The cell
The cell Pt | H₂(1 bar) | H⁺ || KCl (1.0 M) | Hg₂Cl₂ | Hg | Pt
was used to determine the pH of a 0.01 M -CH₃COOH solution. The cell potential (in V) is:
Given: $K_{a}$ of CH₃COOH = $1.80 \times 1 0^{- 5}$ , $E_{c a l o m e l}^{\circ} = 0.28 V$ , $lo g 1.8 = 0.26$ , $\frac{2.303 RT}{F} = 0.06$ .

Question

The cell

The cell Pt | H₂(1 bar) | H⁺ || KCl (1.0 M) | Hg₂Cl₂ | Hg | Pt

was used to determine the pH of a 0.01 M -CH₃COOH solution. The cell potential (in V) is:

Given: $K_{a}$ of CH₃COOH = $1.80 \times 1 0^{- 5}$ , $E_{c a l o m e l}^{\circ} = 0.28 V$ , $lo g 1.8 = 0.26$ , $\frac{2.303 RT}{F} = 0.06$ .

TestHub · Accepted Answer

Concepts: Nernst equation, weak acid dissociation, pH calculation. Solution: Calculate [ H + ] from K a ​ , then E ce ll ​ = E c a l o m e l ∘ ​ − 0.06 × p H . E ce ll ​ = 0.48 V .

Chemistry - Electrochemistry Question with Solution | TestHub

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