You are titrating 100.0 mL of 0.0400 M Fe2 in 1 M HClO4 with 0.100 M Ce4 to give

Question

You are titrating 100.0 mL of 0.0400 M Fe2 in 1 M HClO4 with 0.100 M Ce4 to give Fe3 and Ce3 using Pt and calomel electrodes to find the endpoint.

(c) From the list in the column at the right, select the two correct Nernst equations for the cell A) E-0.767-0.05916log 0.241 voltage. (Each applying at different points in the titration.) f the calomel electrode is 0.241 V [Fe -0.241 (B) 2.7/ _ 0.241 F0241 Fe-0241 Ce0241 E-0.767-0.059|610g (C) E=1.70-0.05916|og 0.241 (D) (D) E-1.70-0.05916|og| 1-0.24 1 -0241 [ce _ 0.241 [ce -0.241 E E-0.767-0.05916log (d) Calculate the values of E for the cell when the following volumes of the Ce4+ titrant have been added: (Activity coefficients may be ignored as they tend to cancel when calculating concentration ratios.) ( |[G F) E=0.767-0.059 16 log There is additional feedback available! View this feedback by clicking on the G) E-1.70-0.05916log T bottom divider bar, Click on the divider bar again to hide the additional feedback

Explanation / Answer

E^0 (Fe3+/Fe2+) = 0.767 V

E^0(Ce4+/Ce3+) = 1.70 V

two nernst equation are :

E = E^0 (Fe3+/Fe2+) - 0.059/1*log[Fe^2+/Fe3+]

= 0.767- 0.059/1*log[Fe^2+/Fe3+]

E= E^0(Ce4+/Ce3+)- 0.059/1log[Ce^3+/Ce^4+]

= 1.70-0.059/1log[Ce^3+/Ce^4+]

Correct answer : A and G

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