Calculate the pH of a solution containing 6.0 | vedclass

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(A) $1$. Calculate the molar mass of acetic acid $(CH_3COOH)$: $M = (2 	imes 12) + (4 	imes 1) + (2 	imes 16) = 60 \ g/mol$. $2$. Calculate the num

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(A) $1$. Calculate the molar mass of acetic acid $(CH_3COOH)$: $M = (2 	imes 12) + (4 	imes 1) + (2 	imes 16) = 60 \ g/mol$. $2$. Calculate the number of moles of acetic acid: $n = \frac{6.0 \ g}{60 \ g/mol} = 0.1 \ mol$. $3$. Calculate the molarity $(C)$ of the solution: $C = \frac{0.1 \ mol}{0.250 \ L} = 0.4 \ M$. $4$. For a weak acid,$[H^+] = \sqrt{K_a 	imes C} = \sqrt{1.8 	imes 10^{-5} 	imes 0.4} = \sqrt{0.72 	imes 10^{-5}} = \sqrt{7.2 	imes 10^{-6}} \approx 2.68 	imes 10^{-3} \ M$. $5$. Calculate $pH$: $pH = -\log[H^+] = -\log(2.68 	imes 10^{-3}) = 3 - \log(2.68) \approx 3 - 0.428 = 2.572$.

Calculate the $pH$ of a solution containing $6.0 \ g$ of acetic acid $(CH_3COOH)$ in $250 \ mL$ of water. Given: $K_a = 1.8 \times 10^{-5}$ at $298 \ K$,and atomic masses are $C = 12, H = 1, O = 16$. (in $.57$)

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