1 / 20

Acids Lesson 14 Calculating Kbs

Acids Lesson 14 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

graiden-poole
Download Presentation

Acids Lesson 14 Calculating Kbs

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Acids Lesson 14 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 10-14 Ka(1.7 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. Little Big H2SO4 +2NaOH → Na2SO4 + 2HOH 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 amber in neutral red and yellow in 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 unit of 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 For each change 1 unit of 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

  11. [H+] pH The pH Scale For each change 1 unit of 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 pH decreases by 2 2. If [H+] decreases by 1000 x

  12. [H+] pH The pH Scale For each change 1 unit of 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 pH decreases by 2 2. If [H+] decreases by 1000 x

  13. [H+] pH The pH Scale For each change 1 unit of 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 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 For each change 1 unit of 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 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 For each change 1 unit of 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 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 For each change 1 unit of 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 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 For each change 1 unit of 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 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 For each change 1 unit of 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 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 100x 6. If the pH decreases by 3 units

  19. [H+] pH The pH Scale For each change 1 unit of 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 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 0x 6. If the pH decreases by 3 units

  20. [H+] pH The pH Scale For each change 1 unit of 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 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 100x 6. If the pH decreases by 3 units the [OH-] decreases by 1000x

More Related