1. Mullis Acids, Bases and Salts Acids give up hydrogen ions (H + ) in a water solution. Bases give up hydroxide ions (OH - ) in a water solution.

2. Mullis Properties of Bases Bitter taste Feel slippery if you touch them pH > 7.0 Strong bases: –Sodium hydroxide (NaOH) –Potassium hydroxide (KOH) Weak bases: –Sodium bicarbonate (NaHCO 3 )

3. Mullis Properties of Acids Sour taste pH < 7.0 React with metals to form H 2 gas Strong acids: –Sulfuric acid (H 2 SO 4 ) –Hydrochloric acid (HCl) Weak acids: –Acetic acid (vinegar – CH 3 COOH)) –Citric acid (in fruits) –Ascorbic acid (Vitamin C)

4. Mullis Naming Acids Binary Acid = 2 elements (HCl) –Begin with hydro-. –Use name of 2 nd element and end with –ic. –HCl is hydrochloric acid. Oxyacid = H + O + 3 rd element (H 2 SO 4 ) –Usually incorporates the polyatomic ion name into the acid name. –Written with H first, then the polyatomic ion. –H 2 SO 4 is sulfuric acid.

5. Mullis Acid Strength Strong acids ionize completely in water. –Many H 3 O + ions –Strong electrolyte Weak acids do not ionize completely in water. –Some H 3 O + ions –Weak electrolyte –The ionized H 3 O + ions are being bonded back to the negative species (reverse reaction) at the same time some acid molecules are being ionized to form H 3 O + ions. Strong and weak bases are similar, except ion involved is OH - instead of H 3 O +.

6. Mullis Classifying strength of electrolytes from solubility (general rules for compounds) Strong electrolyte –Water soluble AND ionic –Strong acid, water soluble and not ionic –Strong base, water soluble and not ionic Weak electrolyte –Weak acid or base, water soluble and not ionic Nonelectrolyte –None of the above

7. Mullis Cl The Hydronium Ion Ionization is the creation of ions from a molecular compound. –If the force of attraction between solvent molecules and parts of the solute are stronger than the covalent bonds of the solute, the solute breaks into ions. –In water, HYDRATION produces heat, which provides energy to break more covalent bonds. H + attracts other molecules or ions In water, H + becomes a proton bonded to the oxygen of a water molecule. The hydronium ion is H 3 O +. Cl O O++ - + H HH H H H

8. Mullis Acid-Base Systems TypeAcidBaseExamples Arrheniu s H + or H 3 O + produce r OH - produc er HNO 3 + H 2 O H 3 O + + NO 3 - NH 3 + H 2 O NH 4 + + OH - Brønsted -Lowry proton (H + ) donor proton (H + ) accepto r HCl + NH 3 NH 4 + + Cl - Lewiselectron pair accepto r electro n pair donor BF 3 + F - BF 4 - BF 3 is Lewis acid, F - is Lewis base

9. Mullis Brønsted-Lowry Acids Brønsted-Lowry acids donate a proton. A monoprotic acid donates one proton per molecule, such as HCl and HClO 4. A polyprotic acid donates more than one proton per molecule, such as H 2 SO 4 and H 3 PO 4. –H 2 SO 4 is a diprotic acid. –H 3 PO 4 is a triprotic acid.

10. Mullis Conjugate acids and bases The species remaining after a Brønsted-Lowry acid gives up its proton is the conjugate base of that acid: Take off one H from the acid. The species remaining after a Brønsted-Lowry base accepts its proton is the conjugate acid of that base: Take off one H. Add an H to the base. CH 3 COOH(aq) + H 2 O(l) H 3 O + (aq) + CH 3 COO - (aq) acid baseconjugate conjugate (proton donor) acid base

11. Mullis Examples of conjugate acids and bases HCO 3 - (aq) + H 2 O(l) H 2 CO 3 (aq) + OH - (aq) base acidconjugate conjugate (proton acid base acceptor) HF(aq) + H 2 O(l) H 3 O + (aq) + F - (aq) acid baseconjugate conjugate (proton acid base donor)

12. Mullis Salts An acid and base combined together react to neutralize each other. Neutralization is a process which produces produces that are not acids or bases. H+ and OH- make water. The remaining reactants combine to make a salt. A salt is an ionic compound made of a metal and a nonmetal. Soap and detergent are organic salts.

