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
why is the answer Hcl and HF but not H2SO4
The answer is HCl and HF because HCl and HF are strong acids, while H2SO4 is a strong acid with two ionizable protons but it is not considered a strong acid in this case.
In a titration, the equivalence point is the point at which the moles of acid are equal to the moles of base. At the equivalence point, all of the HCl or HF in the solution has reacted with the NaOH, resulting in the formation of the respective salt and water.
H2SO4, on the other hand, is a diprotic acid, meaning it can donate two protons. In this case, it would take twice as much NaOH to reach the equivalence point, as each mole of H2SO4 can react with two moles of NaOH. Therefore, H2SO4 is not the correct answer for this particular situation.