Chemistry: The Fe 2 + ( 55.845 g/mol) content of a 2.349 g steel sample dissolved in 50.00 mL of an acidic solution was determined by tiration with a standardized 0.100 M potassium permanganate ( KMnO 4 , 158.034 g/mol) solution. The titration required 43.16 mL to reach the end point. What is the concentration of iron in the steel sample? Express your answer as grams of Fe per gram of steel. MnO − 4 + 8 H + + 5 Fe 2 + − ⇀ ↽ − Mn 2 + + 5 Fe 3 + + 4 H 2 O

Omg thank you so muchExplanation:...

The Fe 2 + ( 55.845 g/mol) content of a 2.349 g steel - id25584523495187002, njimenez1231

jharrington583

19.01.2022

0.513 iron per gram of steel is the concentration of iron in the steel sample.

Explanation:

$MnO_4^{-} +8 H^+ +5Fe^{2 +}\rightarrow Mn^}{2 +} + 5 Fe^{3 +} + 4 H_2O$

Molarity of KMnO_4 solution = 0.100 M

Volume of KMnO_4 solution = 43.16 mL = 0.04316 L( 1mL=0.001 L)

Moles of KMnO_4 = n

$Molarity=\frac{Moles}{Volume (L)}$

$n=0.100 M\times 0.04316 L=0.004316 mol$

1 mole of KMnO_4 gives 1 mole of potassium ion and manganate ions.

Moles of $MnO_4^{-}=0.004316 mol$

According to reaction, 1 mole of manganate ion reacts with 5 moles of ferrous ions.Then 0.004316 mole of manganate ion will react with L:

$\frac{5}{1}\times 0.004316mol=0.02158 mol$ of ferrous ions

Mass of 0.02158 moles of ferrous ion:

0.02158 mol × 55.845 g/mol = 1.2051 g

Mass of steel sample = 2.349 g

Concentration on iron in sample :

$\frac{1.2051 g\text{iron}}{2.349 g\text{steel}}=0.513$ iron per gram of steel

0,0(0 оценок)