Acid-base titrations (neutralisation titrations)

The course of such a titration curve depends strongly on the acids and bases involved - do my php assignment . The values determined during the titration are used as the basis for the calculation.

Example:

If, for example, the acidity c(H2SO4) of a wastewater originating from sulphuric acid production is to be tested in the laboratory, one generally titrates with a sodium hydroxide solution of known concentration - domyhomework club. In a routine titration, 5 ml of sodium hydroxide solution C(NaOH) = 0.1 mol⋅l-1 was consumed for the neutralisation of 20 ml of sampled waste water containing sulphuric acid.

The indicator bromothymol blue can be used. (The pH value of the salt solution formed during neutralisation should be in the middle of the envelope range of the indicator).

To evaluate titrations, consider the neutralisation equation of the titration:

2 NaOH (aq) + H2SO4(aq) ? Na2SO4(aq) + 2 H2O(l)

Assuming a complete reaction of the two reactants, the ratio of the amounts of substances is as follows

n(H2SO4) : n(NaOH) = 1 : 2from this follows: n(H2SO4) = n(NaOH)2

The quantities of substances result from the product of consumed volume and concentration n = c ⋅ V.

c(H2SO4)⋅V(H2SO4) = c(NaOH)⋅V(NaOH)2 c(H2SO4) = c(NaOH)⋅V(NaOH)2⋅V(H2SO4) c(H2SO4) = 0.1 mol⋅l-1⋅0.005 l2⋅0.020 l c(H2SO4) = 0.0125 mol⋅l-1

According to this principle, the concentration of any acid soluble in water can be calculated based on the corresponding neutralisation equation.

The equivalence point in acid-base titrations can be determined not only with the help of colour indicators. The pH meter can also be used to measure the change in the pH value of the analysis solution and calculate the equivalence point from the titration curve - solve my chemistry problem . For this purpose, a special electrode is used whose voltage or electrode potential depends only on the pH value of the solution. This is why we also speak of potentiometric titration.

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