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Entry Task: May 8 th -9 th Block 1

Entry Task: May 8 th -9 th Block 1. Question: Identify B-L acid. Base, c-acid and c-base. C 2 O 4 2- + HC 2 H 3 O 2  HC 2 O 4 - + C 2 H 3 O 2 -. Agenda:. Discuss Bronsted - Lowery ws Acid-Base Part 3- Ionization & pH Notes Ionization & pH ws.

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Entry Task: May 8 th -9 th Block 1

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  1. Entry Task: May 8th-9th Block 1 Question: Identify B-L acid. Base, c-acid and c-base. C2O42- + HC2H3O2 HC2O4- + C2H3O2-

  2. Agenda: • Discuss Bronsted- Lowery ws • Acid-Base Part 3- Ionization & pH Notes • Ionization & pH ws

  3. For the following reactions, label the acid, base, conjugate acid and conjugate base. H2SO4 + NH3 HSO4- + NH4+ NaHCO3 + HClNaCl + H2CO3 OH- + HCN  H2O + CN- c-acid c-base base acid base c-base acid c-acid acid base c-acid c-base

  4. For the following reactions, label the acid, base, conjugate acid and conjugate base. HC2H3O2+ H2O  H3O+ + C2H3O2- HCl+ NH3 NH4+ + Cl PO4-3+ HNO3 NO3- + HPO42- c-base base acid c-acid acid c-base base c-acid acid c-base c-acid base

  5. What is the conjugate base of the following acids? HClO4 b) NH4+ c) H2O d) HCO3- ClO4- NH3 CO3-2 OH-

  6. What is the conjugate acid of the following bases? CN- b) SO42- c) H2O d) HCO3- HCN HSO4- H2CO3 H3O+

  7. H3O+ NO2- H2O + F-HF + OH- HCN NH3 CN- NH4+ OH- HClO3 HClO3 + OH- H2O + ClO3- HPO4-2 SO4-2 HSO4- + PO4-3 H2SO4-+ HPO4-2 H2O S-2 HS- OH- H2O CO2H- HCO2H + OH- H2O + CO2H-

  8. Acid Ionization Acid solutions contains more positive ions (H3O+) than negative (Cl-) ions 1st CO2 + H2O  H2CO2 Not balanced to simplify things Ionization part CO2 CO2-2 H2CO2 + H2O  H3O + CO2-2 Not balanced to simplify things H3O+ H3O+ CO2-2 H3O+ H3O+ CO2-2 CO2-2

  9. Practice Acid Ionization reactionsMonoprotic HClO3 + H2O  _______ + ClO3- H3O+ CHO2- HCHO2 + H2O  H3O+ + _______ HC6H5S ________ + H2O H3O+ + C6H5S- HCN + H2O  ______ + _____ H3O+ CN- Monoprotic acids: have one acidic hydrogen Diprotic acids: have two acidic hydrogens H2SO4 Triprotic acids: have three acidic hydrogens H3C6H5O7

  10. Practice Acid Ionization reactionsDiprotic H2SO4 + H2O  H3O+ + HSO4- Step 1 HSO4- + H2O  H3O+ + SO4-2 Step 2

  11. Practice Acid Ionization reactionsTriprotic Step 1 H3PO4 + H2O  H3O+ + H2PO4- H2PO4- + H2O  H3O+ + HPO4-2 Step 2  HPO4-2 + H2O H3O+ + PO4-3 Step 3

  12. Strong verses Weak What make a strong acid or base different from a weak acid or base?

  13. Lets examine the ionization of this acid- HA HA What happens to the HA molecules in solution?

  14. Complete Ionization of HA HA H+ Strong Acid A- Would the solution be conductive?

  15. Lets examine the ionization of this acid- HA HA What happens to the HA molecules in solution?

  16. Partial ionization of HA HA H+ Weak Acid A- Would the solution be conductive?

  17. HA  H+ + A- HA Weak Acid H+ At any one time, only a fraction of the molecules are ionizedand stay that way A-

  18. Ionization and what it means Strong acids tend to have weak conjugate bases Strong bases tend to have weak conjugate acids

  19. Expression of Ion relationships H2O(l) H3O+(aq) + OH−(aq) Water has an equal [H+] as [OH-]. The brackets [ ] means concentration. Acids the [H+] is higher Acids the [OH-] is lower OR Bases the [H+] is lower Bases the [OH-] is higher

  20. What is pH? It’s the negative logarithm of the concentration of hydrogen ions in a solution is expressed as a number (0-14) pH is short for the power of hydrogen.

  21. pH Notes Acids- amount of H+ pH Base- amount of OH- 0 1x10-14= 0.00000000000001 1x100= 1 3 1x10-11= 0.00000000001 1x10-3= 0.001 7 1x10-7= 0.0000001 1x10-7= 0.0000001 1x10-11= 0.00000000001 11 1x10-3= 0.001 14 1x100= 1 1x10-14= 0.00000000000001

  22. What is the correlation between the pH value and hydrogen ions? If there is a high amount of hydrogen ions the lower the pH number is. Think of it this way: 1x100= 1 = pH of 0 this means that there are TONS of hydrogen ions 1x10-4= 0.0001 = pH of 4 = this means that there are thousandth of hydrogen ions 1x10-11= 0.00000000001 = pH of 11 this means that there are not a lot of hydrogen ions

  23. How many hydrogen ions are expressed in a pH of 12? 1x10-12 How does pH express the concentration of hydroxide ions? In short~ it is what is NOT measured. So if the pH is 3, the amount of hydrogen ions is 1x10-3so this same solution would have 1x10-11HYDROXIDE ions. So if the pH is 12, the amount of hydrogen ions is 1x10-12so this same solution would have 1x10-2HYDROXIDE ions.

  24. If a solution has a pH of 10, what is the concentration of hydrogen ions is ___ and the hydroxide ions are ____. 1x10-10 1x10-4 What happens to the pH if the amount of hydrogen ions increases? The pH would be more acidic of lower pH.

  25. pH Notes Acids- amount of H+ pH Base- amount of OH- 0 1x10-14= 0.00000000000001 1x100= 1 3 1x10-11= 0.00000000001 1x10-3= 0.001 7 1x10-7= 0.0000001 1x10-7= 0.0000001 1x10-11= 0.00000000001 11 1x10-3= 0.001 14 1x100= 1 1x10-14= 0.00000000000001

  26. What is the concentration difference between a pH of 3 and a pH of 4? 1x10-3 has 10 times > H+ than a solution with 1x10-4. 1x10-3 has 10 times <OH- than a solution with 1x10-4.

  27. What is pOH? It’s the negative logarithm of the concentration of hydroxide ions in a solution is expressed as a number (0-14). It mirrors the same relationship. pH of 4 the pOH would be= pH of 1 the pOH would be= pH of 7 the pOH would be= pH of 11 the pOH would be=

  28. What is pOH? 1x10-10has 10 times >H+ than a solution with1x10-11. 1x10-10has 10 times <OH- than a solution with 1x10-11.

  29. Finish the backside of the notesIonization and pH ws pH lab Tomorrow wear appropriate garments!!

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