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In section G of the text book, there are a lot of questions regarding multiple ionic compounds that share an ion and having to solve for the molarity of the common ion. Does it matter what ion the ion we are solving for is bonded to? Sorry if this doesn't make sense :/
It kind of matters what the ion is bonded to when determining the concentration of the ion. You need to first find the concentrations of the individual compounds and then use the appropriate molar ratio to determine the ion's concentration. Once you have found the concentration of the ion from each compound, you can find the total concentration.
Last edited by Rachana Jayaraman 1H on Wed Oct 03, 2018 4:40 pm, edited 1 time in total.
When ions dissolve in aqueous solutions, they undergo ionic dissociation, meaning the individual ions are freed from their bonds. For example, when NaCl is dissolved in water, the cation Na+ and anion Cl- completely separate. So, no, it really shouldn’t matter what ion the ion you are solving for is bonded to because in solution, the ions are no longer involved in the bond. But you must take into consideration the molar ratios of the individual ions and the ionic compounds when solving for molarity!
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