Titration Lab
Part A
1.	Obtain two 50 mL burets. Using a wax pencil, label one acid and the other base. 
2.	Pour about 5 mL of acid in the buret labeled “acid” rinse and drain. Repeat two more times, mount the buret as shown in figure 43.1; let each portion drain out of the buret before adding the next rinse.

3.	Pour 5 mL of base in the buret labeled “base” rinse and drain. Repeat two more times, mount the buret as shown in figure 43.1; let each portion drain out of the buret before adding the next rinse. 

9. If you overshoot the end point, that is, if you add too much base so the solution turns bright pink, simply add a few drops of acid from the acid buret to turn the solution colorless again. Approach the end point again, adding base drop by drop, until one drop causes the color change to pale pink. 

10. When you are sure that you have achieved the end point, record the final volume reading of each buret. 

11. Discard the solution in the Erlenmeyer flask as directed by your teacher, and rinse the flask well with distilled water. 

12. Calculate the concentration (molarity) of NaOH.

                            Formula for calculating the concentration using molarity:

			(Ma) (Va) = (Mb) (Vb)            M = molarity (mols/L)
							  V = volume (L)
							   a = acid
							   b = base

12. Repeat steps 2-11, until you have two titrations that agree within 1% on the concentration of NaOH. 

		                                                     Titration Lab
                                                              Part B