An aqueous solution contains 70.0 wt% h2so4 (sg = 1.60, = 98.08 g/mol, = 18.02 g/mol). (a) find the molar concentration, c, in mol/l. show your basis of calculation. (b) find the mole fraction of h2so4. (c) find the average molecular weight of the solution.

a. 9.68 mol/L.

b. 0.3.

c. 42.04 g/mol.

Explanation:

Hello, in the attached picture, you can check the mathematical procedure for you to substantiate the answers.

a. At first, a basis of 100 g of the solution is taken, thus the mass of sulfuric acid and water is 70 g and 30 g respectively. Then, we compute the mole and volume of sulfuric acid and water. Finally, we add the volume of water and sulfuric acid to get the volume of the solution and we develop the division to find the concentration in mol/L of sulfuric acid.

b. We previously computed the mole of sulfuric acid and now the waters mole is computed by considering its molecular mass. Finally, we develop the corresponding formula for the molar fraction.

c. Since the addition of the molar fraction in a dissolution must be equal to one (1), we solve for the molar fraction of water and develop the subsequent addition for the average molecular mass.

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the answer is barium and copper bromide