determine the correct amount of sodium hydroxide needed to react with 1.0g iron (III) chloride.

To determine the correct amount of sodium hydroxide (NaOH) needed to react with 1.0g of iron (III) chloride (FeCl3), we need to use stoichiometry, which relates the moles of one substance to another in a chemical reaction.

1. Start by writing the balanced chemical equation for the reaction between sodium hydroxide and iron (III) chloride:
FeCl3 + 3NaOH → Fe(OH)3 + 3NaCl

2. Calculate the molar mass of FeCl3 and NaOH:
- Molar mass of FeCl3: 55.85 g/mol (Fe) + 3 * 35.45 g/mol (Cl) = 162.2 g/mol
- Molar mass of NaOH: 22.99 g/mol (Na) + 16.00 g/mol (O) + 1.01 g/mol (H) = 39.99 g/mol

3. Convert the mass of iron (III) chloride to moles:
Moles of FeCl3 = Mass of FeCl3 / Molar mass of FeCl3
= 1.0 g / 162.2 g/mol

4. Use the stoichiometry of the balanced equation to relate the moles of FeCl3 to the moles of NaOH:
Moles of NaOH = Moles of FeCl3 * (3 moles NaOH / 1 mole FeCl3)

5. Calculate the mass of NaOH using the moles of NaOH and its molar mass:
Mass of NaOH = Moles of NaOH * Molar mass of NaOH

By following these steps, you can determine the correct amount of sodium hydroxide needed to react with 1.0g of iron (III) chloride.