Question

A `0.600*mol` quantity of magnesium acetate is dissolved in `135*mL` of water, what are the concentrations with respect to magnesium and acetate ions?

Answer 1

When we report `"concentration"` we take the quotient...
`"concentration"="moles of solute"/"volume of solution"`

Explanation:

And thus, reasonably, we get units of `mol*L^-1`....

And thus with respect to `"magnesium acetate"` we gots a concentration of..........

`(0.600*mol)/(135*mLxx10^-3*L*mL^-1)=4.44*mol*L^-1`

And since we got `Mg{O(O=)C-CH_3}_2`...

`[Mg^(2+)]=4.44*mol*L^-1`

But....

`[{""^(-)O(O=)C-CH_3}]=8.88*mol*L^-1`.

And so because of the stoichiometry of the salt, acetate anion is TWICE as concentrated as magnesium cation. With me?