which of the following is a soluble strong base l.
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Which of the following is a soluble, strong base? - PowerPoint PPT Presentation


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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.

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slide3
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
slide4

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
the ph of a solution is 4 80 what is the concentration of hydroxide ions in this solution
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
we add enough acid to a solution to cause the ph to decrease from 6 5 to 5 5 this means that
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.
slide8

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
calculate the original molarity of a solution of acetic acid that is 3 0 ionized k a 1 8 x 10 5
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
slide11

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%
slide13

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
what is the value of the base hydrolysis constant for nabo 2 sodium metaborate
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
calculate the h 3 o in a 0 20 m kcn solution
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
the hydrolysis constant that would be used to calculate the ph in nh 4 cl solution is given by
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)