To calculate the volume of HCl required to reach the equivalence point, we need to determine the stoichiometry of the reaction and the molarity of the HCl solution.
Let's assume that we are titrating a 25.0 mL sample of a strong base solution (such as NaOH) with a standardized 0.100 M HCl solution. The balanced chemical equation for the reaction is:
HCl + NaOH -> NaCl + H2O
From the balanced equation, we can see that 1 mole of HCl reacts with 1 mole of NaOH. Therefore, the moles of HCl required to reach the equivalence point can be calculated as:
moles of HCl = volume of NaOH (in L) * concentration of NaOH
moles of HCl = 0.025 L * 0.100 mol/L = 0.0025 mol
Since the stoichiometry of the reaction is 1:1, the moles of HCl required are the same as the moles of NaOH in the sample. Therefore, the volume of HCl required to reach the equivalence point is:
volume of HCl = moles of HCl / concentration of HCl
volume of HCl = 0.0025 mol / 0.100 mol/L = 0.025 L or 25.0 mL
Therefore, 25.0 mL of HCl is required to reach the equivalence point.
To calculate the pH at 0.0, 10.0, 25.0, and 30.0 mL of titrant in the titration, you should consider the initial pH of the base solution and the pH changes associated with the addition of the HCl titrant. This calculation requires knowledge of the concentrations and dissociation constants of the acid and base involved in the titration.
Calculate the
• (i) Volume of HCl required to reach the equivalence point.
• (ii) pH at 0.0, 10.0, 25.0, and 30.0 mL of titrant in the titration
1 answer