I need help with this question please help, I just don't understand it
Fe3+ (aq), Ca2+ (aq) and Ba2+ are all present in the same solution. Fully describe a procedure whereby you could separate these ions from one another
Mr Pursley posted this response, but I don't understand and I have a test this week and its worth 20%. Thanks
chemistry - bobpursley, Monday, November 7, 2011 at 8:11pm
look at your solubility chart
Check your chart with this:
what happens if you make the OH ion strong? Doesnt that precipated the Ca, and Fe? filter those off, leaving the Ba ion in the solute.
Add water to the filtrate, add just a tad of sulfuric acid to dissolve one, and the other does not dissolve (check your chart).
It appears to me that the directions are clear. What do you not understand about Bob Pursley's response?
To fully describe a procedure for separating Fe3+, Ca2+, and Ba2+ ions from each other, you can follow these steps:
1. Begin by making a solution containing Fe3+, Ca2+, and Ba2+ ions. You can obtain this solution from a laboratory or use appropriate chemical reagents to create it.
2. Consult a solubility chart to determine the solubility of various hydroxide (OH-) ions. The solubility chart will show you which ions will precipitate and form solids when reacted with hydroxide ions.
3. To separate Ca2+ and Fe3+, you can add a strong base, such as sodium hydroxide (NaOH), to the solution. The OH- ions from the base will react with Ca2+ and Fe3+ ions to form insoluble precipitates. Consult the solubility chart to identify which hydroxide precipitates are insoluble.
4. Once the Ca(OH)2 and Fe(OH)3 precipitates have formed, you can filter them off from the solution using a filter paper or other appropriate filtration method. The solids caught in the filter will be the Ca2+ and Fe3+ ions, separated from the solution.
5. The remaining solution after filtration will contain the Ba2+ ions. Add water to this filtrate to dilute it.
6. Next, add a small amount of sulfuric acid (H2SO4) to the diluted filtrate. You are trying to dissolve one of the precipitates selectively. Consult the solubility chart to determine whether BaSO4 is soluble or insoluble in acidic conditions. The chart will also indicate whether Ca(OH)2 and Fe(OH)3 are soluble or insoluble in acidic solutions.
7. The addition of sulfuric acid will dissolve the BaSO4 precipitate since it is soluble in acidic conditions. However, the Ca(OH)2 and Fe(OH)3 powders will remain insoluble and unaffected by the acid.
8. At this stage, you can use another round of filtration to remove the remaining insoluble precipitates of Ca2+ and Fe3+. This will yield a filtrate that contains the Ba2+ ions, which can be used separately.
Remember to consult the solubility chart to confirm the solubility properties and decide the appropriate reactions and steps for separation. This procedure should help you separate Fe3+, Ca2+, and Ba2+ ions from each other in a solution. Good luck with your test!