Which of the following is a soluble, strong base? RbOH NH3 Al(OH)3 Co(OH)3 Co(OH)2 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50

Which salt is produced from a strong acid and a strong base? NH4Cl NaClO KClO3 Na2CO3 LiNO2 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50

0.10 M NH4NO3 0.10 M K2SO4 0.20 M BaSO4 0.10 M NaCl 0.10 M HClO4 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 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50

I and II I, II, and III IV and V IV, V, and VI none of these 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 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50

The pH of a solution is 4.80. What is the concentration of hydroxide ions in this solution? 4.2 x 10-9 M 1.6 x 10-5 M 3.6 x 10-12 M 6.3 x 10-10 M 2.0 x 10-8 M 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50

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 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50

We add enough acid to a solution to cause the pH to decrease from 6 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. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50

I, II, and III II, IV, V, and VI I, II, and VI IV, V, and VI I and III 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 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50

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 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50

Calculate the original molarity of a solution of acetic acid that is 3 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 10-2 M 0.038 M 3.4 x 10-4 M 6.7 x 10-4 M 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50

Trimethylamine ionizes as follows in water 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% 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50

Which of the following anions is the strongest base? Cl- NO3- ClO4- F- Br- 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50

I and II I, II, III, and V III and IV IV and V I, II, and V 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 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50

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 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50

What is the pH of 0.25 M KCN solution? 1.17 2.60 10.42 11.40 12.83 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50

What is the percent hydrolysis in 0.20 M NaNO2 solution? 0.0064% 0.0047% 0.0010% 0.00061% 0.00092% 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50

Calculate the [H3O+] in a 0.20 M KCN solution. 2.2 x 10-3 M 1.0 x 10-7 M 2.4 x 10-11 M 4.5 x 10-12 M 3.0 x 10-12 M 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50

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) 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50

Calculate the pH of 0.050 M NH4Cl. 4.62 4.84 5.04 5.16 5.28 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50

Calculate the pH of 0.15 M Co(NO3)2. 4.52 4.74 4.88 5.06 5.28 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 45 46 47 48 49 50