A hydrogen electrode placed in a buffer solution of $C H_{3} C O O N a$ and $C H_{3} C O O H$ in the ratios $x : y$ and $y : x$ has electrode potential values $E_{1}$ volts and $E_{2}$ volts respectively at 25 $^{0}$ C . The $p K_{a}$ value of acetic acid is :

[ $E_{1}$ and $E_{2}$ are oxidation potentials]

Q. A hydrogen electrode placed in a solution containing sodium acetate and acetic acid in the concentration ratios of

x : y

and

y : x

has electrode potential values

E_{1}

and

E_{2}

volts, respectively, at

25^{\circ} C

. The

p K_{a}

value of acetic acid is:

A hydrogen electrode placed in a buffer solution of $C H_{3} C O O N a$ and $C H_{3} C O O H$ in the molar ratios x : y and y : x has oxidation potentials $E_{1}$ and $E_{2}$ volts respectively at 298 $K, (p_{H_{2}} = 1 a t m)$ . The $p K_{a}$ a value of acetic acid will be given by

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A hydrogen electrode placed in a solution containing sodium acetate and acetic acid in the ratio of x:y and y:x has an electrode potential value E1 and E2 volts, respectively, at 25∘C. The pKa value of acetic acid is:

The correct option is A −(E1+E1)2×0.059Pt|H2|Sodiumacetate+CH3COOH(x:y)pH of acidic buffer = pKa+log(SaltAcid)∴pH1=pKa+logxySimilarly, pH2=pKa+logxy∴E1=−0.059pH1E2=−0.059pH2(E1+E2)=−0.059(pKa+logxy)−0.059(pKa+logyx)pKa=−(E1+E2)2 ×0.059

A hydrogen electrode placed in a solution containing sodium acetate and acetic acid in the ratio of $x : y$ and $y : x$ has an electrode potential value $E_{1}$ and $E_{2}$ volts, respectively, at $25^{\circ} C$ . The $p K_{a}$ value of acetic acid is: