Consider the following 0.100M solutions: the equivalence point is reached when 10ml of 0.100M NaOH have been added to 10.00ml of solutions
H2SO4 . HCL. HF
In order to determine the equivalence point, we need to know the balanced chemical equation for the reaction between NaOH and the acids H2SO4, HCl, and HF.
1) H2SO4 + 2NaOH -> Na2SO4 + 2H2O
2) HCl + NaOH -> NaCl + H2O
3) HF + NaOH -> NaF + H2O
From the balanced equations, we can see that for 1 mole of NaOH, we need 1 mole of H2SO4, 1 mole of HCl, and 1 mole of HF for complete neutralization.
Given that we have a 0.100M solution of NaOH, we can calculate the amount of NaOH needed for the equivalence point using the equation:
moles NaOH = concentration (mol/L) x volume (L)
For 10.00 mL of NaOH solution, we have:
moles NaOH = 0.100 mol/L x 0.010 L = 0.001 moles NaOH
Since we need an equal number of moles for H2SO4, HCl, and HF, we would require 0.001 moles of each of these acids for complete neutralization.
To determine the concentration of the acid solutions, we divide the moles of acid by the volume in liters:
H2SO4:
concentration (mol/L) = moles H2SO4 / volume (L)
If we assume the volume of H2SO4 solution is also 10.00 mL, then:
concentration H2SO4 = 0.001 moles / 0.010 L = 0.100 M
HCl:
concentration (mol/L) = moles HCl / volume (L)
If we assume the volume of HCl solution is also 10.00 mL, then:
concentration HCl = 0.001 moles / 0.010 L = 0.100 M
HF:
concentration (mol/L) = moles HF / volume (L)
If we assume the volume of HF solution is also 10.00 mL, then:
concentration HF = 0.001 moles / 0.010 L = 0.100 M
So, for a 0.100M NaOH solution and when 10 mL of NaOH is added to 10.00 mL acid solutions of H2SO4, HCl, and HF, we would reach the equivalence point.