2. Objective: Students will learn how to name acids, identify the properties of acids and bases, and calculate pH, pOH, [H+] and [OH-]. Warm-Up: KWL for Acids and Bases

3. Objective: Students will learn how to name acids, identify the properties of acids and bases, and calculate pH, pOH, [H+] and [OH-]. Warm-Up: How many grams of KOH are needed to make 250. mL of a 0.25 M solution?

4. Properties of Acids and Bases Acids Sour taste pH<7 Vinegar, lemon juice, orange juice, Releases H+ ion in water Turns litmus paper red HCl, HNO 3, H 2 SO 4 electrolyte Bases Bitter taste pH > 7 Baking soda, bleach, soap Releases OH- ion in water Turns litmus paper blue NH 4 OH, NaOH, KOH electrolyte

5. Naming Acids How do you know it is an acid? The compound starts with an “H”. With a partner, complete the packet.

6. Rules for Naming Acids Rule #1-If the acid has only two elements, then it starts with HYDRO- and end in –IC Acid Rule #2-If the acid has 3 elements and the anion ends in –ATE, the acid ends in –IC ACID, if the anion ends in –ITE, the acid ends in –OUS ACID

7. In other words… I –ATE something –ICky and got a disease called –ITE –OUS.

8. Objective/Warm-Up SWBAT name acids, calculate pH and pOH. Label as acid or base. pH = 3 Feels slippery Releases OH- ions Tastes sour Releases H+ ions pH = 12

9. Naming Acids AcidIon NameStemAcid Name H3NH3NNitrideNitrHydronitric acid HNO 2 NitriteNitrNitrous acid HNO 3 NitrateNitrNitric acid

10. Binary Acids HCl HYDRO chlor IC ACID HI HYDRO iod IC ACID H 2 S HYDRO sulfur IC ACID

11. Ternary Acids-End in ATE HNO 3 NitrIC ACID H 3 PO 4 PhosphorIC ACID H 2 SO 4 sulfurIC ACID

12. Ternary Acids-End in ITE HNO 2 nitrOUS ACID H 3 PO 3 phosphorOUS ACID H 2 SO 3 sulfurOUS ACID

13. Bases KOH Potassium hydroxide Ca(OH) 2 Calcium hydroxide NH 4 OH Ammonium hydroxide Na 2 SO 4 Sodium sulfate

14. What does pH mean? pH = -log [H + ] Brackets indicate Molarity [H+]pH 10 -1 0.1 M 1 10 -2 0.01 M 2 10 -3 0.001 M 3

16. What does pH mean? It is a way to measure the hydrogen ion concentration. Water breaks apart to hydrogen and hydroxide ions: H 2 O  H + + OH - pH + pOH = 14

18. pH and pOH [H+]pH[OH-]pOHAcid or Base 10 -5

19. pH and pOH [H+]pH[OH-]pOHAcid or Base 10 -5 510 -9 9acid 6

20. pH and pOH [H+]pH[OH-]pOHAcid or Base 10 -5 510 -9 9acid 10 -8 810 -6 6base 10 0

21. pH and pOH [H+]pH[OH-]pOHAcid or Base 10 -5 510 -9 9acid 10 -8 810 -6 6base 10 0 010 -14 14acid neutral

22. pH and pOH [H+]pH[OH-]pOHAcid or Base 10 -5 510 -9 9acid 10 -8 810 -6 6base 10 0 010 -14 14acid 10 -7 7 7neutral

24. Acid-Base Reactions Like double displacement reactions.

25. Label the Acid, Base, Conjugates HCN + H 2 O  H 3 O + + CN - Acid + base  CA + CB NaHCO 3 + HBr  NaBr + H 2 CO 3 Base + Acid  CB + CA H 2 O + NH 3  NH 4 + + OH - Acid + Base  CA + CB

26. What is the Conjugate Base? HNO 3 NO 3 - H 2 PO 3 - HPO 3 -2 NH 3 NH 2 -

27. Is it an Acid or a Base? pH = 3 Feels slippery Releases OH- ions Tastes sour Releases H+ ions pH = 12 pH = 7 electrolyte Acid Base Acid Base Neutral both