For strong acid/strong base reactions: pH 7 is the equivalence point
For titration of a weak base with strong acid : pH 6-3 is the equivalence point
For titration of a weak acid with strong base : pH 8-11 is the equivalence point
For weak acid/weak base reactions it is also around pH 7, but it happens so NON-sharply, vague, that titrations can't be used for these.
Without seeing the curve, we can't answer this.
In strong acid base titrations when pH meter shows the value 7 then it is equivalence point.
pH = 5.56 at 36.0 ml(equivalence point)
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.
It depends on the equivalence point of the solutions you're titrating.
Without seeing the curve, we can't answer this.
In strong acid base titrations when pH meter shows the value 7 then it is 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 indicator should change color right at the equivalence point, so 5.
pH = 5.56 at 36.0 ml(equivalence point)
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.
It depends on the equivalence point of the solutions you're titrating.
when the equivalence point of a titration is achieved.. Added: (More precisely:) The equivalence point is the point where the number of moles of base equal the number of moles of acid. The end point is the point where the indicator being used changes color (also 'indication point)'. If the indicator is chosen correctly, the end point will essentially be exactly as near as possible at the equivalence point. The point of the titration is to find the equivalence point -- the end point is just a very close approximation to it. This is because the pH of the solution changes very rapidly close to the equivalence point. Therefore, the indicator will change color very close to the equivalence point because of the steepness of the pH change
The pH at point of halfway titration is at pKa level (this even might be at pH above 7)andpH of equivalence point (end point) is not at pH = 7.0 , but (sometimes far) above 7.0.
The equivalence point is the point where the number of moles of base equal the number of moles of acid. The end point is the point where the indicator being used changes color (also 'indication point)'. If the indicator is chosen correctly, the end point will essentially be exactly as near as possible at the equivalence point. The point of the titration is to find the equivalence point -- the end point is just a very close approximation to it. This is because the pH of the solution changes very rapidly close to the equivalence point. Therefore, the indicator will change color very close to the equivalence point because of the steepness of the pH change.
The equivalence or stoichiometric point of a titration of a strong acid versus a strong base is always equal to pH 7.
Phenolphthalein changes from colorless to red in the range of pH = 8.0 to 9.6