1. 7.00 Let the Titrations Begin
Dr. Fred Omega Garces
Analytical Chemistry 251
Miramar College, SDCCD

2. Titration
A technique of chemical analysis to determine the amount of a substance in a sample. Common titration include
A sample can be tested by titration. In a titration experiment, a known volume of a standard concentrated solution (the titrant) is used to analyze a sample (the analyte). One is usually an acid, the other a base. An indicator is added to the analyte to signal when the titration is complete. This is called the endpoint. When the moles of acid(H3O+) and moles of base (OH-) are equal in a titration experiment, the stoichiometric equivalent point is reached. This is called the equivalent point.
Indicator changes endpoint
moles titrant = moles analyte.
@ equivalent point.

3. ... remember
a titration problem is nothing more than a stoichiometry problem

4. Titration Common Terms: Titrant Analyte Indicator
A technique of chemical analysis to determine the amount substance in a sample. Common titration include:
Acid-Base
Oxidation-Reduction
Complex Formation
Precipitation Reaction
The requirement for these classic techniques are that the reactions are fast, have large Keq, and the analyte are consume and used up.
Common Terms:
Titrant Analyte Indicator
Endpoint Equivalent point Titration Error
Blank Titration Primary Standard Standardization
Direct Titration Back Titration

5. Titration Setup Setting up a titration experiment.
Titration is a common laboratory method of quantitative/chemical analysis which can be used to determine the concentration of a known reactant. Because volume measurements play a key role in titration, it is also known as volumetric analysis. A reagent, called the titrant, of known concentration (a standard solution) and volume is used to react with a measured quantity of reactant (Analyte). Using a calibrated burette to add the titrant, it is possible to determine the exact amount that has been consumed when the endpoint is reached. The endpoint is the point at which the titration is stopped. This is classically a point at which the number of moles of titrant is equal to the number of moles of analyte, or some multiple thereof (as in di- or tri- protic acids). In the classic strong acid-strong base titration the endpoint of a titration is when the pH of the reactant is just about equal to 7, and often when the solution permanently changes color due to an indicator. There are however many different types of titrations (see below).
Many methods can be used to indicate the endpoint of a reaction; titrations often use visual indicators (the reactant mixture changes color). In simple acid-base titrations a pH indicator may be used, such as phenolphthalein, which turns (and stays) pink when a certain pH (about 8.2) is reached or exceeded. Methyl orange can also be used, which is red in acids and yellow in alkalis.
Not every titration requires an indicator. In some cases, either the reactants or the products are strongly colored and can serve as the "indicator". For example, an oxidation-reduction titration using potassium permanganate (pink/purple) as the titrant does not require an indicator. When the titrant is reduced, it turns colorless. After the equivalence point, there is excess titrant present. The equivalence point is identified from the first faint pink color that persists in the solution being titrated.
Due to the logarithmic nature of the pH curve, the transitions are generally extremely sharp, and thus a single drop of titrant just before the endpoint can change the pH significantly — leading to an immediate colour change in the indicator. That said, there is a slight difference between the change in indicator color and the actual equivalence point of the titration. This error is referred to as an indicator error, and it is indeterminate. (wikipedia.org)

6. Acid-Base Calculations
Indicator changes endpoint.
Indicator is chosen so that endpoint occurs at equivalent pt.
The following is true at the equivalence point.
moles H3O+ = moles OH-
Macid • Vacid = Mbase • Vbase For monoprotic A & B
Macid • Vacid ≠ Mbase • Vbase For polyprotic A & B
but Nacid•Vacid = Nbase•Vbase for monoprotic and polyprotic A & B
eq H3O+ • L H3O+ = eq OH- • L OH-
L Soln L Soln
For Acid base calculation at Equivalence pt:
Sometimes: Macid • Vacid = Mbase •Vbase
but always: Nacid•Vacid = Nbase•Vbase

7. Acid-Base Titration of Mixture
A mixture containing K2CO3 (FW ) and KHCO3 (FW ) requires 15.00mL of 1.000M HCl. Find the mass of each component.
Stoichiometry Problem:
K2CO HCl  2 KCl + H2O + CO2
KHCO HCl  KCl + H2O + CO2

8. The Precipitation Titration
In a precipitation titration, the reaction is monitored by weighing out the precipitate and knowing the stoichiometric ratio.
A precipitation titration curve is monitored like an acid-base titration curve. MA D M+ + A : M+ is the titrant, Ksp is used for rxn.
pX = - log [X], where [X] is the concentration of X. X = M+
Before Equiv Pt: [M+] = Ksp / [A-],
A- is in excess before equivalent pt and determines the pX of the solution.
The excess A- concentration is corrected for by dilution factor.
At the Equiv Pt: Ksp = [M+] [A-] = s2 , pM = -log s
Past Eqivalent Pt. All M+ added has precipitated. There is now excess M+ which determines the pM. Remember the M+ must be corrected for by dilution factor.

9. The Precipitation Titration Curve
Shape of titration curve
Before Equiv Pt
At Equiv Pt
Past Equiv Pt.

10. Titration of a Mixture
In a mixture, two ions are titrated and less soluble precipitates first. Consider the addition of AgNO3 to KI and KCl, Ksp (AgI) << Ksp (AgCl)

11. Titration with a Spreadsheet
Titration of I- with Ag+ via Excel

12. End Point Detection: Indicator
Some common acid-base indicators. The color changes occur over a range of pH values. Notice that a few indicators have two color changes over two different pH ranges.
Mechanism for phenolphthalein indicator. At Low pH phenolphthalein is colorless and has a structure in which there is a five membered ring. In the presence of excess acid the five membered ring is broken and the resulting change in conformation gives rise to a compound which is pink.

13. End-Point Detection
Volhard Titration: The technique is to measure Cl-. Cl- is precipitated by addition of Ag+ to form AgCl. AgCl is precipitated out and worked up and the Ag+ is titrated with KSCN. With the formation of FeSCN2+ indicating the end point of the titration.
Fajans Titration: Uses adsorption indicator. When Ag+ is added to Cl-, AgCl forms and its surface attracts (adsorbs) Cl- ions. After equivalence point, the excess goes from Cl- to Ag+. The abrupt change from negative to positive occurs at the equivalence point. An adsorption indicator such as will change color when the charge is reverse.
Ag+ (aq) + SCN- (aq) ® AgSCN (s).
Fe3+ (aq) + SCN- (aq) ® FeSCN2+ (aq).