A bottle of aromatic ammonia spirit has been recalled from the market for containing less amount of ammonia as compared with the content declared on its label. The label claims that it contains 2% v/v of ammonia. To confirm the legitimacy of this claim, an Assay testing must be conducted to quantify the amount of ammonia present in each bottles. The assay will involve reacting whatever amount of ammonia present in 10 mL sample with 30 mL of 0.25 M sulfuric acid for this reaction to occur: 2NH3 + H2SO4 → (NH4)2SO4 1. If the label claim of 2% v/v ammonia is true, how many moles of ammonia from a 10 mL sample will be available to react with sulfuric acid? The molar weight of ammonia is 17.031 g/mol. The density of ammonia is 0.73 g/mL. 0.0086 mol B. 0.0117 mol C. 0.0161 mol D. 0.1609 mol 2. Given the calculated moles of ammonia from the previous item, how many mL of 0.25 M Sulfuric acid is expected to react with it? 17.2 mL B. 22.2 mL C. 24.4 mL D. 26.8 mL 3. Therefore, of the total 30 mL 0.25 M Sulfuric acid added, only the calculated mL from the previous item will react, and the rest will become excess. To accurately quantify how many of the sulfuric acid is actually in excess, the sample will then be reacted with 0.5 N NaOH so that whatever excess sulfuric acid will react with it in the following way: 2NaOH + H2SO4 → Na2SO4 + H2O After performing the test, you have recorded that 25 mL of 0.5 N NaOH was consumed in the reaction. Calculate how many moles of 0.5 N NaOH reacted? 0.0063 moles B. 0.0125 moles C. 0.0250 moles D. 0.0375 moles
(4-10 only) A bottle of
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