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Acids Lesson 12 Calculating Kbs

Acids Lesson 12 Calculating Kbs. You can calculate the Kb using the Ka from the data package page 6 and the equation below. Ka x Kb = 1.0 x 10 -14 @ 25 o C Kb = Kw Ka(conjugate) or Ka = Kw Kb(conjugate). Calculate the Kb for CN - . Kb( CN - ) = Kw

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Acids Lesson 12 Calculating Kbs

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  1. Acids Lesson 12 Calculating Kbs

  2. You can calculate the Kb using the Ka from the data package page 6 and the equation below. Ka x Kb = 1.0 x 10-14 @ 25 oC Kb = Kw Ka(conjugate) or Ka = Kw Kb(conjugate)

  3. Calculate the Kb for CN-. • Kb(CN-) = Kw • Ka(HCN) • = 1 x 10-144.9 x 10-10 • = 2.0 x 10-5

  4. 2. Calculate the Kb for K2HPO4. Kb(HPO42-) = Kw Ka(H2PO4-) = 1 x 10-146.2 x 10-8 = 1.6 x 10-7

  5. 3. Calculate the Kb for K2HC6H5O7. Kb(HC6H5O72-) = Kw Ka(H2C6H5O7-) = 1 x 10-141.7 x 10-5 = 5.9 x 10-10

  6. 4. 200.0 mL of 0.200 M H2SO4 is mixed with 400.0 mL of 0.250 M NaOH. Calculate the pH of the new solution. H2SO4 +2NaOH 0.2000 L x 0.200 mole 0.4000 L x 0.250 mole 1 L 1 L I 0.0400 moles 0.100 moles C -0.0400 moles -0.0800 moles E 0 0.020 moles note the loss of 1 sig fig Final volume = 200.0 mL + 400.0 mL = 600.0 mL [NaOH] = 0.020 moles = 0.033 M0.6000 L pOH = 1.48 pH = 12.52

  7. 5.What is the pH of a solution that is amberin neutral red and yellowin thymol blue? Look at page 7 amber in neutral red pH is 8 or higher yellow in thymol bluepH is 8 or less pH = 8

  8. 6. What is the pH of a solution that is blue in Indigo carmine and thymolphthalein? Look at page 7 blue in indigo carmine pH is 11.4 or less blue in thymolphthaleinpH is 10.6 or greater pH = 11

  9. [H+]pH The pH Scale For each change 1 unitof pH the [H+]and [OH-]change by a factor of 10 x. This is the nature of the logarithm. 1. If [H+] increases by 100 x

  10. [H+] pH The pH Scale 1. If [H+] increases by 100 x

  11. [H+] pH The pH Scale 1. If [H+] increases by 100 x pH decreases by 2 2. If [H+] decreases by 1000 x

  12. [H+] pH The pH Scale 1. If [H+] increases by 100 x pH decreases by 2 2. If [H+] decreases by 1000 x

  13. [H+] pH The pH Scale 1. If [H+] increases by 100 x pH decreases by 2 2. If [H+] decreases by 1000 x the pH increases by 3 3. If [OH-] increases by 100 x

  14. [H+] pH The pH Scale 1. If [H+] increases by 100 x pH decreases by 2 2. If [H+] decreases by 1000 x the pH increases by 3 3. If [OH-] increases by 100 x

  15. [H+] pH The pH Scale 1. If [H+] increases by 100 x pH decreases by 2 2. If [H+] decreases by 1000 x the pH increases by 3 3. If [OH-] increases by 100 x the pH increases by 2 4. If [OH-] decreases by 1000 x

  16. [H+] pH The pH Scale 1. If [H+] increases by 100 x pH decreases by 2 2. If [H+] decreases by 1000 x the pH increases by 3 3. If [OH-] increases by 100 x the pH increases by 2 4. If [OH-] decreases by 1000 x

  17. [H+] pH The pH Scale 1. If [H+] increases by 100 x pH decreases by 2 2. If [H+] decreases by 1000 x the pH increases by 3 3. If [OH-] increases by 100 x the pH increases by 2 4. If [OH-] decreases by 1000 x the pH decreases by 3 5. If the pH increases by 2 units

  18. [H+] pH The pH Scale 1. If [H+] increases by 100 x pH decreases by 2 2. If [H+] decreases by 1000 x the pH increases by 3 3. If [OH-] increases by 100 x the pH increases by 2 4. If [OH-] decreases by 1000 x the pH decreases by 3 5. If the pH increases by 2 unitsthe [H+] decreases by 100 x 6. If the pH decreases by 3 units

  19. [H+] pH The pH Scale 1. If [H+] increases by 100 x pH decreases by 2 2. If [H+] decreases by 1000 x the pH increases by 3 3. If [OH-] increases by 100 x the pH increases by 2 4. If [OH-] decreases by 1000 x the pH decreases by 3 5. If the pH increases by 2 units the [H+] decreases by 100 x 6. If the pH decreases by 3 units

  20. [H+] pH The pH Scale 1. If [H+] increases by 100 x pH decreases by 2 2. If [H+] decreases by 1000 x the pH increases by 3 3. If [OH-] increases by 100 x the pH increases by 2 4. If [OH-] decreases by 1000 x the pH decreases by 3 5. If the pH increases by 2 units the [H+] decreases by 100 x 6. If the pH decreases by 3 units the [OH-] decreases by 1000 x

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