The fe2 (55.845 g/mol) content of a 2.465 g steel sample dissolved in 50.00 ml was determined by tiration with a standardized 0.140 m potassium permanganate (kmno4, 158.034 g/mol) solution. the titration required 34.59 ml to reach the end point. what is the concentration of iron in the steel sample? express your answer as grams of fe per grams of steel (g fe2 / g steel).

The concentration of ions is

Explanation:

To calculate the number of moles for given molarity, we use the equation:

Molarity of = 0.140 M

Volume of solution = 34.59 mL

Putting values in above equation, we get:

The chemical equation for the reaction of iron (II) ion with potassium permanganate follows:

By Stoichiometry of the reaction:

1 mole of permanganate ions react with 5 moles of iron (II) ions.

So, moles of permanganate ions will react with = of iron (II) ions.

To calculate the mass for given number of moles, we use the equation:

Molar mass of iron (II) ions = 55.845 g/mol

Moles of iron (II) ions = moles

Putting values in above equation, we get:

To calculate the concentration of ions in steel by mass, we use the equation:

Mass of steel = 2.465 g

Mass of ions = 1.351 g

Putting values in above equation, we get:

Hence, the concentration of ions is

the answer is d   for sure : )