Suppose 0.829g of zinc chloride is dissolved in 100.mL of a 0.60M aqueous solution of potassium carbonate. Calculate the final molarity of chloride anion in the solution. You can assume the volume of the solution doesn't change when the zinc chloride is dissolved in it. Be sure your answer has the correct number of significant digits.

Molarity of   anion in solution is 0.122 M.

Explanation:

Chemical Reaction:

As KCl is a strong electrolyte therefore it dissociates completely in solution. Hence present in final solution is equal to present in 0.829 g of  .

Molar mass of = 136.286 g/mol

So, 0.829 g of = moles of

1 mol of contains 2 moles of .

Hence number of moles of in solution = moles

So, molarity of in solution = [(number of moles of in solution)/(volume of solution in mL)]

= M

= 0.122 M

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