1 / 33

AP Chemistry Chapter 17 Jeopardy

AP Chemistry Chapter 17 Jeopardy. Jennie L. Borders. Round 1 – Chapter 17. K sp 100. The molar solubility of PbBr 2 at 25 o C is 1.0 x 10 -2 mol/L. Calculate K sp. 4 x 10 -6. K sp 200. If 0.0490g of AgIO 3 dissolves per liter of solution, calculate the solubility-product constant.

pamelahall
Télécharger la présentation

AP Chemistry Chapter 17 Jeopardy

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. AP ChemistryChapter 17 Jeopardy Jennie L. Borders

  2. Round 1 – Chapter 17

  3. Ksp 100 The molar solubility of PbBr2 at 25oC is 1.0 x 10-2 mol/L. Calculate Ksp. 4 x 10-6

  4. Ksp 200 If 0.0490g of AgIO3 dissolves per liter of solution, calculate the solubility-product constant. 3.03 x 10-8

  5. Ksp 300 A 1L solution saturated at 25oC with calcium oxalate contains 0.0061g calcium oxalate. Calculate the solubility product constant for this salt at 25oC. 2.28 x 10-9

  6. Ksp 400 Calculate the molar solubility of AgBr in 0.1M NaBr solution. The Ksp for AgBr is 5.0 x 10-13. 5 x 10-12M

  7. Ksp 500 Calculate the solubility of Cu(OH)2 in grams per liter of solution. The Ksp for Cu(OH)2 is 4.8 x 10-20. 2.23 x 10-5 g/L

  8. Buffers 100 Calculate the pH of a buffer that is 0.105M in NaHCO3 and 0.125M in Na2CO3. The Ka for HCO3- is 5.6 x 10-11. 10.33

  9. Buffers 200 Calculate the pH of a solution formed by mixing 65mL of 0.20M NaHCO3 with 75mL of 0.15M Na2CO3. The Ka for HCO3- is 5.6 x 10-11. 10.18

  10. Buffers 300 What is the ratio of HCO3- to H2CO3 in blood with a pH of 7.4? The Ka for H2CO3 is 4.3 x 10-7. 10.8

  11. Buffers 400 A buffer solution contains 0.1 mol of C2H5COOH and 0.13 mol C2H5COONa in 1.50L. What is the pH of the buffer after the addition of 0.10 mol of NaOH? 5.08

  12. Buffers 500 A buffer solution contains 0.1 mol of C2H5COOH and 0.13 mol C2H5COONa in 1.50L. What is the pH of the buffer after the addition of 0.01 mol of HI? (Ka = 1.3 x 10-5) 4.93

  13. Strong-Strong Titrations 100 A 20mL sample of 0.200M HBr is titrated with 0.200M NaOH solution. Calculate the pH of the solution after 15mL of base has been added. 1.54

  14. Strong-Strong Titrations 200 A 20mL sample of 0.200M HBr is titrated with 0.200M NaOH solution. Calculate the pH of the solution after 19.9mL of base has been added. 3.30

  15. Strong-Strong Titrations 300 A 20mL sample of 0.200M HBr is titrated with 0.200M NaOH solution. Calculate the pH of the solution after 20.0mL of base has been added. 7.00

  16. Strong-Strong Titrations 400 A 20mL sample of 0.200M HBr is titrated with 0.200M NaOH solution. Calculate the pH of the solution after 20.1mL of base has been added. 10.70

  17. Strong-Strong Titrations 500 A 20mL sample of 0.200M HBr is titrated with 0.200M NaOH solution. Calculate the pH of the solution after 35.0mL of base has been added. 12.74

  18. Strong-Weak Titrations 100 Consider the titration of 30.0mL of 0.03 M NH3with 0.025M HCl. Calculate the pH after 0mL of the titrant has been added. (Kb = 1.8 x 10-5) 10.87

  19. Strong-Weak Titrations 200 Consider the titration of 30.0mL of 0.03M NH3with 0.025M HCl. Calculate the pH after 10.0mL of the titrant has been added. (Kb = 1.8 x 10-5) 9.67

  20. Strong-Weak Titrations 300 Consider the titration of 30.0mL of 0.03M NH3with 0.025M HCl. Calculate the pH after 20.0mL of the titrant has been added. (Kb = 1.8 x 10-5) 9.16

  21. Strong-Weak Titrations 400 Consider the titration of 30.0mL of 0.03M NH3with 0.025M HCl. Calculate the pH after 36.0mL of the titrant has been added. (Kb = 1.8 x 10-5) 5.55

  22. Strong-Weak Titrations 500 Consider the titration of 30.0mL of 0.030M NH3with 0.025M HCl. Calculate the pH after 37.0mL of the titrant has been added. (Kb = 1.8 x 10-5) 3.43

  23. Solubility 100 Would MnS be more soluble in acidic solution than in pure water? Write the equation. Yes MnS + 2H+ Mn2+ + H2S

  24. Solubility 200 Would PbF2 be more soluble in acidic solution than in pure water? Write the equation. Yes PbF2 + 2H+ Pb2+ + 2HF

  25. Solubility 300 Would AuCl3 be more soluble in acidic solution than in pure water? Write the equation. No AuCl3 + 3H+ Au3+ + HCl strong acid

  26. Solubility 400 Would Hg2C2O4 be more soluble in acidic solution than in pure water? Write the equation. Yes Hg2C2O4 + 2H+ 2Hg+ + H2C2O4

  27. Solubility 500 Would CuBr be more soluble in acidic solution than in pure water? Write the equation. No CuBr + H+ Cu+ + HBr strong acid

  28. Precipitates 100 Will Ca(OH)2 precipitate from solution if the pH of a 0.05M solution of CaCl2 is adjusted to 8.0? (Ksp = 6.5 x 10-6) Q < Ksp so no Ca(OH)2 will precipitate

  29. Precipitates 200 Will Ag2SO4 precipitate with 100mL of 0.05M AgNO3 is mixed with 10mL of 5.0 x 10-2M Na2SO4 solution? (Ksp = 1.5 x 10-5) Q < Ksp so no Ag2SO4 will precipitate

  30. Precipitates 300 Will Ca(OH)2 precipitate from solution if the pH of a 0.02M solution of Co(NO3)2 is adjusted to 8.5? (Ksp = 1.3 x 10-15) Q > Ksp so Co(OH)2 will precipitate

  31. Precipitates 400 Will AgIO3 precipitate when 20mL of 0.01M AgNO3 is mixed with 10mL of 0.015M NaIO3? (Ksp = 3.1 x 10-8) Q > Ksp so AgIO3 will precipitate

  32. Precipitates 500 A solution of Na2SO4 is added dropwise to a solution that is 0.010M in Ba2+ (Ksp = 1.1 x 10-10) and 0.01M Sr2+ (Ksp = 3.2 x 10-7). Which will precipitate first? BaSO4 precipitates first

More Related