1. Arrhenius Acids & Bases ACIDS ACIDS –Monoprotic (HNO 3 ) –Diprotic (H 2 SO 4 ) –Triprotic (H 3 PO 4 ) –Yield Hydrogen ions (H+) in aqueous solution BASES BASES –Forms Hydroxide ions (OH-) in aqueous solution

2. BRONSTED – LOWERY ACIDS ACIDS ACIDS –Donates a proton/hydrogen ion BASES BASES –Accept proton/hydrogen ion

3. Acids Tart/sour taste Tart/sour taste Acid solutions are electrolytes (conduct electricity) Acid solutions are electrolytes (conduct electricity) Cause indicators to change color Cause indicators to change color High concentrations of hydrogen ions High concentrations of hydrogen ions [H+] [H+] pH 0 – 6.9 pH 0 – 6.9

4. Bases Bitter taste Bitter taste Slippery feel Slippery feel Aqueous solutions are electrolytes Aqueous solutions are electrolytes Cause an indicator to change color Cause an indicator to change color High hydroxide ion concentration High hydroxide ion concentration [OH-] [OH-] pH 7.1 – 14.0 pH 7.1 – 14.0

8. What ions do acids produce in greater concentrations in a solution? What ions do bases produce in greater concentrations in a solution?

9. CONCENTRATED VS. DILUTE

10. STRONG ACIDS HF HF HCl HCl HBr HBr HI HI HNO 3 HNO 3 H 2 SO 4 H 2 SO 4 “STRONG” indicates the degree of dissociation!!! NOT the degree of concentration!!!

12. WEAK ACIDS Acids that DO NOT 100% dissociate Acids that DO NOT 100% dissociate REMINDERS: REMINDERS: –Acids of VERY high concentrations (greater than 1M), will not 100% dissociate –ALL acids have SOME concentration of hydroxide ions….WHY??

14. STRONG BASES GROUP I HYDROXIDES GROUP I HYDROXIDES LiOH - lithium hydroxide LiOH - lithium hydroxide NaOH - sodium hydroxide NaOH - sodium hydroxidesodium hydroxidesodium hydroxide KOH - potassium hydroxide KOH - potassium hydroxidepotassium hydroxidepotassium hydroxide RbOH - rubidium hydroxide RbOH - rubidium hydroxide CsOH - cesium hydroxide CsOH - cesium hydroxide

15. STRONG BASES GROUP II HYDROXIDES GROUP II HYDROXIDES *Ca(OH) 2 - calcium hydroxide *Ca(OH) 2 - calcium hydroxide *Sr(OH) 2 - strontium hydroxide *Sr(OH) 2 - strontium hydroxide *Ba(OH) 2 - barium hydroxide *Ba(OH) 2 - barium hydroxide * These bases completely dissociate in solutions of 0.01 M or less. The other bases make solutions of 1.0 M and are 100% dissociated at that concentration. There are other strong bases than those listed, but they are not often encountered. * These bases completely dissociate in solutions of 0.01 M or less. The other bases make solutions of 1.0 M and are 100% dissociated at that concentration. There are other strong bases than those listed, but they are not often encountered.

16. WEAK BASES Bases that DO NOT 100% completely dissociate Bases that DO NOT 100% completely dissociate REMINDERS: REMINDERS: –Bases of VERY high concentrations (greater than 1M), will not 100% dissociate –ALL bases have SOME concentration of hydrogen ions….WHY??

17. Ionization Constant Example: Ammonia in water

18. Ionization Constant Example: Ionization of nitric acid

19. Ionization Constants: K a, K b, and K w K a K b K w http://www.saskschools.ca/curr_content/chem30_05/5_acids_bases/acids2_2.htm

20. Ionization Constants: K a, K b, and K w A large value of K a means there are many H + ions in solution - in other words, a strong acid A large value of K a means there are many H + ions in solution - in other words, a strong acid A large K b indicates many OH - ions - a strong base A large K b indicates many OH - ions - a strong base

21. Practice Set

22. Calculating pH/pOH [H + ] = 10 -pH [H + ] = 10 -pH [OH - ] = 10 -pOH [OH - ] = 10 -pOH [H + ] [OH - ] = 1 x 10 -14 [H + ] [OH - ] = 1 x 10 -14 pH = -log [H + ] pH = -log [H + ] pOH = -log [OH - ] pOH = -log [OH - ] pH + pOH = 14 pH + pOH = 14

23. Warm-Up A 25.00 mL sample of a 0.5250 M H 2 SO 4 solution is titrated with a NaOH solution using phenolphthalein as the indicator. It is found that 22.07 mL of the NaOH solution is needed to reach the endpoint of the titration. What is the molarity of the NaOH solution?