2. How many milliliters of 0.653 M NaOH are needed to neutralize 25.0 mL of a 1.02 M HBr solution? The neutralization reaction is:
NaOH(aq) + HBr(aq) → H2O(l) + NaBr(aq)
To find the amount of NaOH needed to neutralize the HBr solution, we first need to determine the moles of HBr in the solution:
Moles of HBr = Molarity of HBr x Volume of HBr solution
Moles of HBr = 1.02 mol/L x 0.025 L = 0.0255 moles
Since the neutralization reaction is 1:1, we need the same number of moles of NaOH to neutralize the HBr.
Now, we can calculate the volume of 0.653 M NaOH needed:
Moles of NaOH = 0.0255 moles
Volume of NaOH = Moles of NaOH / Molarity of NaOH
Volume of NaOH = 0.0255 moles / 0.653 mol/L ≈ 39.1 mL
Therefore, approximately 39.1 mL of 0.653 M NaOH are needed to neutralize 25.0 mL of a 1.02 M HBr solution.