1.  Topic 10 Correlates to Topic 10 in review book, pages 174-188

2.  Acids = substances that react with a base; often has a low pH  May be strong or weak  Actual definition depends upon the type of acid/base  Bases = substances reacting with an acid; often has a high pH  May be strong or weak  3 major types of acids and bases here

3.  Acids: o Taste sour o Conduct current in solution o React with bases to form water and salt o React with some metals to make H2(g) o Low pH  Bases: o Taste bitter o Slippery/soapy feeling o Conduct current in solution o React with acids to form salt water o Have low pOH or high pH

4.  1. Arrhenius  2. Bronsted-Lowry

5.  Acid = substances that release hydrogen ions in aqueous solutions  proton donors  Ex.] HCl  H + + Cl -  Base = substances that release hydroxide ions in aqueous solutions  Hydroxide donors  Ex.] NaOH  Na + = OH -

6.  Acid = any substance that can donate hydrogen ions in solution o Proton donors Ex.] HCl  H + + Cl -  Base = any substance that can accept hydrogen ions in solution  Proton acceptors Ex.] NH3 + H +  NH4 +

7.  Acid = any species that can accept an electron pair from another species in solution  Ex.] H + + NH3   Base = any species that can donate an electron pair to another species in solution NH4 +

8.  STRONG acids/bases will completely dissociate [ionize] in solution  Ex.] HCl, HNO 3, H 2 SO 4, NaOH, KOH, etc.  WEAK acids/bases produce very few ions per molecule in solution  Ex.] vinegar, H 3 PO 4, formic acid, citric acid, etc.

9.  Acid/Base Conjugates = species that are formed in solution as a result of the dissociation of an acid or base  Ex.] HCl + NaOH  Na + + Cl - + HOH o Cl - is the conjugate base o Na + is the conjugate acid

10.  Titration = method used to determine the pH of an unknown solution  Process to find the concentration of an unknown acid/base by neutralizing it with a base/acid of known concentration  An indicator signals the equivalence point and tells that the neutralization is complete

11. Uses burets, a standard solution of known pH, an indicator, and a fixed volume of a solution with an unknown pH Titration Formula: M a V a = M b V b  http://www.youtube.com/watch?v=u9nOIZDdvRw http://www.youtube.com/watch?v=u9nOIZDdvRw

12. Acid + Base = Salt + water Acids and bases neutralize each other H + + OH -  H 2 O

13.  pH = the scale, 0-14, that defines the acidity or basicity of a solution  Based on the concentration of hydrogen ions 0-6 = acid 7= neutral 8-14 = base

14.  pOH = the measure of the concentration of OH- ions in solution  Opposite of pH  Scale 0-14 0-6 = strong base 7= neutral 8-14 = acidic

18. pH + pOH = 14 always! pH = -log[H + ] pOH = -log[OH - ]

19. Ex. 1] What is the pH of a solution containing 9.15 x 10 -6 M H + ? Ex. 2] What is the pH of a solution containing [OH - ] = 8.11 x 10 -5 M in 350.mL of solution?

20.  Indicators = compounds that change color when the pH changes o Color changes indicate the pH of the solution! o Use several indicators to pinpoint the final pH!

21.  Find the pH using the indicator and its color in the solution… Tutorial on indicators: http://www.kentchemis try.com/links/AcidsB ases/Indicators.htm