For an ion, the number of equivalents you get is equal to the number of moles of that ion multiplied by its valence.
#color(blue)("Eq" = "moles" xx "valence")#
As you know, magnesium is located in group 2 of the periodic table, which means that it has a valence of
So, if your solution contains
#"0.60 moles" * 2 = color(green)("1.2 Eq")#
As an interesting practice example, magnesium chloride,
#"MgCl"_text(2(aq]) -> "Mg"_text((Aq])^(2+) + color(red)(2)"Cl"_text((aq])^(-)#
Notice that every mole of magnesium chloride will produce one mole of magnesium cations and
This means that the solution will contain
Now, in every aqueous solution, the total number of equivalents of anions must be equal to the total number of equivalents of cations.
In this case, the number of equivalents of chloride anions will be
#"1.20 moles" * 1 = "1.2 Eq"#