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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.
It is the nearly horizontal region before the equivalence point.
In strong acid base titrations when pH meter shows the value 7 then it is equivalence point.
Titration error is simply the difference between the end point of a titration and the equivalence point of it. It can mathematically defined as Error = Vol(End Point) - Vol(Equivalence Point)
a strong acid and a weak base.
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.
It is the nearly horizontal region before the equivalence point.
In strong acid base titrations when pH meter shows the value 7 then it is equivalence point.
Titration error is simply the difference between the end point of a titration and the equivalence point of it. It can mathematically defined as Error = Vol(End Point) - Vol(Equivalence Point)
a strong acid and a weak base.
it depends on the strength of the acid and base used: so, strong acid + strong base = neutral equivalence point strong acid + weak base = acidic equivalence point weak acid + strong base = basic equivalence point In this case, HCl is a strong acid, and Na2CO3 a weak base. Therefore, the equivalence point will be slightly acidic.
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
Assuming you know how to find the equivalence point on the titration curve, and assuming it is not [strong acid/strong base] or [weak acid/weak base], all you need to do is find the half equivalence point, which gives you the pKa of the first solution. Then to get the Ka, you go 10-pKa .
The equivalence or stoichiometric point of a titration of a strong acid versus a strong base is always equal to pH 7.
The chemical process for back titration is to titrate the analyte past the original end point/equivalence point, and then BACK titrate the excess titrant to equivalence.
These terms are synonyms.
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.