2. Acids –Sour Taste –Change the color of an acid-base indicator –React with metals to form H 2 gas –React with bases to produce salts and water –Conduct electric current. Bases –Taste Bitter –Change the color of an acid-base indicator –Feel Slippery –React with acids to produce salts and water –Conduct electric current

3. Acids –Citric Acid (fruits) –Acetic Acid (vinegar) –Sulfuric Acid –Nitric Acid –Phosphoric Acid –Hydrochloric Acid Bases –Ammonia –Milk –General Cleaning (NaOH) –Soaps

4. Binary Acids- acid that contains only two different elements. Hydrogen and one more –Hydro____ic acid HCl= hydrochloric acid HBr= hydrobromic acid

5. Oxyacid-an acid that is a compound of hydrogen, oxygen, and a third element –Look on your reaction foldable or your naming charts. –We wrote this information down back in October.

6. Arrhenius Acid- a chemical compound that increases the concentration of the hydrogen ions, H +, in aqueous solutions. –Form H 3 O + Arrhenius Base- a substance that increases that the concentration of hydroxide ions, OH -, in aqueous solutions

7. Strong: ionize 100% in water –Only 7 are Strong –All are strong electrolytes HI, HClO 4, HBr, HCl, HClO 3, H 2 SO 4, HNO 3 Weak Acid: doesn’t ionize 100% in water –All of the other acids

8. Strong Bases: dissociates 100% –Only 8 –Strong electrolytes Ca(OH) 2, Sr(OH) 2, Ba(OH) 2, NaOH, KOH, RbOH, CsOH, LiOH Weak Bases: doesn’t dissociate 100% –All of the others

9. Page 491 Numbers 3, 5, 8-11 –On 8-11 Name and Classify as strong/weak

10. Bronsted-Lowry Acid- a molecule or ion that is a proton donor Bronsted-Lowry Base- a molecule or ion that is a proton acceptor Water can act as both an acid and a base

11. Conjugate Acid/Base Pairs Acid to form conjugate base it looses an H Base to form conjugate acid it gains an H Amphoteric-species that can react as either an acid or a base

12. Monoprotic Acid- an acid that can donate only one H+ Polyporitc acid is an acid that can donate more than one H+ over a series of steps.

13. Strong Acid + Strong Base = Salt + water Look on page 492 Number 26

14. When water self ionizes it forms an equilibrium reaction. K is a constant that represents equilibrium Kw= ionization constant of water Kw= 1.0 X 10 -14 Kw=[H 3 O+][OH-] AKA: Ka and Kb

15. pH 0-14 This is based on powers of 10 <7 acid >7 base =7 neutral

16. pH + pOH=14 pH= -log [H 3 O + ] [H 3 O + ]=10 -pH pOH= -log [OH - ] [OH - ]= 10 -pOH Kw= [H 3 O + ] [OH - ]

17. Determine the hydronium and hydroxide ion concentration in a solution that is 1E -4 M HCl. 1E -3 M HNO 3 3.0E -2 M NaOH 1.0 E -4 M Ca(OH) 2

18. Determine the pH of the following species –1.0 E -3 M HCl –1.0 E -5 M HNO 3 –1.0 E -4 M NaOH –1.0 E -2 M KOH –Show all ways to work these

19. The pH of a solution is 5. What is the concentration of the hydronium ion? The pH of the solution is 12. What is the hydronium ion concentration? The pH is 1.5. Calculate the hydronium and hydroxide ion. The pH is 3.67 determine the hydronium and hydroxide ion.

20. Page 523 Numbers 8-15, 16 a,b

21. Acid-Base indicators: compounds whose colors are sensitive to pH –Common indicators: methyl red, bromthymol blue, methyl orange, bromphenol blue, phenolphthalein, phenol red

22. You can also use pH paper or a pH meter to give the pH of the solution without a color change. Talk about Titrations