Question

If I titrate an acid with 255mL of 3.4 M NaOH (base) and reach the equivalence point, how many moles of H+ ions were in the acid?

Answer 1

Answer:

Molar Concentration = $\frac{Moles of Solute}{Litres of Solution}$

                                     = $\frac{3.4}{0.255}$

                                    =  13.33

No. of H+ ions present = 13.33

pH value = - log[13.33]

               =  -1.12

Explanation:

The equivalence point, or stoichiometric point, of a substance response is the point at which synthetically identical amounts of reactants have been blended. As such, the moles of corrosive are equal to the moles of base, as per the condition (this doesn't really infer a 1:1 molar proportion of acid:base, simply that the proportion is equivalent to in the condition). It tends to be found by methods for a marker, for instance phenolphthalein or methyl orange. The endpoint (identified with, however not equivalent to the equivalence point) alludes to the point at which the marker changes shading in a colorimetric titration.