Want this question answered?
No. The equivalence point is reached when the moles of titrant equals the moles of analyte.
the equivalence point has been reached
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+H2O1mol 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).
The indicator should change color right at the equivalence point, so 5.
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.
No. The equivalence point is reached when the moles of titrant equals the moles of analyte.
pH = 5.56 at 36.0 ml(equivalence point)
Yes
FeCI2 is a combination of iron and hydrochloride. This solution starts out as a yellowish green color. When the equivalence point is reach the solution turns to an orange brown color.
the equivalence point has been reached
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+H2O1mol 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).
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
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.
Neutralization occurs at the "equivalence point," where the moles of your acid and your base are the same. A chemical indicator tells you when this point is reached, and changes color appropriately.
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
Most solutions used in titrations are colorless, therefore you cannot really estimate the equivalence point (the volume of added titrant that causes a stoechiometric reaction). However, slight variations in other factors such as acidity (pH) can be detected by means of an indicator, which will change color accordingly. This will notify you when you have reached the 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)