What is the resulting pH when of () is mixed with of ()? — Ionic Equilibrium Chemistry Question
Question
What is the resulting pH when $200 \text{ mL}$ of $HCl$ ($pH = 2.0$) is mixed with $300 \text{ mL}$ of $NaOH$ ($pH = 12.0$)?
Answer: B
💡 Solution & Explanation
$HCl$: $[H^+] = 10^{-2} \text{ M}$, mmoles = $200 \times 10^{-2} = 2$. $NaOH$: $[OH^-] = 10^{-2} \text{ M}$, mmoles = $300 \times 10^{-2} = 3$. Excess $OH^-$ = $3 - 2 = 1 \text{ mmole}$. Total volume = $500 \text{ mL}$. $[OH^-] = 1/500 = 2 \times 10^{-3} \text{ M}$. $pOH = 3 - \log 2 = 2.7$. $pH = 14 - 2.7 = 11.3$.
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