Question

Four Learning Points 1

HEBERT, KARINA LAI
How many grams of sodium carbonate would be required to precipitate
all of the Fe³+ ion from a 89.4 mL solution of 0.255 M iron(III) nitrate
solution?

Answer 1

To precipitate all of the Fe³+ ion from a solution of iron(III) nitrate, we can calculate the mass of sodium carbonate required.

Step-by-step explanation:

To calculate the mass of sodium carbonate required to precipitate all of the Fe³+ ion, we need to use the balanced chemical equation:

2Fe(NO3)3 + 3Na2CO3 → Fe2(CO3)3 + 6NaNO3

From the equation, we can see that 2 moles of Fe(NO3)3 react with 3 moles of Na2CO3 to form 1 mole of Fe2(CO3)3.

To determine the mass of sodium carbonate required, we can use the following steps:

1. Convert the volume of the iron(III) nitrate solution to moles using its molar concentration.
2. Use the mole ratio from the balanced equation to determine the moles of sodium carbonate required.
3. Convert the moles of sodium carbonate to grams using its molar mass.

Using these steps, we can calculate the mass of sodium carbonate required.

Learn more about Mass calculation