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A 50.0 mL sample of a 1.50 M NaOH solution is titrated with a 1.56 M HCl solution. What will be the final volume of the solution when the NaOH has been completely neutralized by the HCl?

a. 98.1 mL
b. 48.1 mL
c. 83.1 mL
d. 167 mL
e. 2.7 mL

Answer :

Final answer:

To calculate the final volume in a titration, the moles of the acid and base that react are determined, and from this, the volume of the titrant needed for complete neutralization is found. The calculated final volume when 1.50 M NaOH is titrated with 1.56 M HCl is a. 98.1 mL.

Explanation:

To determine the final volume of solution when the 50.0 mL of 1.50 M NaOH is completely neutralized by 1.56 M HCl, we need to calculate the amount of HCl needed to completely react with NaOH.

Step by Step Titration Calculation:

  1. Write the balanced equation: NaOH + HCl → NaCl + H₂O.
  2. Calculate moles of NaOH: moles = concentration (M) × volume (L) = 1.50 M × 0.050 L = 0.075 moles.
  3. Since the reaction ratio is 1:1, moles of HCl needed for neutralization is also 0.075 moles.
  4. Calculate the volume of HCl needed: 0.075 moles ÷ 1.56 M = 0.04808 L or 48.08 mL.
  5. Add the volumes of NaOH and HCl to determine final volume: 50.0 mL + 48.08 mL = 98.08 mL, which can be rounded to 98.1 mL (answer option a).

Since 98.1 mL is the closest to the calculated final volume, option a. is the correct answer.

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