A solid sample of Fe1OH23 is added to 0.500 L of 0.250 M
aqueous ...

Question

A solid sample of Fe1OH23 is added to 0.500 L of 0.250 M
aqueous H2SO4. The solution that remains is still acidic. It
is then titrated with 0.500 M NaOH solution, and it takes
12.5 mL of the NaOH solution to reach the equivalence
point. What mass of Fe1OH23 was added to the H2SO4
solution?

Accepted Answer

Step 1: Identify the balanced chemical equations for the reactions. The Fe(OH)2 reacts with H2SO4 to form FeSO4 and water. The remaining H2SO4 is then neutralized by NaOH to form Na2SO4 and water.. Step 2: Calculate the moles of NaOH used in the titration. This can be done by multiplying the volume (in liters) by the molarity of the NaOH solution.. Step 3: Use stoichiometry to determine the moles of H2SO4 that were neutralized by the NaOH. Since the reaction between H2SO4 and NaOH is a 1:2 ratio, the moles of H2SO4 will be half the moles of NaOH.. Step 4: Subtract the moles of H2SO4 that reacted with NaOH from the initial moles of H2SO4 (which can be calculated from the initial volume and molarity) to find the moles of H2SO4 that reacted with Fe(OH)2.. Step 5: Use stoichiometry to calculate the moles of Fe(OH)2 that reacted with H2SO4. Since the reaction between Fe(OH)2 and H2SO4 is a 1:1 ratio, the moles of Fe(OH)2 will be the same as the moles of H2SO4 that reacted with it. Then, convert the moles of Fe(OH)2 to grams using its molar mass to find the mass of Fe(OH)2 that was added to the H2SO4 solution.

A solid sample of Fe1OH23 is added to 0.500 L of 0.250 M aqueous H2SO4. The solution that remains is still acidic. It is then titrated with 0.500 M NaOH solution, and it takes 12.5 mL of the NaOH solution to reach the equivalence point. What mass of Fe1OH23 was added to the H2SO4 solution?

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Concetti chiave

Stoichiometry

Titration

Molar Mass