Suppose 15.2 g of nickel(II) iodide is dissolved in 200. mL of a 0.50 M aqueous solution of potassium carbonate.
Calculate the final molarity of nickel(II) cation in the solution. You can assume the volume of the solution doesn't change when the nickel(II) iodide is dissolved in it.
Be sure your answer has the correct number of significant digits.
Molarity = moles / liter
mass of NiCl2 = 15.2 g; molar mass of NiCl2 = 129.5994 g/mol
moles NiCl2 = 15.2g / 129.5994 g/mol = 0.1172844936 mol
volume = 200 mL = 0.2 L
Molarity = 0.1172844936 mol / 0.2 L = 0.586422468 M
Answer: 0.586 M = 586 x 10-3 M
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