A standard solution of FeSCN^2+ is prepared by combining 9.0 mL of 0.20 M Fe(NO_

Question

A standard solution of FeSCN^2+ is prepared by combining 9.0 mL of 0.20 M Fe(NO_3)_3 1.0 mL of 0.0020 M KSCN. The equation for the reaction is as follows. Fe(NO_3)_3+KSCN FeSCN^2+ + KNO_3 + 2NO_3^- What allows us to assume that the reaction goes essentially to completion? The excess Fe^3+ prevents the formation of the neutral Fe(SCN)_3. The concentration of Fe(NO_3)_3 is much higher than the concentration of KSCN. The reaction quotient Q is greater than K_c. Under the conditions given above, LeChatelier's principle dictates that the reaction shifts to the left. The equilibrium reaction has a very high K_c. Based on that assumption, what is the equilibrium concentration of FeSCN^2+

Explanation / Answer

The equilibrium reaction has a very high Kc.

No.of moles of FeSCN2+ produced = no.of moles of KCN

therefore conc. Of FeSCN2+ = 1.00 x 0.0020/ 10.0 = 0.0002 M

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