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(A) $1$. Calculate the millimoles of $H^+$ ions from $H_2SO_4$: $n(H^+) = 2 	imes M 	imes V = 2 	imes 0.05 \ M 	imes 300 \ mL = 30 \ mmol$. $2$. C

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(A) $1$. Calculate the millimoles of $H^+$ ions from $H_2SO_4$: $n(H^+) = 2 	imes M 	imes V = 2 	imes 0.05 \ M 	imes 300 \ mL = 30 \ mmol$. $2$. Calculate the millimoles of $OH^-$ ions from $KOH$: $n(OH^-) = M 	imes V = 0.05 \ M 	imes 150 \ mL = 7.5 \ mmol$. $3$. Calculate the remaining $H^+$ after neutralization: $n(H^+)_{rem} = 30 - 7.5 = 22.5 \ mmol$. $4$. Calculate the total volume of the solution: $V_{total} = 300 \ mL + 150 \ mL = 450 \ mL$. $5$. Calculate the concentration of $H^+$: $[H^+] = \frac{22.5 \ mmol}{450 \ mL} = 0.05 \ M$. $6$. Calculate $pH$: $pH = -\log[H^+] = -\log(0.05) = -\log(5 	imes 10^{-2}) = 2 - \log(5) = 2 - 0.699 = 1.301$.

Calculate the $pH$ of a mixed solution containing $300 \ mL$ of $0.05 \ M \ H_2SO_4$ and $150 \ mL$ of $0.05 \ M \ KOH$. (in $.301$)

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