For nitrous acid, HNO2, the value of Ka is 4.0 x 10-4.
a. What is the formula of the conjugate base of HNO2?
b. What is the pH of a 0.250 M solution of this weak acid
HNO2?
Nitrous acid, HNO2, has a Ka of 7.1 x 10-4. What are (H3O+),
(NO2-), and (OH-) in 0.700M HNO2?
a) (H3O+)=.........M…………………………answer a in M
b)) (NO2-)=..........M…………………………answer b in M
c) (OH-)..............x 10 .......M...........(
answer c in scientific notation)
Given the following information:
nitrous acid
HNO2
Ka = 4.5×10-4
hydrocyanic acid
HCN
Ka = 4.0×10-10
(1) Write the net ionic equation for the reaction
that occurs when equal volumes of 0.242
M aqueous nitrous acid and
sodium cyanide are mixed. It is
not necessary to include states such as (aq) or (s).
_____
+
_____
_____
+
_____
(2) At equilibrium the
_________(reactants/products) will be favored.
(3) The pH of the resulting solution will be
_________(greater than/equal to/less than)...
Consider the reaction of nitrous acid in water where Ka =
4.0 ✕ 10−4. HNO2(aq) + H2O(l) equilibrium reaction arrow NO2−(aq) +
H3O+(aq) (a) Which two bases are competing for the proton? (Select
all that apply.) HNO2 H2O NO2− H3O+ (b) Which is the stronger base?
HNO2 H2O NO2− H3O+ (c) In light of your answer to (b), why do we
classify the nitrite ion (NO2−) as a weak base? The nitrite ion is
a (stronger or weaker) base than...
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
Given the following information: nitrous acid = HNO2 hydrocyanic
acid = HCN HNO2 is a stronger acid than HCN (1) Write the net ionic
equation for the reaction that occurs when equal volumes of 0.080 M
aqueous nitrous acid and sodium cyanide are mixed. It is not
necessary to include states such as (aq) or (s). + + (2) Which is
the strongest base, NO2- or CN- ? (3) At equilibrium the what will
be favored?
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