The titration shown here with an acidic titrant, such as HCl, is the reverse of the original picture in titration, in which apparently a basic titrant is used with phenolphthalein.
32.
Since this is a different species with different diffusion characteristics ( and different half-reaction ), the slope of current versus added titrant will have a different slope after the equivalence point.
33.
In this instance, it has been found advantageous to incorporate the potassium iodide reagent with the thiosulfate titrant in such proportions that iodine is released into solution just prior to its reduction by thiosulfate.
34.
When this titration is done using nickel acetate, two moles of isohumulones combines with one mole of nickel acetate, and each milliliter of titrant contains 1 / 500 of a millimole of nickel.
35.
Because of this, a small change in titrant volume near the equivalence point results in a large pH change and many indicators would be appropriate ( for instance litmus, phenolphthalein or bromothymol blue ).
36.
In thermometric titrations, a constant addition rate of titrant equates to a constant amount of heat being given out or consumed, and hence a more or less constant temperature change up to the endpoint.
37.
The equivalence point on the graph is where all of the starting solution ( usually an acid ) has been neutralized by the titrant ( usually a NaOH solution has been titrated into the oxalic acid solution.
38.
Due to the quantitative nature of this reaction, as well as because Na 2 S 2 O 3 ?H 2 O has an excellent shelf-life, it is used as a titrant in iodometry.
39.
This number is determined by titration of the sake with a mixture of sodium hydroxide solution and formaldehyde, and is equal to the milliliters of titrant required to neutralize the amino acids in 10 mL of sake.
40.
If one reagent is a weak acid or base and the other is a strong acid or base, the titration curve is irregular and the pH shifts less with small additions of titrant near the equivalence point.
