1. ACIDSBASES ACIDS, BASES, & SALTS

2. Electrolyte Substance that dissolves in H 2 O to produce a solution that conducts an electric current Acids, bases, & salts are electrolytes – form ions in H 2 O NaCl(s)  Na +1 (aq) + Cl -1 (aq)

3. Acids Properties of Acids 1.Sour taste 2.Electrolytes: - aqueous solns conduct an electric current 3.React with bases to form water and a salt (Neutralization Reaction) 4.React with most metals to produce H 2 (g) dd 5.Acids turn litmus red

4. Formulas of Acids HFormat: HX where X = nonmetal (F, Cl, Br, I) or or X = negative polyatomic ion HSome acids have 2 or 3 H’s HHH –Ex: HF, H 2 S, H 3 PO 4

5. Which metals react with acids? See Table J All metals above H 2 react with acids Cu, Ag, and AunotCu, Ag, and Au do not react with acids

6. 2HCl + Mg  MgCl 2 + H 2 Mg above H 2 so reaction proceeds Single replacement reaction

7. Bases Properties of Bases 1.Bitter taste 2.Slippery or soapy feeling 3.Electrolytes 4.React with acids to produce water and a salt 5.Bb 5.Bases turn litmus blue

8. Formulas of Bases OHFormat: MOH where M is a metal OHOHEx: NaOH, Ca(OH) 2 Exception: NH 3 and NH 4 +1 NOTCH 3 OH is NOT a base. WHY?

9. Identify the Electrolytes NaClNaCl C 2 H 5 OHC 2 H 5 OH H 2 SO 4H 2 SO 4 NaOHNaOH C 6 H 12 O 6C 6 H 12 O 6 CaI 2CaI 2 HFHF Mg(OH) 2Mg(OH) 2 C 3 H 7 OHC 3 H 7 OH CCl 4CCl 4 HNO 3HNO 3 C 5 H 12C 5 H 12 K 3 PO 4K 3 PO 4 CH 3 OCH 3CH 3 OCH 3 LiOHLiOH HIHI (NH 4 ) 2 SO 4(NH 4 ) 2 SO 4 C 12 H 22 O 11C 12 H 22 O 11 Yes - S Yes - B NO NO NO NO NO NO NO Yes - A Yes - B Yes - A Yes - B Yes - A Yes - B Yes - A

10. Acid, Base, or Neutral? all H 2 O contains some H +1 and some OH -1 ions –pure H 2 O: concentrations very low Neutral solution: [H +1 ] = [OH -1 ] Acidic solution: H +1 > OH -1 Basic solution: OH -1 > H +1

11. Water & self-ionization H 2 O(l) + H 2 O(l)  H 3 O +1 (aq) + OH -1 (aq) H 3 O +1 H 3 O +1 = hydronium ion OH -1 = OH -1 = hydroxide ion H 2 O(l)  H +1 (aq) + OH -1 (aq) H +1 and H 3 O +1 used interchangeably H +1 H +1 called proton or hydrogen ion

12. Self-ionization of water H 2 O + H 2 O → H 3 O +1 + OH -1

13. Arrhenius Acid H +1Substance that contains hydrogen & ionizes to produce H +1 ions in aqueous solution H +1 HCl(g)  H +1 (aq) + Cl -1 (aq) acid H +1 HNO 3  H +1 (aq) + NO 3 -1 (aq) acid

14. Arrhenius Base OH -1substance that contains hydroxide group & ionizes to produce OH -1 ions in aqueous solution OH -1 NaOH(s)  Na +1 (aq) + OH -1 (aq) base

15. Arrhenius Model has limitations Don’t always use H 2 O as solvent –Arrhenius model only applies when H 2 O is solvent Doesn’t explain all cases: –NH 3 doesn’t contain OH -1 but it produces OH -1

16. Alternate Theory: Bronsted-Lowry Acid = a proton donorAcid = a proton donor All Arrhenius acids = Bronsted-Lowry Acids H +1 HX(g) + H 2 O(l)  H 3 O +1 + X -1 acid H +1 H 3 O +1 hydronium ion) H +1 forms molecule-ion bond with water molecule  H 3 O +1 (hydronium ion)

17. Bronsted-Lowry Acids H +1 HCl + H 2 O  H 3 O +1 + Cl -1 HNO 3 + H 2 O  H 3 O +1 + NO 3 -1 H 2 SO 4 + H 2 O  H 3 O +1 + HSO 4 -1 HSO 4 -1 + H 2 O  H 3 O +1 + SO 4 -2 H +1

18. Bronsted-Lowry Base Base = proton acceptorBase = proton acceptor OH -1 is a base H +1 + OH -1  H 2 O Not restricted to aqueous solution NH 3 + H 2 O  NH 4 +1 + OH -1 NH 3 is a base! H +1

19. Bronsted-Lowry Acids & Bases

20. Amphoteric Substance that acts as both acid & base H 2 O is amphoteric HX(g) + H 2 O(l)  H 3 O +1 + X -1 (base) H 2 O NH 3 + H 2 O  NH 4 +1 + OH -1 (acid) H +1

21. Water is amphoteric!

22. Naming Acids & Bases

23. Naming Binary Acids Hydro + stem of nonmetal + ic HF = ? HCl = ? H 2 S = ? Hydrofluoric acid Hydrochloric acid Hydrosulfic acid

24. Naming Ternary Acids polyatomicName derived from polyatomic anion (see Table E) iteousReplace –ite with –ous, add acid HNO 2 is nitrous acid ateic, addReplace –ate with –ic, add acid HNO 3 is nitric acid

25. Ternary Acids polyatomics with S and P, make stem long again –H 3 PO 4 = phosphoric acid, not phosphic acid –H 2 SO 4 = sulfuric acid, not sulfic acid –H 2 SO 3 = sulfurous acid, not sulfous acid SEE TABLE K

26. Naming Bases Name the metal + hydroxide NaOH = ? Ca(OH) 2 = ? Mg(OH) 2 = ? Sodium hydroxide Calcium hydroxide Magnesium hydroxide