Question

Equal volumes of 0.120 M weak base (Kb = 5.0× 10–9) and 0.120 M HCl are mixed. Calculate the pH of the resulting solution.

Answer #1

if both are equal volume

then 0.12 / 2 = **0.06 M s**alt will form

it is a salt of weak base and strong acid.

for such salts pH = 1/2 (pKw - pKb - log C)

Kb = 5.0 x 10^{-9}

pKb = -log (5.0 x 10^{-9})

pKb = 8.3

pH = 1/2 (14 - 8.3 - log 0.06)

**pH = 3.46**

Equal volumes of 0.190 M weak base (Kb = 2.0× 10–9) and 0.190 M
HCl are mixed. Calculate the pH of the resulting solution.

A 0.120 M solution of a weak base has a pH of
11.27.
Part A
Determine Kb for the base.

During the titration of 25.00 mL of 0.130 M weak base NH3 (Kb =
1.8 x 10^-5) with 0.100 M HCl, calculate the pH of the solution at
the following volumes of acid added:
a) 10.00 mL
b) 32.50 mL
c) 50.00 mL

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 =

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.

Equal volumes of 0.1 M NH3 (Kb= 1.8x10^-5) and 0.1 M HCN (Ka=
4.9x10^-10) are mixed together. will the resulting solution be
acidic, basic, or neutral? PLEASE SHOW WORK

1.) If a buffer solution is 0.110 M in a weak base (Kb = 5.7 ×
10-5) and 0.590 M in its conjugate acid, what is the pH?
2.) You need to prepare 100.0 mL of a pH=4.00 buffer solution
using 0.100 M benzoic acid (pKa = 4.20) and 0.240 M sodium
benzoate. How much of each solution should be mixed to prepare this
buffer?
3.) Calculate the change in pH when 6.00 mL of 0.100 M HCl(aq)
is added...

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?

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