A student carried out the synthesis described in this experiment. In the first s

Question

A student carried out the synthesis described in this experiment. In the first step of the synthesis the student combined 4.918 g of Fe(NH4Mso,)2·6H20 with 25.0 mL of 1.0 M H,C204. Inthe second step of the synthesis the student added 20.0 mL of saturated K,C204, 20.0 mL of390 H,02, and 8.0 mL of 1.0 M H,C,O, to the solid FeC,O 2H,O produced in the first step. I. (a) Calculate the number of moles of Fe(NH4)2(SO4)2·6H20 in 491 8 g of Fe(NH4MSOJ 6H2O (b) Calculate the number of moles H C,04 in 25.0 mL of 1.0 M H,C,04 (c) Calculate the number of moles of K C,04 in 20.0 mL of a saturated K,C,04 (300 g K C,0, H2O per liter) solution. (d) Calculate the number of moles of H202 in 20.0 mL of a solution that is 3% H2O2 by weigh Assume that the density of the solution is 1.01 g/mL (e) Calculate the number of moles H2C20, in 8.0 mL of 1.0 M H2C204

Explanation / Answer

a)

MW of Fe(NH4)2(SO4)26H2O= 392.1388 g/mol

mol = mass/MW = 4.918/ 392.1388

mol of Fe(NH4)2(SO4)26H2O = 0.012541

b}9

mol of acid = MV = 1*(25*10^-3) = 25*10^-3 = 0.025 mol

c)

in 1000 mL = 300 g

in 20 mL --> 20/1000*300 = 20/1000*300 6 g of K2C2O4 wil be present

d)

mol of H2O2 in 20 mL of a 3% solution

20 mL = 20*1.01 = 20.2 g of H2O2

3/100*20.2 =0.606 g of H2O2

mol = mass/MW = 0.606/34

mol of H2O2 = 0.0178

e)

mol = MV = (1)(8*10^-3) = 8*10^-3 mol of H2C2O4

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