The balanced chemical equation for the reaction is
FeCl3(aq) + 3NaOH(aq) Fe(OH)3 (s) + 3NaCl
Concentration of FeCl3(aq) =0.276 mol/L
Volume of FeCl3(aq) =24mL
No. of moles of FeCl3 in 24 mL solution = [0.276 mol/1000mL] x 24 mL (1L= 1000mL)
=0.006624 moles
Concentration of NaOH(aq) =0.545 mol/L
Volume of NaOH (aq) =43.5 mL
No. of moles of NaOH in 43.5 mL solution = [0.545 mol/1000mL] x 43.5 mL (1L= 1000mL)
=0.02371 moles
From the reaction stoichiometry,
1 mole of FeCl3 requires 3 moles of NaOH
So, No. of moles of NaOH required to completely react with 0.006624 moles of FeCl3 =3 x 0.006624 moles
=0.01987 moles
Now, available moles of NaOH (0.02371 moles) is more than required moles(0.01987 moles), therefore NaOH will not get exhausted during the reaction.
The reactant to get exhausted is FeCl3, therefore FeCl3 is the limiting reagent.
1 mole of FeCl3 produces 1 mole of Fe(OH)3 ( from the balanced equation)
Therefore,0.006624 moles of FeCl3 will produce 0.006624 moles of Fe(OH)3
Molar mass of Fe(OH)3 =162.2 g/mol
Mass of 0.006624 moles of Fe(OH)3=0.006624 moles x 162.2 g/mol
= 1.074 g
Mass of Fe(OH)3 precipitated =1.074 g
The reactant in stoichiometric excess is NaOH.
No. of moles of NaOH in excess= No. of moles of NaOH present - No. of moles of NaOH consumed
=0.02371 moles-0.01987 moles
=0.00384 moles
Total volume of solution=( 24+43.5)mL =67.5 mL= 0.0675 L
Concentration of excess NaOH left in solution=( No. of moles of NaOH in excess) / (Total volume of solution in L)
=(0.00384 moles) / 0.0675 L
= 0.0569 mol/L
Concentration of excess NaOH left in solution =0.0569 M
You mix 23.0 mL of 0.225 M FeCl3 with 44.5 mL of 0.461 M NaOH. What mass of Fe(OH)3 (in grams) will precipitate from this reaction mixture? Mass = g One of the reactants (FeCl3 or NaOH) is present in a stoichiometric excess. What is the molar concentration of the excess reactant remaining in solution after Fe(OH)3 has been precipitated? Assume the volumes are additive. Concentration = M
You mix 23.0 mL of 0.225 M FeCl3 with 44.5 mL of 0.461 M NaOH. What mass of Fe(OH)3 (in grams) will precipitate from this reaction mixture? Mass = g One of the reactants (FeCl3 or NaOH) is present in a stoichiometric excess. What is the molar concentration of the excess reactant remaining in solution after Fe(OH)3 has been precipitated? Assume the volumes are additive. Concentration = M