Question

How many milliliters of a solution that is 10.48 % (w/w) HNO3 with a density of 1.1390 g/mL should be diluted to make 5.00 L of a 0.300 M HNO3 solution?

volume= ? mL

Answer 1

density of solution = 161390 g/m2 Mars of al solution = 1.1390g/mLX 1000 m 1139.09. This solution contains 10.48% (w/w) HNO3. La Mass of HNO in tl solution - 1139.09 x 10-48 D 1. = 119.37g Molar mass of HNO = 1+14+3 x16 = 63 g/mol . Moles of HNO₃ in th solution = 119.37g - 63 g/mol 1.9948 mol . We know molarity is the moles of solute per liter of solution is molarity. So Molarity of original solution - 18948 M. Now we have to make soon of 0.300 m we haw, MVMQVH solution. > 1.8948MX V, = 5.0LX0.300M - V = 0.7916 L V = 0.7916LX 1000 m2 = 791-6 mL. which is the required volume.