What is the PH of 0.1N CH3COOH solution? The ionisation constant of CH3COOH is 1.8×10−5 . What is the PH of the solutions?

α=k4c =1.8×10-50.1 α=1.34×10−2 CH3COOH⇌H++CH3COO- C O O C(1−α) Cα Cα [H+] = Cα= 0.1 X 1.34 X 10-2P H2−log[H+] =−log[1.34×10−3] P H2=2.87

What is the PH of 0.1N CH3COOH solution? The ionisation constant of CH3COOH is 1.8×10−5 . What is the PH of the solutions?

α=k4c =1.8×10-50.1 α=1.34×10−2 CH3COOH⇌H++CH3COO- C O O C(1−α) Cα Cα [H+] = Cα= 0.1 X 1.34 X 10-2P H2−log[H+] =−log[1.34×10−3] P H2=2.87

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What is the $P^{H}$ of 0.1N $C H_{3} C O O H$ solution? The ionisation constant of $C H_{3} C O O H$ is $1.8 \times 10^{- 5}$ . What is the $P^{H}$ of the solutions?

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4.72

3.39

2.87

3.9

answer is A.

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Detailed Solution

$α= \sqrt{\frac{k_{4}}{c}} = \sqrt{\frac{1.8 \times 10^{-5}}{0.1}} α= 1.34 \times 10^{- 2} \begin{array}{l} {CH}_{3} COOH ⇌ H^{+} + {CH}_{3} {COO}^{-} \\ C O O \\ C (1 - α) Cα Cα \end{array}$
[H⁺] = $Cα$
= 0.1 X 1.34 X 10^-2
${P_{}^{H}}_{2} - \log [H^{+}] = - \log [1.34 \times 10^{- 3}] {P_{}^{H}}_{2} = 2.87$