Question

Suppose 1.87g of nickel(II) bromide is dissolved in 200.mL of a 52.0mM 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) bromide is dissolved in it.
Be sure your answer has the correct number of significant digits.
The answer is needed in M.

Answer 1

0.0428 M

Step-by-step explanation:

Because we're asked to calculate the molarity of nickel(II) cation, we need to determine all sources for that species, in this case, all Ni⁺² comes from the nickel(II) bromide solid (NiBr₂).

We use the molecular weight of NiBr₂ to calculate the moles of Ni:

1.87 g NiBr₂ ÷ 218.49g/mol * (1molNi⁺²/1molNiBr₂) = 8.55x10⁻³ mol Ni⁺²

Then we divide the moles by the volume in order to calculate the concentration:

8.55x10⁻³ mol Ni⁺² / 0.200 L = 0.0428 M