Determine the concentrations of the ionic species present in a
0.268 M solution of the
NaO2CCOCH2CO2Na.
(pKa1=3.40, pKa2=5.11 for
HO2CCOCH2CO2H).
a) [HO2CCOCH2CO2H]
b)[HO2CCOCH2CO2-]
c)
[-O2CCOCH2CO2-]
d) [H3O+]
e) [OH-]
Determine the concentrations of the following ionic species
present in a 0.296 M solution of Na2SO3. For
H2SO3, Ka1 = 1.4E-2,
Ka2 = 6.3E-8.
a) What is the OH- ion concentration?
b) What is the HSO3- ion
concentration?
c) What is the SO32- ion
concentration?
calculate the concentrations of all species present at
equilibrium for a .200M solution of sodium arsenate, Na3AsO4. (
Don't forget the hydrolysis reactions of the arsenate ion)
What are the equilibrium concentrations of all the solute
species in a 0.92 M solution of phenol,
HC6H5O?
(a) [H3O+], M;
(b) [OH-], M;
(c) [HC6H5O], M;
(d) What is the pH of the solution? For
HC6H5O, Ka = 1.3 x
10-10.
Calculate the pH of a 5.0 M H3PO4 solution
and the equilibrium concentrations of the species
H3PO4,
H2PO4-,
HPO42- and PO43- (ka1 =
7.5 x 10-3, ka2 = 6.2 x 10-8, ka3 = 4.8 x
10-13)
Calculate the concentrations of all the species in a
0.301 M
Na2CO3
solution.
[CO32−]
= M
[Na+] = M
[HCO3−] = M
[OH−] = M
[H2CO3] = × 10
M
(Enter your answer in scientific notation.)
[H+] = × 10 M
(Enter your answer in scientific notation.)
Part A
Calculate the pH and the concentrations of all species present
in 0.16 M H2SO3. (Ka1 = 1.5×10−2, Ka2 =
6.3×10−8)
Express your answer to three significant figures and include the
appropriate units.
pH =
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Part B
Calculate the concentration of H2SO3 in solution.
Express your answer to two significant figures and include the
appropriate units.
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Part C
Calculate the concentration...
Calculate the concentrations of all the species in a
0.487 M
Na2CO3
solution. For
H2CO3,
Ka1 = 4.2 ×10−7
and Ka2 =
4.8
×10−11.
[CO32−]
= M
[Na+] = M
[HCO3−] = M
[OH−] = M
[H2CO3] = M
(Enter your answer in scientific notation.)
[H+] = M
(Enter your answer in scientific notation.)