Final answer:
To react completely with 9.04 mL of 0.1601 M HCl, 12.13 mL of 0.1192 M NaOH is needed, accounting for the one-to-one mole ratio in the reaction between HCl and NaOH.
Step-by-step explanation:
The question asks how many milliliters of 0.1192 M NaOH solution are required to completely react with 9.04 mL of 0.1601 M HCl solution. To find the answer, the reaction between NaOH and HCl, which is a one-to-one stoichiometric reaction, must be considered:
HCl + NaOH → NaCl + H2O
To calculate the number of moles of HCl, we use the formula:
# mol HCl = volume (L) × molarity (M)
# mol HCl = 0.00904 L × 0.1601 M = 0.001446 mol
Since the stoichiometry of the reaction is 1:1 for HCl to NaOH, the moles of NaOH needed are also 0.001446 mol. To get the volume of NaOH solution needed, use the formula:
Volume NaOH = # mol NaOH / molarity NaOH
Volume NaOH = 0.001446 mol / 0.1192 M
Volume NaOH = 0.01213 L or 12.13 mL
Therefore, you will need 12.13 mL of 0.1192 M NaOH solution to completely react with 9.04 mL of 0.1601 M HCl.