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Question: Dissociation constants of \(\Delta G = RTInK_{c}\)and \(- \Delta G = RTInK_{c}\) in aqueous solution...

Dissociation constants of ΔG=RTInKc\Delta G = RTInK_{c}and −ΔG=RTInKc- \Delta G = RTInK_{c} in aqueous solution are ΔGo=RTInKc\Delta G^{o} = RTInK_{c} If pH of a −ΔGo=RTInKc- \Delta G^{o} = RTInK_{c}solution is 3, what will be the pH of ΔGo\Delta G^{o}?

A

−13.13kcal- 13.13kcal

B

−0.13kcal- 0.13kcal

C

−3.158kcal- 3.158kcal

D

−0.413kcal- 0.413kcal

Answer

−0.413kcal- 0.413kcal

Explanation

Solution

: pH of CH3COOH=3CH_{3}COOH = 3

[H+]=10−3M\lbrack H^{+}\rbrack = 10^{- 3}M from CH3COOHCH_{3}COOH

[NH4OH]=[CH3COOH]=10−3M\lbrack NH_{4}OH\rbrack = \lbrack CH_{3}COOH\rbrack = 10^{- 3}M

[OH−]=10−3M\lbrack OH^{-}\rbrack = 10^{- 3}M

[H+][OH−]=10−14\lbrack H^{+}\rbrack\lbrack OH^{-}\rbrack = 10^{- 14}

[H+]=10−1410−3=10−11\lbrack H^{+}\rbrack = \frac{10^{- 14}}{10^{- 3}} = 10^{- 11}

pH of NH4OH=−log⁡(10−11)=11NH_{4}OH = - \log(10^{- 11}) = 11