When 62.1 moles of calcium acetate are

dissolved in enough water to make 585.1
milliliters of solution, what is the molarity
of acetate ions?
Answer in units of M

Please Explain how to do it because i've been stuck on it and gotten it wrong multiple times

Calcium acetate is Ca(C2H3O2)2 which I abbreviate as Ca(Ac)2.

Remember the definition.
M = mols/L solution.
mols given in the problem as 62.1
volume given as 585.1 mL which is 0.5851 L.
Then 62.1 mols/0.5851 L = 106.136 M for Ca(Ac)2. There are two Ac^- ions in each molecule of Ca(Ac)2 so multiply that by 2 for M Ac.
106.136 x 2 = 212.27. Then look at the number of significant figures allowed and that is 3 from the 62.1 so I would round that to 212 M which is an unusually high value but I guess this is a made up problem.

Alright that makes sense, thank you very much for the help.

To find the molarity of acetate ions in the solution, we need to first determine the number of moles of acetate ions present in the solution, and then divide it by the volume of the solution in liters.

The chemical formula for calcium acetate is Ca(C2H3O2)2, which means there are two acetate ions (C2H3O2-) for every formula unit of calcium acetate.

Given that there are 62.1 moles of calcium acetate dissolved in the solution, this means there are also 62.1 moles of acetate ions present.

To convert the volume of the solution from milliliters to liters, we divide 585.1 milliliters by 1000:
585.1 mL ÷ 1000 = 0.5851 liters

Now we can calculate the molarity of acetate ions by dividing the moles of acetate ions by the volume of the solution in liters:
Molarity = Moles of acetate ions / Volume of solution

Molarity = 62.1 moles / 0.5851 liters

Calculating this division:
Molarity ≈ 105.96 M

Therefore, the molarity of acetate ions in the solution is approximately 105.96 M.