Question

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.

 

Answer 1

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

O STOICHIOMETRY Solving limiting reactant problems in solution Nicole 8 Suppose 15.2 g of nickel(I1) iodide is dissolved in 200. mL of a 0.50 M aqueous solution of potassium carbonate. Calculate the final molarity of nicke!(TI) 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 nificant digits 58610-3

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