Question

Question 5 (1 point) How many moles of \( \mathrm{H}^{+} \)are in \( 120.0 \mathrm{~mL} \) of an \( \mathrm{HCl} \) stock solution if a \( 30.00 \mathrm{~mL} \) aliquot was titrated with \( 51.46 \mathrm{~mL} \) of \( 0.1100 \mathrm{M} \mathrm{NaOH} \) ? 0.1887 0.01052 0.04561 0.02264 0.7580

          Question 5 (1 point)
How many moles of \( \mathrm{H}^{+} \)are in \( 120.0 \mathrm{~mL} \) of an \( \mathrm{HCl} \) stock solution if a \( 30.00 \mathrm{~mL} \) aliquot was titrated with \( 51.46 \mathrm{~mL} \) of \( 0.1100 \mathrm{M} \mathrm{NaOH} \) ?
0.1887
0.01052
0.04561
0.02264
0.7580

Question 5 (1 point)
How many moles of H^+are in 120.0 mL of an HCl stock solution if a 30.00 mL aliquot was titrated with 51.46 mL of 0.1100 MNaOH ?
0.1887
0.01052
0.04561
0.02264
0.7580

Added by Stephen M.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Sudhir Kumar

Step 1

The question asks for the total moles of \( \mathrm{H}^{+} \) ions in a 120.0 mL solution of HCl, given that a 30.00 mL aliquot of this solution was titrated with 51.46 mL of 0.1100 M NaOH. Show more…

Show all steps

Thanks for your feedback!

Question 5 (1 point) How many moles of \( \mathrm{H}^{+} \)are in \( 120.0 \mathrm{~mL} \) of an \( \mathrm{HCl} \) stock solution if a \( 30.00 \mathrm{~mL} \) aliquot was titrated with \( 51.46 \mathrm{~mL} \) of \( 0.1100 \mathrm{M} \mathrm{NaOH} \) ? 0.1887 0.01052 0.04561 0.02264 0.7580