Prelab: Determination of Iron by Reaction with Permanganate Name: Class period:
ID: 568184 • Letter: P
Question
Prelab: Determination of Iron by Reaction with Permanganate Name: Class period: 1. Rewrite the balanced net ionic equation for the reaction you will do (found in the introduction). Note Date: that this is a reduction oxidation reaction in the presence of acid. (2 pt.) can be oxidized to Fe" by 1.5 x 10* moles of Mno.? 2. Using that equation, how many moles of Fe (2 pt.) 3. A sample is analyzed as outlined in this experiment. If the sample weight is 2.408 g, and it requires 25.25 mL of 0.01505M KMnO4 to get to the pale pink endpoint, Show calculations for credit. Be mindful of significant figures. How many moles of KMnO4 or Mno were required? (4 pt.) How many moles of Fe were in the sample? (4 pt.) How many grams of iron were in the sample? (4 pt.) What was the % mass of Fe in the sample? (4 pt.)Explanation / Answer
Answer 1 :
KMnO4, is a strong oxidizing agent. So, The reduction of permanganate requires strong acidic conditions.
5Fe2+ + MnO4- + 8H+ 5Fe3+ + Mn2+ + 4H2O ( only reaction is asked )
Answer 2 :
The stoichiometric coefficient of both Fe+2 and Fe+3 are same. So, 1.5*10-2/5 =0.3*10-2 moles of Fe+2 can be oxidised to Fe+3.