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How does the equivalence point differ from the half equivalence point?
Wiki User
∙ 14y ago
Equivalence point is reached when Reactants react at Stoichiometric ratios and reach the Endpoint so that no more of the solution being titrated is found.
Eg: Strong base + Strong Acid: HCL+NaOH--> NaCl+H2O
1mol of Hcl Requires 1 mol of NaCl,
Therefore 3.65 moles of Hcl Requires 3.65Moles of NaOH and equivalence point is reached when that much is added to the acid being titrated for example .
Half Eq point is when Half of the Solution being titrated has reacted. It is a point on a titration curve which corresponds to the addition of exactly half of the volume of the titrant needed to reach equivalence point (or end point )
Corrected:
So, at HALF-WAY Eq. point the pH = pKa, since the actual concentration of ACID is equal to concentration of its conjugate BASE because both are equal to HALF of the original (unknown) acid concentration to be titrated (half left = half formed).
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∙ 14y ago
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The equivalence point reached when the pH reaches it maximum value?
No. The equivalence point is reached when the moles of titrant equals the moles of analyte.
If the equivalence point of a titration is 5 what range of pH should the indicator be?
The indicator should change color right at the equivalence point, so 5.
What is the chemical process for back titration?
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.
What is the point in a titration at which the added solute reacts completely with the solute present in the solution?
It is the equivalence point.
Why does the pH change rapidly at the equivalence point of a titration?
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.
How does the equivalence point of a titration differ from its end point?
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.
What is the difference between the end point and the equivalence point?
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
In a titration when does the indicator change color?
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
Equivalence point and endpoint pH and pKa How do they relate?
Endpoint (also called indication point) should be as near as possibly be at equivalence point, it is indicated by sudden change of pH or the color of an appropriate indicator.pH of Equivalence point of strong acid or base analyte is 7.0 (+/- 1.5 unit)Of weak acids and bases:pH of Equivalence point of weak acid or base analyte= (about) 14 - 0.5*[ pKb + pCb ] for weak acid analytes (+/- 1.0 unit)or= (about) 0.5*[ pKa + pCa] for weak base analytes (+/- 1.0 unit)in which'p' means negative log10(value)Ka and Kb means acid and base constants (of the analyt conjugated pair)Ca and Cb means actual acid and base concentration (of the analyte conjugates)At HALF-WAY equivalence point the pH = pKa, since the actual concentration of ACID is equal to concentration of its conjugate BASE, because both are equal to HALF of the original (= unknown analyte) concentration to be titrated (half left = half formed).
The equivalence point reached when the pH reaches it maximum value?
No. The equivalence point is reached when the moles of titrant equals the moles of analyte.
What is titration error?
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)
Consider the titration of 30.0 ml of 0.030 M NH3 with 0.025 M HCl the equivalence point is reached when 36 ml of HCl titrant is added what is the pH at the equivalence point?
pH = 5.56 at 36.0 ml(equivalence point)
Standardising HCl using Na2CO3 titration. textbook says the solution at the equivalence point is slightly acidic. is it and why?
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.
If the equivalence point of a titration is 5 what range of pH should the indicator be?
The indicator should change color right at the equivalence point, so 5.
How do you determine ka from a titration curve?
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 .
What is the relation between pK and pH?
At half equivalence (half neutralisation) pH=pK.
How can the equivalence point in a titration be detected by using a pH meter?
In strong acid base titrations when pH meter shows the value 7 then it is equivalence point.
