determine the molatiry of each of the ions present in the following aqueous solutions[assume 100% ionization]
2.25 M FeCl3
determine the molarity of each of the ions present in the following aqueous salt solutions (assume 100% ionization)
2.25M FeCl3
This is done the same way (same concept) as the MgSO4 problem but there are 1 Fe and 3 Cl ions per molecule..
This is unhelpful
To determine the molarity of each ion in a given aqueous solution, you need to know the chemical formula of the compound and its ionic nature. In this case, we have FeCl3, which is iron (III) chloride.
Iron (III) chloride dissociates into iron ions (Fe3+) and chloride ions (Cl-) when it is dissolved in water. Since the problem assumes 100% ionization, we can consider that all the FeCl3 will dissociate into its constituent ions.
Looking at the chemical formula FeCl3, we can see that there is one iron atom (Fe3+) and three chloride ions (3Cl-).
Therefore, the molarity of Fe3+ ions will be the same as the molarity of FeCl3, which is 2.25 M.
On the other hand, the molarity of Cl- ions will be three times the molarity of FeCl3 because there are three chloride ions for every FeCl3 molecule. So, the molarity of Cl- ions will be 3 times 2.25 M, which is 6.75 M.
To summarize:
- The molarity of Fe3+ ions is 2.25 M.
- The molarity of Cl- ions is 6.75 M.