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Entry Task: Jan 25 th Friday

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

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Entry Task: Jan 25 th Friday

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  1. Entry Task: Jan 25th 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.

  4. 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. H2SO4 ____ 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

  5. Provide the name or formula the following acids and bases HF Phosphoric acid H2SO3 Carbonic acid Zn(OH)2 Barium hydroxide KOH Sulfuric acid Fe(OH)2 Hydrocyanic acid H3PO4 Hydrofluoric acid H2CO3 Sulfurous acid Ba(OH)2 Zinc II hydroxide H2SO4 Potassium hydroxide Iron II hydroxide HCN

  6. Identify the B-L acid, base, c-acid, and c-base for the following H2SO4 + NH3 HSO4- + NH4+ NaHCO3 + HClNaCl + H2CO3 CO32– + HC2H3O2 C2H3O2– + HCO3– Base C-base C-acid Acid C-acid C-base Acid Base C-acid Base Acid C-base

  7. Identify the B-L acid, base, c-acid, and c-base for the following HC2H3O2 + H2O  H3O+ + C2H3O2- HF + SO32– F– + HSO3– H3O+ + HSO3– H2O + H2SO3 Base C-acid C-base Acid Base C-acid Acid C-base Base C-base C-acid Acid

  8. Give the conjugate base for each of the following Brønsted-Lowry acids HI NH4+ H2CO3 4. HNO3 I- NH3 HCO3- NO3-

  9. Give the conjugate acid for each of the following Brønsted-Lowry bases. CN– O2– CH3COO– 4. NH3 HCN OH- CH3COOH NH4+

  10. 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.

  11. Exercise Questions 16.8 • Designate the BL acid and BL base on the left side of each reaction and its conjugates on the right. • HCHO2 + H2O  CHO2- + H3O+ • HSO4- + CO32-  SO42- + HCO3– • H3O+ + HPO42-  H2PO4- + H2O Acid C-base C-acid Base Base C-base C-acid Acid Base C-acid C-base Acid

  12. 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 • HNO2 ________________________________ • H2SO4 _______________________________ • HPO42-______________________________ • CH4_________________________________ • CH3NH3+_____________________________ Weak Acid NO2+1 HSO4+1 Strong Acid Weak acid PO4+3 negligible CH3+1 CH3NH2+2 Weak acid

  13. Exercise Questions 16.16 • Predict the products of the following acid-base reactions also predict whether the equilibrium lies to the right or left. • NH2+ H2O  • HClO2+ H2O  • H3O+ + F- Which scenario would likely happen? NH3+ + OH- Water is a stronger acid than OH- so the equilibrium will shift to the product ClO2- + H3O+ HClO2 is a stronger acid than H3O+ so the equilibrium will shift to the product H2O + HF HF is a stronger acid than F- so the equilibrium will shift to the reactant

  14. 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+]= 2.0 x 10-10 this is a basic solution [H+] = 1.0x 10-14 [0.00005] [H+]= 3.1x 10-6 this is a acidic solution [H+] = 1.0x 10-14 [3.2 x10-9] [H+]= 1.0 x 10-9 this is a basic solution [H+] = 1.0x 10-14 [100] [1.0 x10-7]

  15. 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 + H2O  Na+ + OH- + H3O+ This just dilute the solution doing nothing to the H+ level pH = -log (0.0003) = pH = -(-3.52) = 3.52 [H+] = -7.8 [H+]= 1.6 x10-8

  16. Exercise Questions 16.27 Fill in the missing information 1.3 x10-12 2.1 11.9 Acid Acid 2.8 x10-5 9.4 4.6 5.6 x10-9 1.8 x10-6 5.7 Base Base 8.3 5.0 x10-9 2.0 x10-6

  17. Exercise Questions 16.28 Fill in the missing information 7.1 x10-6 1.4 x10-9 8.85 Acid 7.1 x10-7 1.4 x10-8 6.15 Acid 5.6 x10-9 Acid 5.74 8.25 1.1 x10-3 2.96 11.0 Acid

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