1. Acid - Base Titrations
They are an application of acid-base neutralization reactions that require the use of an indicator. 1

2. NaOH (aq) + HCl (aq)  NaCl (aq) + H2O (l)
Stoichiometry
The stoichiometry of an acid-base neutralization reaction is the same as that of any other reaction that occurs in solution (they are double displacement reactions, after all).
For example, in the reaction of sodium hydroxide and hydrogen chloride, 1 mol of NaOH neutralizes 1 mol of HCl:
NaOH (aq) + HCl (aq)  NaCl (aq) + H2O (l)
Stoichiometry provides the basis for a procedure called titration, which is used to determine the concentrations of acidic and basic solutions.

4. Titration
Titration is a method for determining the concentration of a solution by reacting a known volume of that solution with a solution of known concentration.
If you wish to find the concentration of an acid solution, you would titrate the acid solution with a solution of a base of known concentration.
You could also titrate a base of unknown concentration with an acid of known concentration.

5. Objectives of Titration Practicle
One objective of this practicle is to observe differences in shapes of titration curves when various strengths of acids and bases are combined.
You will also learn about the function and selection of appropriate acid-base indicators in this experiment.
In order to do several other experiments in this lab manual, you need to be able to interpret the shape of a titration curve.

6. Titration Equipment
In the titration of an acid by a base, the Vernier pH sensor placed in measures the pH of the acid solution in the beaker as a solution (analyte) of a base with a known concentration(titrant) is added from the burette.

7. Titration Procedure
A measured volume of an acidic or basic solution of unknown concentration is placed in a beaker. The electrodes of a pH meter are immersed in this solution, and the initial pH of the solution is read and recorded.
A burette is filled with the titrating solution of known concentration. This is called the standard solution, or titrant.
Measured volumes of the standard solution are added slowly and mixed into the solution in the beaker. The pH is read and recorded after each addition. This process continues until the reaction reaches the equivalence point, which is the point at which moles of H+ ion from the acid equal moles of OH- ion from the base.

8. Equivalence Point and End Point

9. Indicators and Titration Curve9

10. Strong Acid – Strong Base Titration

13. High resolution touch screen
12.8 cm, 800 x 480 pixel resolution
Designed for both stylus and touch
Wide viewing angle for lab groups
Full sensor support
Compatible with all Vernier sensors
Faster analysis
Quick response to touch, curve fits and modelling

14. Built-in sensors
GPS
3-axis accelerometer
Ambient temperature
Light
Microphone
Fast data collection
100,000 samples per second
Rechargeable batteries
High-capacity, lithium-ion rechargeable battery
Wireless connectivity
Wi-Fi
Bluetooth

15. References http://inds.co.uk/education/labquest2.htm
Performing a Titration - YouTube
Acid-Base Titration (LabQuest)