Question

Suppose of nickel(II) iodide is dissolved in of a 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. Round your answer to significant digits.

Answer 1

Answer:

0.619 M to 3 significant figures.

Explanation:

1 mole of $NiI_{2}$ - 312.5 g

? mole of $NiI_{2}$ - 2.9 g

= 2.9/312.5

= 0.0928 moles.

Concentration = no. of moles/vol in litres = $\frac{0.0928}{0.150L}$

= 0.619 M