When 100 , mL of M/10 , NaOH solution and 50 | vedclass

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(B) Step $1$: Calculate the millimoles of $NaOH$.$n(NaOH) = M 	imes V(mL) = \frac{1}{10} 	imes 100 = 10 \, mmol$.Step $2$: Calculate the millimoles

Vedclass · Accepted Answer

$7$

Vedclass · Answer

(B) Step $1$: Calculate the millimoles of $NaOH$.$n(NaOH) = M 	imes V(mL) = \frac{1}{10} 	imes 100 = 10 \, mmol$.Step $2$: Calculate the millimoles of $HCl$.$n(HCl) = M 	imes V(mL) = \frac{1}{5} 	imes 50 = 10 \, mmol$.Step $3$: Since $NaOH$ and $HCl$ react in a $1:1$ molar ratio $(NaOH + HCl ightarrow NaCl + H_2O)$,the $10 \, mmol$ of $NaOH$ will exactly neutralize $10 \, mmol$ of $HCl$.Step $4$: As both reactants are completely consumed,the resulting solution contains only $NaCl$ (a salt of a strong acid and a strong base),which is neutral.Therefore,the $pH$ of the resulting solution is $7$.

When $100 \, mL$ of $M/10 \, NaOH$ solution and $50 \, mL$ of $M/5 \, HCl$ solution are mixed,the $pH$ of the resulting solution would be:

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