The reaction of iron (III) metal with a solution of copper (II) sulfate releases iron ions into the solution through a single displacement reaction. 1. What mass of iron (in grams) is required to remove all the copper ions from a 150mL of 0.100 mol/L solution of copper (II) sulfate?
2. Determine the moles of iron ions produced in this reaction.
3. Name a soluble compound that could be added to precipitate all of the iron ions from the solution.
4. What mass of the soluble compound from part (c) is required to precipitate all of the iron ions you determined in part (b)? Give your final answer in grams.

Oxidation-reduction reactions (often called "redox" for short) are reactions that involve the transfer of electrons from one species to another. oxidation states, or oxidation numbers, allow chemists to keep track of these electron transfers. in general, one element will lose electrons (oxidation), with the result that it will increase in oxidation number, and another element will gain electrons (reduction), thereby decreasing in oxidation number. the species that is oxidized is called the reducing agent or reductant. the species that is reduced is called the oxidizing agent or oxidant. to sum up: oxidation = increase in oxidation state = loss of electrons = reducing agent reduction = decrease in oxidation state = gain of electrons = oxidizing agent part a which element is oxidized in this reaction? fe2o3+3co→2fe+3co2 enter the elemental symbol. view available hint(s) is oxidized part b which element is reduced in this reaction? 2hcl+2kmno4+3h2c2o4→6co2+2mno2+2kcl+4h2o enter the elemental symbol. view available hint(s) is reduced