If a solution contains 0.65mol of OH−, how many moles of H+ would be required to reach the equivalence point in a titration?
.65moles
To determine the number of moles of H+ required to reach the equivalence point in a titration, we need to use the concept of stoichiometry. The reaction between H+ and OH- is a neutralization reaction, and it proceeds in a 1:1 ratio. This means that one mole of H+ reacts with one mole of OH-.
In this case, we know that the solution contains 0.65 mol of OH-. So, to completely react with this amount of OH-, we would need an equal molar amount of H+. Therefore, the number of moles of H+ required would also be 0.65 mol.
To summarize,
Number of moles of H+ required = Number of moles of OH- = 0.65 mol