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
The point at which the indicator changes color in a colorimetric titration.
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.
The equivalence or stoichiometric point of a titration of a strong acid versus a strong base is always equal to pH 7.
The defect which disturb the stoichiometric of the compound is called non-stoichiometric compounds.
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
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.
The equivalence or stoichiometric point of a titration of a strong acid versus a strong base is always equal to pH 7.
In can occur if the reaction in question in exothermic. After the stoichiometric point , there is no reactant left to react. No reaction occurs and no heat is evolved and as a result temperature drops.
The defect which disturb the stoichiometric of the compound is called non-stoichiometric compounds.
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
'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)
is fe3o4 non stoichiometric
Non stoichiometric compounds do not match to law of definite proportions.
In an acid-base titration for the reaction HCl + NaOH -> H2O + NaCl the equivalence point is when the hydrochloric acid and sodium hydroxide neutralise each other in equimolar proportions. When one mole of HCl is added to one mole of NaOH then equivalence point is reached.The 'end point' in a titration is when the indicator changes to the neutral colour (e.g. green) and this is usually an approximation of where the equivalence point is.As a result, we can deduce concentrations of unknown substances if we know the stoichiometric numbers of in the chemical reaction (i.e. 1HCl) and have a substance of known concentration react the unknown with.
Completely titrated means it reached the stoichiometric point (usually pH=7). Simply means neutralized.
Ideal Stoichiometric calculations give the theoretical yield of the products of the reaction