13. Mullis Neutralization HCl + NaOH NaCl + H 2 O HNO 3 + KOHKNO 3 + H 2 O H + + OH - H 2 O ACID + BASE YIELDS SALT + WATER salt acid basewater

14. Mullis Neutralization The reaction between an acid and a base which produces a salt and water. Recall: A salt is an ionic compound: metal + nonmetal which is likely to dissociate in water. Ex: You take a dose of the antacid magnesium hydroxide, Mg(OH) 2, to relieve excess stomach acid, HCl. Equations for this neutralization: 2HCl(aq) + Mg(OH) 2 (s)  MgCl 2 (aq) + 2H 2 O(l) 2H + (aq) + Mg(OH) 2 (s)  Mg 2+ (aq) + 2H 2 O(l)

15. Mullis Ionic Equations for Acid-Base Reactions H + (aq) + OH - (aq)  H 2 O (l) Strong acids ionize completely. HCl  H + + Cl - Weak acids do not ionize completely. HF H + + F - Water and ammonia are a weak acid and a weak base, respectively. NH 3 (aq) + H 2 O (l) NH 4 + (aq) + OH - (aq)

16. Mullis Measuring Strength of Acids and Bases pH is a measurement which indicates acidic or basic strength, measuring the concentration of H+ ions. More H+ ions = lower pH = acid. An indicator changes color depending on pH of a solution. pH paper is treated with indicators to change color when dipped in a solution. 1: acid 7: neutral14: base

17. Mullis pH and acidity pH is related to the concept of concentration of hydronium ions found in water. Water and all its solutions contain hydronium ions and hydroxide ions. Acidic solutions: More H 3 O + ions. Basic solutions: Fewer H 3 O + ions / more OH - ions. If pH = 2: H 3 O + ion concentration = 0.01 M OH - ion concentration = 0.000000000001 M If pH = 12: H 3 O + ion concentration = 0.000000000001 M OH - ion concentration = 0.01 M

18. Mullis The pH scale pH stands for “power of hydronium ion.” pH = -log [H 3 O + ] pH value is the exponent on the power of 10 with its sign changed.

19. Mullis pH examples Example 1: –0.001 mol H 3 O + = 1 x 10 -3 mol H 3 O + –Concentration is 0.001M –pH = -log [H 3 O + ] = -log (1x 10 -3 ) = -(-3.0) = 3.0 –pH is 3.0 - This is an acid. Example 2: –0.000 000 01 mol H 3 O + = 1 x 10 -8 mol H 3 O + –Concentration is 0.000 000 01M –pH = -log [H 3 O + ] = -log (1x 10 -8 ) = -(-8.0) = 8.0 –pH is 8.0 - This is a base.

20. Mullis pOH pOH is the negative of the logarithm of the hydroxide ion (OH - ) concentration. pOH = -log [OH - ] pH + pOH = 14.0 at 25 deg. C

21. Mullis Buffers Why is the pH of some lakes unaffected by acid rain even when they are downwind of big polluters? The lakes are surrounded by soils which neutralize the acidic precipitation. 1.One way to neutralize acid is to add a base. Limestone (CaCO 3 ) is a weak base. 2.Another way to neutralize either an acid or a base is to add a buffer. A buffer is a substance or combination of substances capable of neutralizing limited quantities of either acids or bases.

22. Mullis Buffers Calcium carbonate around a lake contaminated with acid rain would react this way: CaCO 3 + H 3 O + Ca 2+ + HCO 3 - + H 2 O The polyatomic ion HCO 3 - acts as a buffer: HCO 3 - + H 3 O + 2H 2 O + CO 2 HCO 3 - + OH - H 2 O + CO 3 2- Another buffer is the hydrogen phosphate ion. Possible sources of this ion are Na 2 HPO 4 and NaH 2 PO 4. H 3 O + + H 2 PO 4 2- H 2 PO 4 - + H 2 O