Question

uy.cun/myct/itemViewrassignmer < Chapter 13 Exercise 13.115 Constants I Periodic Table Pa A solution of 49.4% H2SO4 by mass has a density of 1.39 g/cm' at 293 K A 24.4 cm3 sample of this solution is mixed with enough water to increase the volume of the solution to 99.5 cm3 Finc

Answer 1

we know that

mass = volume x density

so

mass of H2SO4 solution taken = 24.4 cm3 x 1.39 g/cm3

mass of H2SO4 solution taken = 33.916 g

now

mass of H2SO4 = 33.916 g x 49.4 / 100

mass of H2SO4 = 16.7545 g

now

moles = mass / molar mass

so

moles of H2SO4 = 16.7545 g / 98 (g/mol)

moles of H2SO4 = 0.17096 mol

now

final volume = 99.5 cm3 x 1 L / 1000 cm3

final volume = 0.0995 L

now

molarity = moles of H2SO4 / volume of solution (L)

molarity = 0.17096 mol / 0.0995 L

molarity = 1.718 mol/L

so

the molarity of H2SO4 is 1.718 M