Redox Reactions And Electrochemistry Question 561
Question: $ I_2(s)|{I^{-}}(0.1M) $ half-cell is connected to a $ {H^{+}}( aq )| H_2( 1bar ) |Pt $ half cell and e.m.f. is found to be $ 0.7714V.if,{E^{{}^\circ }}_{I_2|{I^{-}}}=0.535V $ , find the pH of $ {H^{+}}|H_2 $ half-cell.
Options:
A) 1
B) 3
C) 5
D) 7
Show Answer
Answer:
Correct Answer: B
Solution:
[b] The cell reaction is $ H_2(g)+I_2(s)\rightarrow 2{H^{+}}(aq)+2{I^{-}}(aq) $ $ 0.7714=0.535-\frac{0.0591}{2}\log \frac{{{[{H^{+}}]}^{2}}{{[{I^{-}}]}^{2}}}{{P_{H_2}}} $ pH=3
BETA
