One mole of each of the following compounds is added to water in separate flasks to make 1.0 L of solution. Which solution has the largest total ion concentration?
a. aluminum hydroxide
b. silver chloride
c. sodium chloride
d. calcium carbonate
e. potassium phosphate

I just need help finding out how to calculate the ion concentration of a solution with just the given known. what formula do i need to use for this question?

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  1. You don't need a formula and you don't need to calculate the molarity. The problem tells you that you have 1 MOLE of each of the compounds ADDED to H2O to make 1 L of soln.
    What you need to know is the solubility of the compound as well as the formula of the compound. For example, the first two are not very soluble at all; therefore, the ionic concn is small (although you CAN calculate the (Al^3+) and (OH^-) from Ksp data and (Ag^+) and (Cl^-) from Ksp data if you wish.) NaCl is quite soluble so the (Na^+) is 1 mole/L and the Cl^- is 1 mole/L for a total of 2 moles ion/L. How soluble is CaCO3? How soluble is K3PO4? If they are soluble to any extent, calculate the concn of the ions in those solns and you will have your answer.

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  2. does the ratio between the cation and anion affect the ionic concentration? like, the ratio between K and PO4 is 3:1, so it's more likely that it'll be soluble, in comparison to the Al and OH which is 1:3 (which is not soluble)?

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  3. Yes, it does affect the ratio; however, that has little to do with the solubility. Here is a simplified set of solubility rules. You need to memorize these. CaCO3 is largely insoluble. K3PO4 is soluble and ionizes into 3K^+ and 1PO4^3-.

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  4. Thank you so much!!!

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  5. its e

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