What is the pH of a solution obtained by diss | vedclass

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(C) $1$. Calculate the number of moles of $NaOH$: $n = \frac{	ext{mass}}{	ext{molar mass}} = \frac{0.2 \, g}{40 \, g/mol} = 0.005 \, mol$. $2$. Calc

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(C) $1$. Calculate the number of moles of $NaOH$: $n = \frac{	ext{mass}}{	ext{molar mass}} = \frac{0.2 \, g}{40 \, g/mol} = 0.005 \, mol$. $2$. Calculate the molarity $(M)$ of the solution: $M = \frac{n}{V(L)} = \frac{0.005 \, mol}{0.1 \, L} = 0.05 \, M$. $3$. Since $NaOH$ is a strong base,$[OH^-] = 0.05 \, M = 5 	imes 10^{-2} \, M$. $4$. Calculate $pOH$: $pOH = -\log[OH^-] = -\log(5 	imes 10^{-2}) = 2 - \log(5) = 2 - 0.699 = 1.301$. $5$. Calculate $pH$: $pH = 14 - pOH = 14 - 1.301 = 12.699$.

What is the $pH$ of a solution obtained by dissolving $0.2 \, g$ of $NaOH$ in $100 \, mL$ of water (in $.699$)?

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