1 / 20

Which of the following is a soluble, strong base?

Which of the following is a soluble, strong base?. RbOH NH 3 Al(OH) 3 Co(OH) 3 Co(OH) 2. Which salt is produced from a strong acid and a strong base?. NH 4 Cl NaClO KClO 3 Na 2 CO 3 LiNO 2.

maesimpson
Download Presentation

Which of the following is a soluble, strong base?

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. Which of the following is a soluble, strong base? • RbOH • NH3 • Al(OH)3 • Co(OH)3 • Co(OH)2

  2. Which salt is produced from a strong acid and a strong base? • NH4Cl • NaClO • KClO3 • Na2CO3 • LiNO2

  3. Which solution should be the best conductor of electrical current because it would contain the largest number of ions in aqueous solution? • 0.10 M NH4NO3 • 0.10 M K2SO4 • 0.20 M BaSO4 • 0.10 M NaCl • 0.10 M HClO4

  4. Consider a 0.020 M Fe2(SO4)3 solution. Which one of the responses includes all of the following statements that are correct, and no incorrect statements? I. The solution is 0.020 M in Fe3+. II. The solution is 0.030 M in SO42-. III. The total concentration of ions in the solution is 0.050 M. IV. The solution is 0.040 M in Fe3+. V. The solution is 0.060 M in SO42-. VI. The total concentration of ions in the solution is 0.10 M. • I and II • I, II, and III • IV and V • IV, V, and VI • none of these

  5. The pH of a solution is 4.80. What is the concentration of hydroxide ions in this solution? • 4.2 x 10-9M • 1.6 x 10-5M • 3.6 x 10-12M • 6.3 x 10-10M • 2.0 x 10-8M

  6. Calculate the pH of a solution that is 0.00030 M in Ba(OH)2. • 10.47 • 9.94 • 8.63 • 12.42 • 10.78

  7. We add enough acid to a solution to cause the pH to decrease from 6.5 to 5.5. This means that • [OH-] increases by a factor of 10. • [H3O+] increases by a factor of 10. • [OH-] increases by 1 M. • [H3O+] increases by 1 M. • [H3O+] increases by a factor of 6.5/5.5.

  8. Which response includes all of the following that are weak acids, and no strong acids? I. H2SO3 II. HClO III. H2SO4 IV. HClO3 V. HClO4 VI. C6H5COOH • I, II, and III • II, IV, V, and VI • I, II, and VI • IV, V, and VI • I and III

  9. Calculate the pH of 0.020 M HOBr solution. Ka= 2.5 x 10-9 • 4.80 • 4.91 • 5.02 • 5.15 • 5.38

  10. Calculate the original molarity of a solution of acetic acid that is 3.0% ionized. Ka = 1.8 x 10-5 • 0.076 M • 1.9 x 10-2M • 0.038 M • 3.4 x 10-4M • 6.7 x 10-4M

  11. Trimethylamine ionizes as follows in water. What is the percent ionization for a 9.0 x 10-2 M solution of (CH3)3N? Kb = 7.4 x 10-5 (CH3)3N + H2O {image} (CH3)3NH+ + OH- • 2.9% • 0.030% • 0.18% • 0.42% • 5.8%

  12. Which of the following anions is the strongest base? • Cl- • NO3- • ClO4- • F- • Br-

  13. Which response includes all of the following salts that give neutral aqueous solutions, and no other salts? I. KNO3 II. BaCl2 III. NaCH3COO IV. NH4Cl V. NaBr • I and II • I, II, III, and V • III and IV • IV and V • I, II, and V

  14. What is the value of the (base) hydrolysis constant for NaBO2, sodium metaborate? • 3.2 x 10-6 • 1.7 x 10-5 • 1.8 x 10-6 • 6.0 x 104 • 2.2 x 10-7

  15. What is the pH of 0.25 M KCN solution? • 1.17 • 2.60 • 10.42 • 11.40 • 12.83

  16. What is the percent hydrolysis in 0.20 M NaNO2 solution? • 0.0064% • 0.0047% • 0.0010% • 0.00061% • 0.00092%

  17. Calculate the [H3O+] in a 0.20 M KCN solution. • 2.2 x 10-3M • 1.0 x 10-7M • 2.4 x 10-11M • 4.5 x 10-12M • 3.0 x 10-12M

  18. The hydrolysis constant that would be used to calculate the pH in NH4Cl solution is given by • Kw/Ka (HCl) • Kw/Ka(Cl-) • Kw/Kb(NH3) • Kw/Kb(NH4+) • Kw/Kb(NH4Cl)

  19. Calculate the pH of 0.050 M NH4Cl. • 4.62 • 4.84 • 5.04 • 5.16 • 5.28

  20. Calculate the pH of 0.15 M Co(NO3)2. • 4.52 • 4.74 • 4.88 • 5.06 • 5.28

More Related