Uppose of nickel(ii) iodide is dissolved in of a aqueous solution of potassium carbonate. calculate the final molarity of iodide anion 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.

Explanation:

Let us assume that mass of nickel(II) iodide is 2.90 g, volume is 150.ml, and concentration is 0.70 M.

When is added into the solution then it will not affect the concentration.

Moles of =

                          =

                          = 0.00928 mol

Moles of =

                  =

                 = 0.01856 mol

Molarity of =

                        =

                        = 0.124 M

Thus, we can conclude that final molarity of iodide anion in the solution is 0.124 M.

wher is the rest of the question