Suppose 3.32g of nickel(II) iodide is dissolved in 50mL of a 0.40 M 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.

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Suppose 3.32g of nickel(II) iodide is dissolved in 50mL of a 0.40 M 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.
Suppose 3.32 g of nickel(II) iodide is dissolved in 50. mL of a 0.40 M 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) lodide is dissolved in it.
Round your answer to 2 significant digits.
M
X
S
?
Transcribed Image Text:Suppose 3.32 g of nickel(II) iodide is dissolved in 50. mL of a 0.40 M 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) lodide is dissolved in it. Round your answer to 2 significant digits. M X S ?
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