Themes > Science > Chemistry > Inorganic Chemistry > Acids and Bases > Acids and Bases Index > Strong acid-weak base titration


The titration of a weak base with a strong acid is very similar in form to that of the titration of a weak acid with a strong base. The reaction that occurs in the solution is

H+(aq) + B(aq) -> HB+(aq)
When doing this kind of titration, the solution starts out basic with a pH equal to that of the weak base solution. As acid is added, a buffer solution forms and the pH does not change rapidly until all of the weak base reacts with the acid. When it does, the equivalence point is in the acid range.

Working problems of this type is very similar to those of adding acid or base to a buffer. You need to first do the stoichiometry, then work an equilibrium calculation to figure out the final pH if the solution is still in the buffer range, otherwise figure out the pH from the excess acid.

Examples: You titrate 100 ml of 1.00 M sodium chlorate, NaClO with 1.00M HCl. What is the pH after you add 0 ml, 50 ml, 100 ml and 150 ml of acid? Kb for ClO- is 3.6*10-7.

Solutions


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