The fe2+(aq) solution described in part a was produced by dissolving 4.05 g of ore in acid. what was the percentage of fe by mass in this ore sample? express your answer to three significant figures and include the appropriate units. submithintsmy a

Information from part a is missing in the question which is given below.

Part a ) The titration of 25.0 mL of an iron(II) solution required 18.0 mL of a 0.225 M solution of dichromate to reach the equivalence point. What is the molarity of the iron(II) solution?

Balanced chemical equation for the reaction is

Let us use the information from part a to find grams of Fe.

Step 1 : Find moles of dichromate solution

Step 2 : Find moles of Fe(II) solution using balanced equation and mol dichromate

Step 3 : Convert moles of Fe(II) to grams of Fe

Step 4 : Find % of Fe by mass

Grams of Fe present in the ore are 1.357

Grams of ore are given as 4.05

% of Fe in the ore can be found out using following formula

% Fe by mass =

% Fe by mass = 33.5%

Percentage of Fe by mass in the ore is 33.5%

h let me think

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation: