6.00 mL of 5.00 x 10-3 M Fe(NO3)3 (5.00 times 10 to the minus 3rd power M F e (NO3)3) is added to 9.00 mL of 7.00 x 10-3 M KSCN (7.00 times 10 to the minus 3rd power M KSCN) along with 5.00 mL of water. The concentration of [F e(SCN)2+] was found to be 2.00 x 10-3 M (2.00 times 10 to the minus 3rd power M) at equilibrium. How many initial moles of SCN^- are present in the solution? Express your answer as a decimal number (no exponents).

Answered: 6.00 mL of 5.00 x 10-3 M Fe(NO3)3 (5.00…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

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6.00 mL of 5.00 x 10^-3 M Fe(NO₃)₃ (5.00 times 10 to the minus 3rd power M F e (NO3)3) is added to 9.00 mL of 7.00 x 10^-3 M KSCN (7.00 times 10 to the minus 3rd power M KSCN) along with 5.00 mL of water. The concentration of [F e(SCN)²⁺] was found to be 2.00 x 10^-3 M (2.00 times 10 to the minus 3rd power M) at equilibrium. How many initial moles of SCN^- are present in the solution? Express your answer as a decimal number (no exponents).

Expert Solution

Step 1

Volume of Fe(NO3)3 = 6ml

Concentratio of Fe(NO3)3 = 5×10^-3M

Volume of KSCN = 9ml

Concentratio of KSCN = 7×10^-3M

Volume of water = 5ml

Equilibrium concentration of Fe(SCN)²⁺ = 2×10^-3

We are asked to calculate the initial moles of SCN^-present.

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