How to Create 1% Iron Solution - Step by Step Guide

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Discussion Overview

The discussion revolves around the preparation of a 1% iron solution, specifically focusing on the dissolution of iron III chloride in water. Participants are exploring the calculations needed to verify the concentration of iron in the solution, addressing both theoretical and practical aspects of the preparation process.

Discussion Character

  • Homework-related
  • Mathematical reasoning
  • Technical explanation

Main Points Raised

  • One participant questions the calculation of the iron percentage in the solution, noting difficulty in verifying the value.
  • Another participant clarifies that the 1% refers to the iron III chloride (FeCl3) concentration rather than elemental iron (Fe).
  • A participant provides a link to a protocol for preparing the solution and requests assistance with the calculations involved.
  • There is a suggestion to determine the form of iron being reported (Fe, Fe2O3, or FeCl3) and to adjust calculations accordingly.
  • One participant estimates that to prepare a 1% w/w FeCl3 solution, approximately 1.68 g of FeCl3.6H2O should be dissolved in water.
  • Another participant emphasizes the importance of calculating the mass of FeCl3 in the given amount of FeCl3.6H2O and suggests starting with molar mass calculations.
  • A later reply mentions the possibility of labeling the solution as 0.10 M instead of 1%, indicating a potential misunderstanding in the task requirements.

Areas of Agreement / Disagreement

Participants express varying interpretations of the task, with some focusing on the percentage of iron in the solution while others clarify the concentration of iron III chloride. No consensus is reached on the correct approach to the calculations or the labeling of the solution.

Contextual Notes

Participants highlight the need for clarity on the form of iron being measured and the importance of precise measurements in the calculations. There are unresolved aspects regarding the definitions and assumptions related to the solution's concentration.

lesieux
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1% iron solution??

Homework Statement



Dissolve 1.70g of iron III chloride in 99 ml of distilled water. Mix well and label 1% iron.

Homework Equations



I've tried to check the value of the iron percentage but I don't succeed.


The Attempt at a Solution



First I've tried to find out the number of mole of FeCl3,6H2O (M=270g.mol-1) in 1.70 g and found the mass of iron 0.352 g then divide this mass by the total mass (1,7+99), but it doesn't work. Could anyone help me? Thanks in advance.
 
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This will be 1% in FeCl3, not Fe.

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You are going to determine iron in what form? You are going to report iron as Fe or Fe2O3 or FeCl3? I've got a feeling that you won't be reporting iron as FeCl3. Find out the form you need and ratio the molecular wt to that of FeCl3.

I'm guessing that it will be something like 1.7.
 


chemisttree said:
I'm guessing that it will be something like 1.7.

That could be accidental, but to prepare 1% w/w FeCl3 solution you need to dissolve 1.7 g (more precisely 1.68 g) of FeCl3.6H2O in appropriate amount of water.

I wrote concentration calculator just to be able to check such things on the fly...

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I'm sorry to ask you this question.
It may be obvious but as i didn't succeed.
Would you mind showing me the calculation?
Thanks in advance.
 


Basically you have to calculate what is mass of FeCl3 in 1.7g FeCl3.6H3O. Start calculating their molar masses. 1 mole of FeCl3.6H3O contains how many moles of FeCl3?

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Assume that the FeCl3 is anhydrous.

You are asked to label it 0.10 M, not 1%, right? If that is the case, then you are on the right track. Be sure to carefully weigh the FeCl3 and label it accordingly. You might not need to measure it out to three or four decimals, but you should do so in your calculations.

Remember that moles = grams/formula wt. and that concentration (M) = moles/volume(L)
 

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