$I_{2}(s)|{\ I}^{-}(0.1\ M)$ half-cell is connected to a $H^{+}(aq)|{\ H}_{2}(1\ bar)|$ Pt half-cell and emf is found to be 0.7714 V. If $E_{I_{2}/I^{-}}^{{^\circ}} = 0.535\ V,$ find the $pH\$of$\ H^{+}/H_{2}$ half-cell

Question

Dr. Abubacker · Accepted Answer

(c)
The cell reaction is
$H_{2}(g) + I_{2}(s) ightleftharpoons 2H^{+}(aq) + 2I^{-}(aq)$
$0.7714 = 0.535 - \frac{0.0591}{2}\log\frac{\left\lbrack H^{+} ightbrack^{2}\left\lbrack I^{-} ightbrack^{2}}{p_{H_{2}}}$
$	herefore pH = 3$

Q. $I_{2}(s)|{\ I}^{-}(0.1\ M)$ half-cell is connected to a $H^{+}(aq)|{\ H}_{2}(1\ bar)|$ Pt half-cell and emf is found to be 0.7714 V. If $E_{I_{2}/I^{-}}^{{^\circ}} = 0.535\ V,$ find the $pH\$of$\ H^{+}/H_{2}$ half-cell

Explanation

Reviewed by Dr. Abubacker

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