Answer:
In this problem, we can use the concept of acid-base titration to determine the volume of HCl required to neutralize the NaOH solution. The balanced chemical equation for the reaction between HCl and NaOH is:
HCl + NaOH → NaCl + H2O
From the equation, we can see that 1 mole of HCl reacts with 1 mole of NaOH. Therefore, the number of moles of NaOH in the solution is:
moles of NaOH = Molarity × Volume = 1.5 M × 0.080 L = 0.12 moles
Since 1 mole of HCl reacts with 1 mole of NaOH, the number of moles of HCl required to neutralize the NaOH solution is also 0.12 moles.
The molarity of the HCl solution is 4.5 M. We can use the following equation to calculate the volume of HCl required:
moles of HCl = Molarity × Volume
Rearranging the equation gives:
Volume = moles of HCl / Molarity
Substituting the values we have:
Volume = 0.12 moles / 4.5 M = 0.0267 L
Therefore, the volume of 4.5 M HCl solution required to neutralize the 1.5 M NaOH solution is 0.0267 L, or 26.7 mL (since 1 L = 1000 mL).