1. Chapter #16 Acid-Base Titration and pH

2. Chapter 16.1 In the self-ionization of water, two water molecules produce a hydronium ion and a hydroxide ion by transfer of a proton. K w = H 3 O + OH - K w = 1.0 X 10 -14 M 2

3. The pH of a solution is defined as the negative of the common logarithm of the hydronium ion concentration. The pH scale 0-14. 7 is neutral…pH 7 base pH= -log ( H 3 O + )

4. Chapter 16.2 Acid-base indicators are compounds whose colors are sensitive to pH. pH range over which an indicator changes color is called its transition interval. pH meter determines the pH of a solution by measuring the voltage between the two electrodes that are placed in the solution.

5. Titration is the controlled addition and measurement of the amount of a solution of known concentration required to react completely with a measured amount of a solution of unknown concentrations. Equivalence point is the point at which the two solutions used in a titration are present in chemically equivalent amounts. End point is the point in a titration at which an indicator changes color.

7. Titration Problems 1.Balance equation 2.Use the known solution to figure out the number of moles (M=mol/L) 3.Use the mole to mole ratio to figure out the moles of the unknown. 4.Determine the Molarity of the unknown using the given volume

8. “Flask”. May 7, 2007. http://www.chem.ualberta.ca/~iip/chem211 irc/TotalSalt(start).jpg http://www.chem.ualberta.ca/~iip/chem211 irc/TotalSalt(start).jpg “Let’s Titrate”. May 7, 2007. http://genchem.rutgers.edu/aanimate.gif http://genchem.rutgers.edu/aanimate.gif “Titration curve”. May 7, 2007. http://www.cofc.edu/~kinard/Applets/Weak AcidTitration.gif http://www.cofc.edu/~kinard/Applets/Weak AcidTitration.gif