Calculate the pH of a 0.0152 M aqueous solution
of nitrous acid (HNO2,
Ka = 4.6×10-4) and the
equilibrium concentrations of the weak acid and its conjugate
base.
pH
=
[HNO2]equilibrium
=
M
[NO2-
]equilibrium
=
M
Determine the pH during the titration of 24.8
mL of 0.475 M nitrous acid
(Ka = 4.5×10-4) by
0.361 M NaOH at the following
points.
(a) Before the addition of any NaOH
__________
(b) After the addition of 8.20 mL of
NaOH __________
(c) At the half-equivalence point (the titration midpoint)
________
(d) At the equivalence point __________
(e) After the addition of 48.9 mL of
NaOH __________
Calculate the hydronium ion concentration in 0.120 M
nitrous acid. ka( nitrous acid) =7.1x10^4. Use the ICE method to
determone concentration of H3O+ = 9.23 x10^—3
Find the pH during the titration of 20.00 mL of 0.1000 M nitrous
acid, HNO2 (Ka = 7.1 10-4), with 0.1000 M NaOH solution after the
following additions of titrant. Find at volumes of 0 mL, 10.00 mL,
15.00 mL, 20.00 mL, and 25.00 mL.
Find the pH during the titration of 20.00 mL of 0.2300 M nitrous
acid, HNO2 (Ka = 7.1 ✕ 10-4), with 0.2300 M NaOH solution after the
following additions of titrant. a) 0mL b)10.00mL c) 15.00mL d)
19.00mL e)19.95 mL f) 20.00mL g) 20.05mL h) 25.00mL
Find the pH during the titration of 20.00 mL of 0.1820 M nitrous
acid, HNO2 (Ka = 7.1 ✕ 10-4), with 0.1820 M NaOH solution after the
following additions of titrant. (
a) 0 mL
(b) 10.00 mL
(c) 15.00 mL
(d) 19.00 mL
(e) 19.95 mL
(f) 20.00 mL
(g) 20.05 mL
(h) 25.00 mL
Find the pH during the titration of 20.00 mL of 0.1590 M nitrous
acid, HNO2 (Ka = 7.1 ✕ 10-4), with 0.1590 M NaOH solution after the
following additions of titrant. (a) 0 mL (b) 10.00 mL (c) 15.00 mL
(d) 19.00 mL (e) 19.95 mL (f) 20.00 mL (g) 20.05 mL (h) 25.00
mL
Calculate the pH of .346 M aqueous solution hydrocyanic acid HCN,
Ka=4.0x10^-10 and the equilibrium concentrations of the weak acid
and it’s conjugate base
pH=
HCN equilibrium=
CN-=
Calculate the pH of a .0169 M aqueous solution of hydro
fluoric acid HF, Ka=6.6x10^-4 and the equilibrium concentrations of
the weak acid and it’s conjugate base
pH=
HF equilibrium=
F-=