Suppose 4.32 g of nickel(II) iodide is dissolved in 350. mL of a 47.0 m 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. Be sure your answer has the correct number of significant digits. OM X Ś
Suppose 4.32 g of nickel(II) iodide is dissolved in 350. mL of a 47.0 m 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. Be sure your answer has the correct number of significant digits. OM X Ś
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Suppose 4.32 g of nickel (II) iodide is dissolved in 350. mL of a 47.0 m 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.
Be sure your answer has the correct number of significant digits.
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Expert Solution
Step 1: Write the net ionic equation
The balanced equation for the reaction between Nickel(II) iodide and potassium carbonate is
NiI2 (aq) + K2CO3 (aq) --------> NiCO3 (s) + 2 KI (aq)
The total ionic equation is
Ni+2 (aq) + 2 I– (aq) + 2 K+ (aq) + CO3–2 (aq) ---------> NiCO3 (s) + 2 K+ (aq) + 2 I– (aq)
The net ionic equation is
Ni+2 (aq) + CO3–2 (aq) ---------> NiCO3 (s)
Iodide ion is the spectator ion in this reaction. It does not involve in the reaction.
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