# How many moles of salicyclic acid did the company just buy

I need help answering these questions 2. Adapted from Exercise 102 in Ch. 7 of Introductory Chemistry: As an environmental scientist, you may be asked to help revive lakes that have been acidified by acid rain. Calcium carbonate (limestone) is commonly used for this application. It can neutralize the acids (HNO3 and H2SO4) in acidic lakes by a process called liming. You are asked by local community leaders to explain how this will work. To do so, you must provide the ionic and net ionic equations for the reactions between calcium carbonate and HNO3 and between calcium carbonate and H2SO4 in your report. • Write down the ionic and net ionic equations for the two reactions. • If the lake contains 1500 kg of HNO3 and 2000 kg of H2SO4, how much calcium carbonate must be added to neutralize the lake? 3. Imagine that you work for a pharmaceutical company that makes aspirin (acetylsalicylic acid). Aspirin is prepared by heating salicylic acid, C7H6O3, with acetic anhydride, C4H6O3. The other product is acetic acid, C2H4O2. C7H6O3 + C4H6O3  C9H8O4 + C2H4O2 The company just bought 2000 kg of salicyclic acid and 4000 kg of acetic anhydride to produce aspirin. You are asked by your supervisor to provide answers to the following questions: • How many moles of salicyclic acid did the company just buy? • How many moles of acetic anhydride did the company just buy? • What is the theoretical yield (in kg) of aspirin that can be produced from the two compounds that the company just bought? • The company cannot produce the maximum theoretical yield of aspirin. What are some possible reasons for this inefficiency?