Question

Background The common laboratory acids such as H2SO4, HCI, HNO3, and HC2H302 arrive in the teaching stockroom as very concentrated AQUEOUS solutions that we refer to as concentrated H2SO.(aq), concentrated HCl(aq), etc. You used con (concentrated) H2SO4(aq) as a catalyst in the preparation of aspirin. Calculate the molarity of con H2SO4(aq). Information on the container tells us that con H2SO4(aq) is 96.0% by mass H2SO4 and has a density of 1.84 g/mL. In carrying out the calculation, assume you are starting with 1.00 L of con H2SO4(aq). Follow the steps below to calculate the molarity of con H2SO.. SHOW YOUR WORK. a. What is the mass of 1.00 L of con H2SO4(aq)? b. How many grams of H2S04 are in this 1.00 L of solution? How many moles H2SO4 is this? C. Apply the definition of molarity to calculate the molarity of this con H solution

Answer 1

Given, volume of the concentrated H250 Sopa = 12 = 1000 mL density of the solution = 1.84 g/me a mass of 1 L of conc. Hasof (as) = 1000 ml x 1.84 g/ml = 1840 g b. Given, conc. Hq Sog (ar) solution is 96.0 % by mass H2509 Thus, 100 g of sola contain 96 g of Hasoa .. 1840 g of sole contain 96x1840 Too got H₂SO4 = 1766.4 g of H2SO4 in Grams of Hqsoq in L of this soluti- on = 1766.4 g Am

Now, molar mass of Hq soq = 98 g/mol .. No. of moles of Hq Soa - 17 66.4 g 98 g/mol 7 18.0 mol = Molarity = No. of moles volm in in Molarity = 18.0 mol 1 L - 18.0 mol/L = 18.0 M . Molarity of concentrated HQ 509 sofn = 18.0M
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