Question

please help me answer 1-3. My avergae number of mL of 0.100M NaOH required to titrate the remaining anount of HCl in my sample is 1.08mL.

CAMERY Review Layout References Mailings Wednesday, March 25, 2020 View Help ID Number Experiment 17: Analysis of an Antacid Normally in the lab we would do the titration as described. Instead I will be providing you with the results as if you had gotten them from your titration. The procedure calls for you to grind a sample of solid antacid and place an amount (please use 0.200 g as your sample size for the calculations below) in an Erlenmeyer flask along with 25 ml of 0.100 molar HCl. The mixture is then heated to remove any dissolved carbon dioxide. The HCl has reacted with the antacid (either carbonate or hydroxide) and completely overwhelmed any buffering capacity of the antacid. You will then back titrate the remaining acid with 0.100 molar sodium hydroxide. Mol HCl: 25.0 mL x 0.100 M HCI = 0.0025 mol HCI - Mol HCl remaining based on titration= x mol HCl (ml NaOH at 0.100M) =Mol HCl consumed by antacid = mol base in antacid The amount of base (in moles) originally present in the antacid is the difference between the moles of the original acid sample (25 mL of 0.100 molar HCI) and that calculated as remaining after reaction with the antacid by inference by the amount of base needed to neutralize the remaining acid. For the data please use the last 4 digits of your ID number as follows: If your ID number is 12345678, Use 5.678 (rounded to 5.68) as the average number of mL of 0.100M NaOH required to titrate the remaining amount of HCl in your sample. Then do the calculation of the antacid moles in the sample. Do the following calculations: 1. Assume the antacid in the sample is calcium carbonate. How many mg of calcium carbonate are in a 1.00 g tablet of the antacid? 2. Assume the antacid in the sample is magnesium hydroxide. How many mg of magnesium hydroxide are in a 1.00 g tablet of the antacid? 3. Assume the antacid in the sample is aluminum hydroxide. How many mg of aluminum hydroxide are in a 1.00 g tablet of the antacid? Answer the following questions: 1. Why do some antacids cause was to accumulate in the stomach? What is the gas? Write the chemical equation involved. 2. The label on liquid Gaviscon states that each tablespoon (15 ml) contains 95 mg of Al(OH)3 and 412 mg of MgCO3. How many moles of hydronium ion can be neutralized by one tablespoon of Gaviscon?

Answer 1

25 mL 0.1 (M) HU was added, ie 0.0025 molttu. x Excess Hel is consumed by 1.08 ML 01 (1) Naoh. 0 0.2_ x 1.08 mol de. 1000 = 1.08x109 mol He consumed by antusid = 0.0025-1.088109 = 2.392 x 103 mol 1. CaCO3 MW = 100 g/mol sito . 2.392х 10? mol Callz = 0.2392 g C = 239.2 mg CaCO3 2. Mg(OH)₂ = M.W = 58.3 g/rea) 2.392.103 mol Mg(OH)2 = 2.392x 10 x 58.3 * 1000 mg = 139. 4536 mg Mg(OH)2 3. Al(OH)₃ - MW- 78 g/mol. 2.392x 103 mol AllOH)3 = 186.576 mg Alloh) w