In a titration, 35.84 mL of 0.2419 M HCl solution is required to completely neutralize 18.62 mL of Fe(OH) ₃ solution. What is the molarity of the Fe(OH) ₃ solution?
3 HCl + Fe(OH) ₃ $\rightarrow$ FeCl₃ + 3 H₂O

Question

In a titration, 35.84 mL of 0.2419 M HCl solution is required to completely neutralize 18.62 mL of Fe(OH) ₃ solution. What is the molarity of the Fe(OH) ₃ solution?
3 HCl + Fe(OH) ₃

\rightarrow

FeCl₃ + 3 H₂O

Quizplus · Accepted Answer

The balanced chemical equation is:3 HCl + Fe(OH)₃ → FeCl₃ + 3 H₂OFrom the stoichiometry of the balanced equation, we can see that 3 moles of HCl react with 1 mole of Fe(OH)₃. Therefore, the number of moles of Fe(OH)₃ in the solution is:moles of Fe(OH)₃ = (moles of HCl) / 3= (0.2419 M * 0.03584 L) / 3= 2.84 x 10^-3 molThe molarity of the Fe(OH)₃ solution is:molarity of Fe(OH)₃ = (moles of Fe(OH)₃) / (volume of Fe(OH)₃ solution)= (2.84 x 10^-3 mol) / (0.01862 L)= 0.1552 MTherefore, the correct answer is A) 0.1552 M.

In a Titration, 35 →\rightarrow→ FeCl3 + 3 H2O A) 0

In a Titration, 35 $\rightarrow$ FeCl₃ + 3 H₂O
A) 0