a sample aqueous solution of iron(iii) sulfate has a mass of 200g, a density of 1.05...

a sample aqueous solution of iron(iii) sulfate has a mass of 200g, a density of 1.05 g/cm^3 and 8.35 x10^21 atoms of sulfur. What is the molarity of the solution?

Expert Solution

Fe2(SO4)3

1mole of Fe2(SO4)3 contains 3 moles of S

6.023*10^23 molecules of Fe2(SO4)3 contains 3* 6.023*10^23 of S

3 * 6.023*10^23 molecules of S present in 6.023*10^23 molecules of Fe2(SO4)3

8.35*10^21 molecules of S present in 6.023*10^23*8.35*10^21/3*6.023*10^23 = 2.78*10^21 molecules of Fe2(So4)3

6.023*10^23 molecules of Fe2(SO4)3 = 400g

2.78*10^21 molecules of Fe2(SO4)3 = 400*2.78*10^21/6.023*10^23 = 1.85g of Fe2(SO4)3

volume of solution = mass of solution /density

= 200g/1.05g/cm^3 = 190.5cm^3

molarity = W*1000/G.M.Wt* volume of solution in ml

= 1.85*1000/400*190.5 = 0.0243M >>>>answer

queen_honey_blossom answered 8 months ago

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