Suppose 1.47 g of zinc iodide is dissolved in 100. mL of a 76.0m M aqueous solution of potassium carbonate. Calculate the final molarity of zinc cation in the solution. You can assume the volume of the solution doesn't change when the zinc iodide is dissolved in it. Be sure your answer has the correct number of significant digits
Suppose 1.47 g of zinc iodide is dissolved in 100. mL of a 76.0m M aqueous solution of potassium carbonate.
Calculate the final molarity of zinc cation in the solution. You can assume the volume of the solution doesn't change when the zinc iodide is dissolved in it.
Be sure your answer has the correct number of significant digits.
This question involves calculating the final molarity of zinc cation (Zn2+) in a solution that initially contains a specific amount of zinc iodide (ZnI2) and potassium carbonate (K2CO3).
To solve the problem, we need to first determine the number of moles of ZnI2 that are present in the solution, since this is the source of Zn2+ ions. We do this by using the molecular weight of ZnI2 and the given mass of ZnI2.
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