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
3 answers
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.
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.