1. Entry Task: Jan 25 th Friday Question: Identify the acid, base and conjugate acid and conjugate base when nitric acid reacts with sodium hydroxide. You have 5 minutes

2. Agenda: Discuss Acid Base properties & pH ws. HW: Ch. 16 sec. 5-7 reading notes

3. I can… Distinguish an acid from a base by its properties. Explain the difference theories of acid and base behavior of an Arrhenius A/B, Bronsted-Lowry A/B and Lewis A/B. Use the concentrations of acids and bases to calculate pH and pOH.

5. Label the following as A- acid or B- base ____1.KOH ____2.covalently bonded ____3.Red with litmus paper ____4.negative charged solution ____5.Hydrogen ions ____6.pH 8-14 ____7.Reacts to carbonates ____8.positive charged solutions ____9.Reacts to metals ____10.blue with litmus paper ____11.H 2 SO 4 ____12.H in front of its formula ____13.Hydroxide ions ____14.Does not react with carbonates ____15.pH 0-6 ____16.nonmetal-nonmetal ____17.Does not react with metals ____18.metal-nonmetal ____19.OH on the back of its formula ____20.ionically bonded B A A B A B A A A B A A B B A A B B B B

6. Provide the name or formula the following acids and bases HF Phosphoric acid H 2 SO 3 Carbonic acid Zn(OH) 2 Barium hydroxide KOH Sulfuric acid Fe(OH) 2 Hydrocyanic acid Hydrofluoric acidH 3 PO 4 Sulfurous acid H 2 CO 3 Zinc II hydroxide Ba(OH) 2 Potassium hydroxide H 2 SO 4 Iron II hydroxideHCN

7. Identify the B-L acid, base, c-acid, and c-base for the following H 2 SO 4 + NH 3  HSO 4 - + NH 4 + NaHCO 3 + HCl  NaCl + H 2 CO 3 CO 3 2– + HC 2 H 3 O 2  C 2 H 3 O 2 – + HCO 3 – Acid C-baseBaseC-acid Acid C-base Base C-acid AcidC-baseBase C-acid

8. Identify the B-L acid, base, c-acid, and c-base for the following HC 2 H 3 O 2 + H 2 O  H 3 O + + C 2 H 3 O 2 - HF + SO 3 2–  F – + HSO 3 – H 3 O + + HSO 3 –  H 2 O + H 2 SO 3 Acid C-baseBaseC-acid AcidC-base BaseC-acid Acid C-baseBaseC-acid

9. Give the conjugate base for each of the following Brønsted-Lowry acids 1.HI 2.NH 4 + 3.H 2 CO 3 4. HNO 3 I-I- NH 3 HCO 3 - NO 3 -

10. Give the conjugate acid for each of the following Brønsted-Lowry bases. 1.CN – 2.O 2– 3.CH 3 COO – 4. NH 3 HCN OH - CH 3 COOH NH 4 +

11. What is the difference between a strong acid and a weak acid? Strong acids completely ionize in water making them strong conductors of electricity. Weak acids partially ionize in water making them weak conductors of electricity.

12. Exercise Questions 16.8 Designate the BL acid and BL base on the left side of each reaction and its conjugates on the right. HCHO 2 + H 2 O  CHO 2 - + H 3 O + HSO 4 - + CO 3 2-  SO 4 2- + HCO 3 – H 3 O + + HPO 4 2-  H 2 PO 4 - + H 2 O AcidC-base Base C-acid Acid C-baseBaseC-acid Acid C-baseBaseC-acid

13. Exercise Questions 16.11 Label each of the following as being a strong acid, weak acid or a species with negligible acidity AND provide its conjugate base HNO 2 ________________________________ H 2 SO 4 _______________________________ HPO 4 2- ______________________________ CH 4 _________________________________ CH 3 NH 3 + _____________________________ Weak Acid Weak acid Strong Acid negligible Weak acid NO 2 +1 HSO 4 +1 PO 4 +3 CH 3 +1 CH 3 NH 2 +2

14. Exercise Questions 16.16 Predict the products of the following acid-base reactions also predict whether the equilibrium lies to the right or left. NH 2 + H 2 O  HClO 2 + H 2 O  H 3 O + + F -  NH 3 + + OH - Which scenario would likely happen? Water is a stronger acid than OH- so the equilibrium will shift to the product ClO 2 - + H 3 O + HClO 2 is a stronger acid than H 3 O+ so the equilibrium will shift to the product H 2 O + HF HF is a stronger acid than F- so the equilibrium will shift to the reactant

15. Exercise Questions 16.19 Calculate [H+] for each of the following solutions and indicate whether the solution is acidic, basic or neutral: SHOW WORK!! [OH-] = 0.00005M [OH-] = 3.2 x10 -9 Solution with 100 times greater than [H+] [H+] = 1.0x 10 -14 [OH-] [H+] = 1.0x 10 -14 [0.00005] [H+]= 2.0 x 10 -10 this is a basic solution [H+] = 1.0x 10 -14 [3.2 x10 -9 ] [H+]= 3.1x 10 -6 this is a acidic solution [H+] = 1.0x 10 -14 [100] [1.0 x10 -7 ] [H+]= 1.0 x 10 -9 this is a basic solution

16. Exercise Questions 16.25 If NaOH is added to water, how does [H+] change? If [H+] = 0.0003M. What is the pH? If pH is 7.8, what is the molar concentration of H+ and OH- in solution? NaOH + H 2 O  Na + + OH - + H 3 O + This just dilute the solution doing nothing to the H+ level pH = -log (0.0003) = pH = -(-3.52) = 3.52 [H+]= 1.6 x10 -8 [H+] = -7.8

17. [H+][OH-]pHpOHAcid/Base 7.5 x 10 -3 M 3.6 x 10 -10 M 8.25 5.70 Exercise Questions 16.27 Fill in the missing information 1.3 x10 -12 11.9 2.1 Acid 9.42.8 x10 -5 4.6 Acid 5.6 x10 -9 1.8 x10 -6 5.7Base 2.0 x10 -6 5.0 x10 -9 8.3 Base

18. Exercise Questions 16.28 Fill in the missing information [H+][OH-]pHpOHAcid/Base 5.15 7.85 1.8 x 10 -6 M 9.2 x 10 -12 M 7.1 x10 -6 8.85 Acid 1.4 x10 -9 1.4 x10 -8 7.1 x10 -7 6.15 Acid 5.6 x10 -9 8.255.74 Acid 1.1 x10 -3 2.9611.0Acid