In this problem, we will use material balance and chacepts (pages 761-762) to calculate the equilibrium concentrations in an extremely dilute solution of a strong acid, 1.0 × 10 − 7 MHCl ( aq ) . (a) Write down the material balance equation for 1.0 × 10 − 7 MHCl(aq), assuming that HCl ionizes completely in aqueous solution. (b) Write down the charge balance equation (an electroneutrality condition) for this solution. (c) Use the material balance and charge balance equations, and product for water, K z = [ H 2 O - ] [ OH - ] , to show that [ H 2 O - ] -c 2 [ H 2 O+ ] -K c = 0 , where c o = 1.0 × 10 − 7 M . (d) Use the quadratic formula to solve equation in (c) [ H 2 O − ] . (e) Calculate [ OH - ] and compare this value with [ Cl - ] . What conclusion can you draw from this comparison?
In this problem, we will use material balance and chacepts (pages 761-762) to calculate the equilibrium concentrations in an extremely dilute solution of a strong acid, 1.0 × 10 − 7 MHCl ( aq ) . (a) Write down the material balance equation for 1.0 × 10 − 7 MHCl(aq), assuming that HCl ionizes completely in aqueous solution. (b) Write down the charge balance equation (an electroneutrality condition) for this solution. (c) Use the material balance and charge balance equations, and product for water, K z = [ H 2 O - ] [ OH - ] , to show that [ H 2 O - ] -c 2 [ H 2 O+ ] -K c = 0 , where c o = 1.0 × 10 − 7 M . (d) Use the quadratic formula to solve equation in (c) [ H 2 O − ] . (e) Calculate [ OH - ] and compare this value with [ Cl - ] . What conclusion can you draw from this comparison?
Solution Summary: The author explains the material balance equation for given concentration of hydrochloric acid.
In this problem, we will use material balance and chacepts (pages 761-762) to calculate the equilibrium concentrations in an extremely dilute solution of a strong acid,
1.0
×
10
−
7
MHCl
(
aq
)
.
(a) Write down the material balance equation for
1.0
×
10
−
7
MHCl(aq), assuming that HCl ionizes completely in aqueous solution.
(b) Write down the charge balance equation (an electroneutrality condition) for this solution.
(c) Use the material balance and charge balance equations, and product for water,
K
z
=
[
H
2
O
-
]
[
OH
-
]
, to show that
[
H
2
O
-
]
-c
2
[
H
2
O+
]
-K
c
=
0
, where
c
o
=
1.0
×
10
−
7
M
.
(d) Use the quadratic formula to solve equation in (c)
[
H
2
O
−
]
.
(e) Calculate
[
OH
-
]
and compare this value with
[
Cl
-
]
. What conclusion can you draw from this comparison?
Propionic acid, HC3H5O2, has Ka= 1.34 x 10–5.
(a) What is the molar concentration of H3O+ in 0.15 M HC3H5O2 and the pH of the solution?
(b) What is the Kb value for the propionate ion, C3H5O2–?
(c) Calculate the pH of 0.15 M solution of sodium propionate, NaC3H5O2.
(d) Calculate the pH of solution that contains 0.12 M HC3H5O2 and 0.25 M NaC3H5O2.
Calculate the change in pH when 7.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH3(aq) and 0.100 M in NH4Cl(aq). Consult the table of ionization constants as needed.
ΔpH=
Calculate the change in pH when 7.00 mL of 0.100 M NaOH is added to the original buffer solution.
ΔpH=
The ionization constant Ka, for HCN(aq) is 4.3 x 10^-10. What is the pH of a 0.22 molar solution of sodium cyanide, which contains the cyanide ion?
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