Question
How many milliters of 2.00 $\mathrm{M} \mathrm{HCl}$ must be added to neutralize the following solutions?(a) a mixture of 0.160 $\mathrm{M} \mathrm{HNO}_{3}(100.0 \mathrm{mL})$ and 0.100 $\mathrm{M}$ $\mathrm{KOH}$ $(400.0 \mathrm{mL})$(b) a mixture of 0.120 $\mathrm{M} \mathrm{NaOH}(350.0 \mathrm{mL})$ and 0.190 $\mathrm{M}$ $\mathrm{HBr}$ (150.0 $\mathrm{mL} )$
Step 1
For the first solution, we have 100.0 mL of $\mathrm{HNO}_{3}$ which is 0.1000 L. The molarity is 0.160 M, so the moles of $\mathrm{H}^{+}$ ions is $0.1000 \, \mathrm{L} \times 0.160 \, \mathrm{M} = 0.0160 \, \mathrm{mol}$. Show more…
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How many milliliters of $1.00 \mathrm{M}$ KOH must be added to neutralize the following solutions? (a) A mixture of $0.240 \mathrm{M} \mathrm{LiOH}(25.0 \mathrm{~mL})$ and $0.200 \mathrm{M} \mathrm{HBr}$ $(75.0 \mathrm{~mL})$ (b) A mixture of $0.300 \mathrm{M} \mathrm{HCl}(45.0 \mathrm{~mL})$ and $0.250 \mathrm{M} \mathrm{NaOH}$ $(10.0 \mathrm{~mL})$
How many milliliters of 1.00 $\mathrm{M} \mathrm{KOH}$ must be added to neutralize the following solutions? (a) a mixture of 0.240 $\mathrm{M}$ LiOH $(25.0 \mathrm{mL})$ and 0.200 $\mathrm{M}$ HBr $(75.0 \mathrm{mL})$ (b) a mixture of 0.300 $\mathrm{M} \mathrm{HCl}(45.0 \mathrm{mL})$ and 0.250 $\mathrm{M} \mathrm{NaOH}$ $(10.0 \mathrm{mL})$
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