1. AP Chemistry Chapter 17 Jeopardy Jennie L. Borders

2. Round 1 – Chapter 17

3. K sp Buffers Strong- Strong Titrations Strong- Weak Titrations SolubilityPrecipitates 100 200 300 400 500

4. 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

5. K sp 200 If 0.0490g of AgIO 3 dissolves per liter of solution, calculate the solubility-product constant. 3.03 x 10 -8

6. K sp 300 A 1L solution saturated at 25 o C with calcium oxalate contains 0.0061g calcium oxalate. Calculate the solubility product constant for this salt at 25 o C. 2.28 x 10 -9

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

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

9. Buffers 100 Calculate the pH of a buffer that is 0.105M in NaHCO 3 and 0.125M in Na 2 CO 3. The K a for HCO 3 - is 5.6 x 10 -11. 10.33

10. Buffers 200 Calculate the pH of a solution formed by mixing 65mL of 0.20M NaHCO 3 with 75mL of 0.15M Na 2 CO 3. The K a for HCO 3 - is 5.6 x 10 -11. 10.18

11. Buffers 300 What is the ratio of HCO 3 - to H 2 CO 3 in blood with a pH of 7.4? The K a for H 2 CO 3 is 4.3 x 10 -7. 10.8

12. Buffers 400 A buffer solution contains 0.1 mol of C 2 H 5 COOH and 0.13 mol C 2 H 5 COONa in 1.50L. What is the pH of the buffer after the addition of 0.10 mol of NaOH? 5.08

13. Buffers 500 A buffer solution contains 0.1 mol of C 2 H 5 COOH and 0.13 mol C 2 H 5 COONa in 1.50L. What is the pH of the buffer after the addition of 0.01 mol of HI? (K a = 1.3 x 10 -5 ) 4.93

14. 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

15. 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

16. 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

17. 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

18. 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

19. Strong-Weak Titrations 100 Consider the titration of 30.0mL NH 3 with 0.025M HCl. Calculate the pH after 0mL of the titrant has been added. (K b = 1.8 x 10 -5 ) 10.87

20. Strong-Weak Titrations 200 Consider the titration of 30.0mL NH 3 with 0.025M HCl. Calculate the pH after 10.0mL of the titrant has been added. (K b = 1.8 x 10 -5 ) 9.67

21. Strong-Weak Titrations 300 Consider the titration of 30.0mL NH 3 with 0.025M HCl. Calculate the pH after 20.0mL of the titrant has been added. (K b = 1.8 x 10 -5 ) 9.16

22. Strong-Weak Titrations 400 Consider the titration of 30.0mL NH 3 with 0.025M HCl. Calculate the pH after 36.0mL of the titrant has been added. (K b = 1.8 x 10 -5 ) 5.55

23. Strong-Weak Titrations 500 Consider the titration of 30.0mL of 0.030M NH 3 with 0.025M HCl. Calculate the pH after 37.0mL of the titrant has been added. (K b = 1.8 x 10 -5 ) 3.43

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

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

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

27. Solubility 400 Would Hg 2 C 2 O 4 be more soluble in acidic solution than in pure water? Write the equation. Yes Hg 2 C 2 O 4 + 2H +  2Hg + + H 2 C 2 O 4

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

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

30. Precipitates 200 Will Ag 2 SO 4 precipitate with 100mL of 0.05M AgNO 3 is mixed with 10mL of 5.0 x 10 -2 M Na 2 SO 4 solution? (K sp = 1.5 x 10 -5 ) Q < K sp so no Ag 2 SO 4 will precipitate

31. Precipitates 300 Will Ca(OH) 2 precipitate from solution if the pH of a 0.02M solution of Co(NO 3 ) 2 is adjusted to 8.5? (K sp = 1.3 x 10 -15) Q > K sp so Co(OH) 2 will precipitate

32. Precipitates 400 Will AgIO 3 precipitate when 20mL of 0.01M AgNO 3 is mixed with 10mL of 0.015M NaIO 3 ? (K sp = 3.1 x 10 -8 ) Q > K sp so AgIO 3 will precipitate

33. Precipitates 500 A solution of Na 2 SO 4 is added dropwise to a solution that is 0.010M in Ba 2+ (K sp = 1.1 x 10 -10) and 0.01M Sr 2+ (K sp = 3.2 x 10 -7 ). Which will precipitate first? BaSO 4 precipitates first