When 23.5 moles of calcium acetate are
dissolved in enough water to make 825.9
milliliters of solution, what is the molarity
of acetate ions?
Answer in units of M.
.00284538
To find the molarity of acetate ions in the solution, we first need to determine the number of moles of acetate ions present in the solution.
Calcium acetate consists of one calcium ion (Ca2+) and two acetate ions (C2H3O2-). Since each formula unit of calcium acetate produces two acetate ions, the number of moles of acetate ions will be twice the number of moles of calcium acetate.
Given that there are 23.5 moles of calcium acetate, we can calculate the number of moles of acetate ions:
Number of moles of acetate ions = 2 × moles of calcium acetate
= 2 × 23.5 moles
= 47 moles
Now, we need to find the molarity of the acetate ions. Molarity (M) is defined as the number of moles of solute (acetate ions in this case) divided by the volume of the solution in liters.
Given that the volume of the solution is 825.9 milliliters, we need to convert it to liters:
Volume of solution = 825.9 milliliters = 825.9 mL = 825.9 / 1000 liters
= 0.8259 liters
Finally, we can calculate the molarity of the acetate ions:
Molarity of acetate ions = moles of acetate ions / volume of solution in liters
= 47 moles / 0.8259 liters
≈ 56.94 M
Therefore, the molarity of acetate ions in the solution is approximately 56.94 M.
M = moles/L
Substitute and solve.