it will be greater than 7.. as there will be more amount of base than acid//
The equivalence or stoichiometric point of a titration of a strong acid versus a strong base is always equal to pH 7.
end point
At the stoichiometric point of a titration, the total amount (in moles) of OH- ions that have been added as a titrant is exactly equal to the amount of H3O+ ions initially present in the beaker.The measured pH of at the stoichiometric point of a strong acid-strong base titration is expected to be that of pure water i.e. pH = 7. In practice, attainment of the stoichiometric point will be marked by sudden sharp rise in pH from a value significantly below 7 to a value significantly above 7.
'Stoichiometric' means equal amounts according to the balanced reaction. So at that point you have only water where H+ and OH- conc.'s are equal (1.0*10-7)
The purpose of a titration is to find the equivalence point (stoichiometric point) of a solution. At the equivalence point, the moles of the titrant and analyte are equal to one another. At the midpoint of the solution, the pKa value is equal to the pH value.
The equivalence or stoichiometric point of a titration of a strong acid versus a strong base is always equal to pH 7.
end point
At the stoichiometric point of a titration, the total amount (in moles) of OH- ions that have been added as a titrant is exactly equal to the amount of H3O+ ions initially present in the beaker.The measured pH of at the stoichiometric point of a strong acid-strong base titration is expected to be that of pure water i.e. pH = 7. In practice, attainment of the stoichiometric point will be marked by sudden sharp rise in pH from a value significantly below 7 to a value significantly above 7.
'Stoichiometric' means equal amounts according to the balanced reaction. So at that point you have only water where H+ and OH- conc.'s are equal (1.0*10-7)
The purpose of a titration is to find the equivalence point (stoichiometric point) of a solution. At the equivalence point, the moles of the titrant and analyte are equal to one another. At the midpoint of the solution, the pKa value is equal to the pH value.
when stoichiometric amounts of the titrant and the analyte have completely reacted. this differs from an endpoint which is when a secondary indicator's color change takes place. :) hope that helps
It is difficult to determine the end point of such a titration, because the titration produces a buffer solution that changes its pH very slowly at the end point, in contrast to reaction between a strong acid and strong base.
The equivalence point is the point in a titration when the amount of added standard reagent is chemically equal to the amount of analyte. The end point is the point in a titration when a physical change occurring immediate after the equivalence point
It is the nearly horizontal region before the equivalence point.
The equivalence point represents a region where the amount of acid to base (or base to acid) concentration is equal. Before the equivalence point there is a greater amount of acid (or base, depending on the titration). After the titration there is a greater amount of base (or acid). This reverse in dominance results in a dramatic change in pH.
The equivalence point, or stoichiometric point, of a chemical reaction is the point at which an added titrant is stoichiometrically equal to the number of moles of substance (known as analyte) present in the sample: the smallest amount of titrant that is sufficient to fully neutralize or react with the analyte.
a strong acid and a weak base.