1. Operational (properties) Any group 1 metal bound to OH - NaOH, KOH, LiOH Strong Sour Electrolyte – makes ions in solutions Perform single replacement Rxns: Table J Any metal above H 2 will react with an acid to produce H 2(g) Where found –Table K Bitter Electrolyte – makes ions in solutions Referred to as caustic alkaline “Feel slippery” Where found –Table L List: HI, HBr, HCl, H 2 SO 4, HNO 3 Table K– top 3 are strong

2. “B” INDICATORS: PINKColorless Litmus Phenolphthalein “D” Acids turn litmus RED ACID Bases turn litmus BLUE BASE BLUE pH Note: H + = H 3 O + pH < 7 (below 7) [ H 3 O + ] > [OH - ] H 3 O + i s called Hydronium ion Comes from H + + H 2 O H 3 O + pH > 7 (above 7) [ H 3 O + ] < [OH - ] OH - is called hyroxide ion Neutral pH=7 is when [H 3 O + ] = [OH - ]

3. Neutralization It’s when pH =7 Pure water Net ionic result : H + + OH - H 2 O It’s also double replacement reaction Acid + Base Salt + water H x __ + M etal OH Metal with nonmetal + water HI + KOH KI + H 2 O Ionic Arrhenius PRODUCE H + H + : is the only positive ion in solution Ex. HCl H + + Cl - Produces OH - OH - : is the only negative ion in solution Ex. NaOH Na + + OH -

4. Bronsted- Lowry PROTON DONOR (gives an H ) H + : is “given” to an acceptor moves from acid to base Ex. CH 3 COOH can give up that Might see it written HC 2 H 3 O 2 PROTON ACCEPTOR H + : is accepted by the base and makes a coordinate covalent bond Ex. NH 3 + H + NH 4 + The NH 3 is the acceptor Appear on opposite sides of the equation (opposite sides of arrow) Differ only in an H If it’s an acid on the left side becomes the base on the right side of arrow If it’s a base on the left side becomes the acid on the right NH 3 + HSO 4 - NH 4 + + SO 4 2- B B A A Acid/base pairs

5. Binary 2 elements In compound H x ___ y Ex. H 2 S, HCl Tertiary 3 or more elements In compound H x ___ y ___ z TABLE E Always start with “hydro” Hydro____________ic acid Route name of second element Ex. HCl - hydrochloric acid H 2 S – hydrosulfuric acid Going backwards – hydrobromic acid - HBr **NO HYDRO Look at anion ending in table E Ends in –ate, change ending to -ic acid Ex. HClO 3 —chlorate---becomes chloric acid Ends in –ite, change ending to –ous acid Ex. HNO2 – nitrite----becomes nitrous acid Writing formula-phosphoric acid –PO 4 3- : H 3 PO 4

6. Any Metal + OH - contains the OH - ion organic Not CH 3 OH Make sure There is a metal **Name metal then add hydroxide Ex. NaOH—sodium hydroxide Ex. Ca(OH) 2 —calcium hydroxide Writing formula -- Magnesium Hydroxide (criss-cross) Mg 2+ OH - :: Mg(OH) 2

7. K w – Is the equilibrium constant for water H 2 O (l) + H 2 O (l) H 3 O + (aq) + OH - (aq) K w = [H 3 O + ][OH - ] = 1.0 x 10 -14 @ 25ºC pH + pOH = 14 What is the hydroxide ion concentration if th hydronium ion concentration is 1.0 x 10 -5 M? 1.0 x 10 -5 M[OH - ] = 1.0 x 10 -14 [OH - ] = 1.0 x 10 -14 1.0 x 10 -5 = 1.0 x 10 -9 Determining pH – always use concentration of H + ion pH= -log[H + ] Another way to look at it [H+] = 1.0 x 10 -pH The numerical value of exponent = value of pH pH is a log scale. Each number change is a 10 fold change (factor of 10) As you go H + decrease, OH - increase, pH increase As you go H + increase, OH - decrease, pH decreases 1 14 Acid Base 7 Neutral H+H+ OH - If the pH changes from 4 to 8, what is the change in H + concentration 4 to 5 to 6 to 7 to 8 10 10x10x10x10=10,000 fold change DECREASE in H +

8. What is the pH of 1.0 x 10 -3 M solution of HCl? HCl – is an acid so = [H + ] [H + ] = 1.0 x 10 -3 pH = 3 What is the pH of 0.00001 M solution of HCl? 0.00001 M = 1 x 10 -5 =[H + ] pH = 5 What is the pH of 1.0 x 10 -3 M solution of NaOH? NaOH – is a base so = [OH - ] Concentration of [OH - ][H + ]=1x10 -14 [H+] = 1 x 10 -11 pH = 11 What is the pH of 0.001 M solution of NaOH? NaOH – is a base so = [OH - ] Concentration of [OH - ][H + ]=1x10 -14 [H+] = 1 x 10 -11 pH = 11 NaOH = 1x10 -3

9. Buret Solution of known concentration With a known volume, V A known M A Solution Of base. We find M B How much base used will Equal how many moles Acid is there. VBVB Phenol (indicator) TITRATION Use of a known solution to calculate the concentration of an unknown solution Place the indicator in the unknown solution When it changes color you’ve reached the equivalence pnt - you have neutralized it! Moles H + = moles OH - USE TITRATION FORMULA M A V A = M B V B If 50 mL of 0.5M HCl is used to completely neutralize 25 mL of KOH, what is the molarity of the base? (0.5M)(50mL) = M B (25mL) M A V A = M B V B 1.0 M = M B

10. OTHER Indicators – TABLE M Below the 1 st # - 1 st color listed Above the 2 nd # - 2 nd color listed Between the #’s on the chart – will be a blend of the colors Ex. A solutions pH = 5.8 then In methyl orange – color would be yellow In bromthymol blue – color would be yellow In litmus – color would be a reddish-purple (in middle)