The dissociation constant for $$CH_{3}COOH$$ is $$1.8\times 10^{-5}$$ at $$298\ K$$. The electrode potential for the half-cell: $$Pt|H_{2}\ (1\ bar)\|0.5\ M\ CH_{3}COOH$$, at $$298\ K$$ is:
In the cell Pt(s),H2(g)|1barHCl(aq)|Ag(s)|Pt(s) the cell potential is 0.92 when 10−6 molal HCl solution is used. The standard electrode potential of (AgCl/Ag,Cl−) electrode is:
[Given: 2.303RTF=0.06V at 298K]
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Q2
The potential of the cell containing two hydrogen electrodes as represented below, is:
Pt,H2(g)|H+(10−6M)||H+(10−4M)|H2(g),Pt at 298K
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Q3
The change in potential of the half-cell Cu2+/Cu, when aqueous Cu2+ solution is diluted 100 times at 298K?
[2.303RTF=0.06].
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Q4
The degree of dissociation of water is 1.8×10−9 at 298K. Calculate the ionisation constant and ionic product of water at 298K.
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Q5
The standard reduction -potential for the half-cell: NO−3(aq)+2H++e−→NO2(g)+H2O is 0.78V.