An electrochemical cell consists of a hydrogen electrode (p(H2) = 1 bar) immersed in an acid solution and a silver electrode immersed in a saturated Ag2CO3 solution. The electromotive force is 0.064 V at 298 K and the hydrogen electrode is found at the anode. Calculate the concentration of the H+ ion in the hydrogen electrode. [E\deg (Ag+/Ag) = 0.800 V, Ksp(Ag2CO3) = 8.5 \times 10-12].
An electrochemical cell consists of a hydrogen electrode (p(H2) = 1 bar) immersed in an acid solution and a silver electrode immersed in a saturated Ag2CO3 solution. The electromotive force is 0.064 V at 298 K and the hydrogen electrode is found at the anode. Calculate the concentration of the H+ ion in the hydrogen electrode. [E\deg (Ag+/Ag) = 0.800 V, Ksp(Ag2CO3) = 8.5 \times 10-12].
Chemistry
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![An electrochemical cell consists of a hydrogen electrode (p(H2) = 1 bar) immersed in an acid solution and a
silver electrode immersed in a saturated Ag2CO3 solution. The electromotive force is 0.064 V at 298 K and the
hydrogen electrode is found at the anode. Calculate the concentration of the H+ ion in the hydrogen
electrode.
[E\deg (Ag+/Ag) = 0.800 V, Ksp(Ag2CO3) = 8.5 \times 10-12].](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7bbf17ef-66de-465d-8951-24687428512e%2F76e1acab-2e50-4fad-a103-48a4a032c76a%2Fp2t0mbd_processed.png&w=3840&q=75)
Transcribed Image Text:An electrochemical cell consists of a hydrogen electrode (p(H2) = 1 bar) immersed in an acid solution and a
silver electrode immersed in a saturated Ag2CO3 solution. The electromotive force is 0.064 V at 298 K and the
hydrogen electrode is found at the anode. Calculate the concentration of the H+ ion in the hydrogen
electrode.
[E\deg (Ag+/Ag) = 0.800 V, Ksp(Ag2CO3) = 8.5 \times 10-12].
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