Question

The pH of a 9.94×10-4 M solution of a weak base is 8.54. Calculate Kb for this base to three significant figures.

Answer #1

Calculate the pH of a 0.0786 M aqueous solution of the weak base
caffeine (C8H10N4O2, Kb = 4.10×10-4). pH Calculate the pH of a
0.0786 M aqueous solution of the weak base
caffeine
(C8H10N4O2,
Kb = 4.10×10-4).
pH =

Calculate the pH of a weak base solution ([B]0 >
100 • Kb
Calculate the pH of a 0.106 M aqueous solution of
triethanolamine (C6H15O3N, Kb = 5.8×10-7) and the equilibrium
concentrations of the weak base and its conjugate acid.

A 0.150 M solution of a weak base has a pH of 11.28. Determine
the Kb for the base. Express your answer using two significant
figures.

A 1.70 M solution of a weak base has a pH of 9.7. Calculate the
Kb.

A 1.70 M solution of a weak base has a pH of 9.7. Calculate the
Kb.

Calculate the pH of a 0.0416 M aqueous solution of ethylamine
(C2H5NH2, Kb = 4.3×10-4) and the equilibrium concentrations of the
weak base and its conjugate acid.
pH
=
[C2H5NH2]equilibrium
=
M
[C2H5NH3+
]equilibrium
=

If the Kb of a weak base is 2.8 × 10-6, what is the pH of a 0.30
M solution of this base?

If the Kb of a weak base is 1.2 × 10-6, what is the pH of a 0.32
M solution of this base?

If the Kb of a weak base is 5.2 × 10-6, what is the pH of a 0.12
M solution of this base?

If the Kb of a weak base is 7.5 × 10-6, what is the pH of a 0.33
M solution of this base?

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