Determine the mole fraction of nickel(II) chloride in a 5.54 M aqueous solution of nickel(II) chloride. The density of the solution is 1.28 g mL-1.
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A solution is prepared by dissolving 12.15 g of nickel (II) nitrate in 175 mL of water (density = 1.00 g/mL).
(a) What is the mass percent of nickel (II) nitrate in the solution?
(b) What is the mole fraction of nickel (II) ions in the solution?
Suppose 2.57g of nickel(II) chloride is dissolved in 350.mL of a 38.0mM 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) chloride is dissolved in it.
Be sure your answer has the correct number of significant digits.