What is the total moles of ions in 500 mL of 0.120 M Ca(NO3)2?

how would i calculate this? thanks.

I haven't done chemistry for a while, but here's my best guess:

M = mol/L so 0.120 M means there is 0.12 moles of Ca(NO3)2 in a liter. The question ask for 500 mL, which is half of a litter, so I would just divide 0.12 by two and get 0.06 moles of Ca(NO3)2 in 500 mL.

Again, I'm not 100% sure, but it sounds reasonable to me of how I arrive to this answer.

OK so far but didn't go far enough.

The question is for total mols of ions.
So you have 0.12 mol/L or 0.06 mols/500 mL.
There will be 0.06 mols of Ca^+2, and 2*0.06 mols NO3^- = 0.12 mols NO3^-. The total is 0.06 + 0.12 = 0.18 mol Ca + NO3^-.

To calculate the total moles of ions in a solution, we need to find the number of moles for each ion present in the compound and then multiply it by the number of ions contributed by that compound.

In Ca(NO3)2, there are three ions: one Ca^2+ ion and two NO3^- ions.

To find the moles of each ion, we can start by calculating the moles of the compound.

Given:
Volume of solution (V) = 500 mL = 0.5 L
Concentration of Ca(NO3)2 (c) = 0.120 M

Step 1: Calculate moles of Ca(NO3)2
Moles = concentration × volume
Moles of Ca(NO3)2 = 0.120 mol/L × 0.5 L

Step 2: Calculate moles of Ca^2+ ion
Since there is one Ca^2+ ion per molecule of Ca(NO3)2, the number of moles of Ca^2+ ion is the same as the moles of Ca(NO3)2.

Step 3: Calculate moles of NO3^- ions
Since there are two NO3^- ions per molecule of Ca(NO3)2, we multiply the number of moles of Ca(NO3)2 by the number of NO3^- ions contributed by each molecule, which is 2.

Total moles of NO3^- ions = Moles of Ca(NO3)2 × 2

And that's how you calculate the total moles of ions in the given solution.