At the equivalence point, the molarities of the two solutions are equal, so the volume of the NaOH required to neutralize the HCl is also 40.0 mL, for the titration.
The concentration of HCl multiplied by the volume of HCl must be equal to the concentration of NaOH multiplied by the volume of NaOH. The concentration of the HCl is 0.120 moles/L and the volume of the sample is 40.0 mL. This means that the concentration of NaOH multiplied by the volume of NaOH must equal 0.120 x 40.0 = 4.8 moles. The concentration of NaOH is also 0.120 moles/L, so the volume of NaOH must be 4.8/0.120 = 40.0 mL. This means that 40.0 mL of 0.120 m NaOH is needed at the equivalence point of the titration to neutralize a 40.0 mL sample of 0.120 m HCl. To determine the volume of 0.120 m NaOH needed at the equivalence point of a titration, the moles of HCl and NaOH must be equal. This means that the concentration of HCl multiplied by the volume of HCl must be equal to the concentration of NaOH multiplied
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