Question Part I Record the mass of the sodium hydrogen carbonate produced. 11.873 g Part II 1.) pH of sodium bicarbonate solution: 8. Write the corresponding ionic equation below. What is the gas produced after adding HCl? CO2 2.) Write the equation for the heating of sodium bicarbonate below. 3.) pH of second sodium bicarbonate solution:9. Write the corresponding equation below. 4.)If 11.873g of sodium hydrogen carbonate was produced, how many grams of carbon dioxide did you convert into sodium hydrogen carbonate? Please answer questions 1-4 , use lab attached if needed. Name: Munamu K Lawrence Shawarira Experiment 7: The Synthesis of Baking Soda Lab Partner: Michael Fields Date: April 1, 2013 Results and Discussions The apparatus for the experiment was set up by placing 55.0g of limestone in an Erlenmeyer flask on the left. In the flask a thistle tube was inserted and the bottom of the tube was above the level of the rocks. 50 mL were placed in a flask in the middle and the Nalgene tube is just below the surface of the water so that the gas formed can bubble through the water before reaching the final flask. In the right flask 50 mL of saturated ammonium carbonate. 1mL of HCl is added at a time to the left flask, shaking the flask to encourage reaction. Carbon dioxide should now flow through the pipette and into the ammonium carbonate solution. The flask on the right was stirred vigorously as well to mix the solution with the gas. This was done for approximately 90 minutes. Afterward, 3.0 mL of 6M NH3 was added to the solution, the product was vacuum filtered, washed with 20 mL of 50% Ethanol and air dried. Afterward, the mass of the sodium hydrogen carbonate was determined. As a result of the procedure 10.55g of sodium hydrogen carbonate were produced. A portion of the precipitate was dissolved in 5mL of water and the solution was found to have a pH of 9, revealing the basic nature of the precipitate. In the same test tube 2 mL of 6 M HCl were added and with the aid of a flame test it was determined that the adding of the hydrochloric acid produced carbon dioxide. Another portion of the sodium bicarbonate was placed in the test tube and heated and after test tube and contents had cooled, 5 mL of water were added and the pH of the resultant solution was found to be 11. The adding of HCl produced carbon dioxide which reacted with the ammonium carbonate and in turn produced the sodium hydrogen carbonate. However, the pH of the second bicarbonate solution was more basic than that of the first because more hydroxide ions were present in the solution. Also in the second solution the pH reaction begun with carbonate reacting with water whereas in the first solution, bicarbonate is what reacted with water. It was important to bubble the carbon dioxide produced from the limestone through water before allowing it to bubble through the ammonium carbonate because gas from the first flask have pure carbon dioxide go into the reaction flask. The end of the thistle tube needed to be below the surface of the acid to prevent any carbon dioxide from escaping the flask and to ensure that all the carbon dioxide that was produced would be used for the reaction. One of the tests that can be conducted to confirm the presence of carbonate ion in the product is a precipitation test. This would be done by adding a substance that would form a precipitate with carbonate and an example would be to add a silver nitrate solution and observe the reaction. If a yellow-greyish precipitate forms that is indication that carbonate ion is present in solution. Church and Dwight produce 700,000 tons of sodium hydrogen carbonate a year. To maintain this level of production they would need 366,666,666.7 kilograms of carbon dioxide. Based on the amount of sodium hydrogen carbonate obtained in the experiment 5.53 grams of carbon dioxide were converted into sodium hydrogen carbonate.

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