Part one: Fe 3+ reacts with SCN - to form FeSCN 2+ . If 2.0 mL of a 2.3 M soluti

Question

Part one: Fe3+ reacts with SCN- to form FeSCN2+. If 2.0 mL of a 2.3 M solution of Fe3+ is mixed with 2.0 mL of a 0.161 M solution of SCN- and 6.0 mL of water, calculate the concentration of FeSCN2+ in the resulting solution after the reaction completes. Correct significant figures are required to receive credit. Do NOT include units in your answer.

Part two: Fe3+ reacts with SCN- to form FeSCN2+. If 2.0 mL of 0.493 M Fe3+ are mixed with 2.0 mL of 0.104 M SCN- and 6.0 mL of water, calculate the concentration of leftover Fe3+ in the solution after the reaction completes. Correct significant figures are required to receive credit. Do NOT include units in your answer.

Explanation / Answer

Part one : moles of Fe3+ = 2.3 M x 2.0 ml = 4.6 mmol

moles of SCN- = 0.161 M x 2.0 ml = 0.322 mmol

Total volume of solution = 2 + 2 + 6 = 10 ml

concentration of [FeSCN^2+] = 0.322/10 = 0.0322

Part two : moles of Fe3+ = 0.493 M x 2.0 ml = 0.986 mmol

moles of SCN- = 0.104 M x 2.0 ml = 0.208 mmol

Total volume of solution = 2 + 2 + 6 = 10 ml

concentration of [FeSCN^2+] = 0.208/10 = 0.0208

Concentration of leftover [Fe3+]= 0.778/10 = 0.0778

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