been produced from heated NaHCO3‚ and states that the total mass of produced Na2CO3 and the Na2CO3 in the original mass is 1.605g‚ the result that the experimenter gained from the experiment. In the step4‚ one figures out the x‚ the mass of NaHCO3
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|| || Data Tables: Step 3: Show the calculation of the needed amount of Na2CO3 Convert 1.0g of CaCl2-.2H2O to moles of CaCl2-.2H2O 1.0g x 1 mole CaCl2-.2H2O 147.0 g CaCl2-.2H2O = 0.00680 moles CaCl2-.2H2O The mole ratio is 1:1 Hence if we have 0.00680 moles of CaCl2-.2H2O we will as well need 0.00680 moles of Na-2CO3 Convert moles of Na-2CO3 to grams of Na2CO3 = 0.00680 moles Na-2CO3 x 105.99g Na-2CO3 1
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conducted by dissolving three ionic compounds‚ CaCl2‚ Na2CO3‚ and NaCl‚ in distilled water to measure the enthalpy of solution.
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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 and has a high pH in concentrated solutions. It is soluble in water but its
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Ocean County College Department of Chemistry Chem 180 Lab 5: Ionic Reactions Submitted by Abstract: The purpose of this experiment is to work with aqueous solutions of ionic substances. Aqueous solutions are those solutions in which water is the solvent. When ionic substances are dissolved in water‚ the ions separate and become surrounded by water molecules. The focus of this experiment is on precipitates. The goal of this experiment is to study the nature of ionic reactions‚ write balanced
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