Question

Like sulfuric acid, selenic acid (H2SeO4) is a diprotic acid
that has a very large value of *K*a1.

Part A:

Calculate the pH in 0.20 M H2SeO4 (*K*a2=1.2×10−2).
Answer found to be 0.68

Part B

Calculate the concentration of H3O+.

Part C

Calculate the concentration of H2SeO4.

Part D

Calculate the concentration of HSeO−4.

Part E

Calculate the concentration of SeO2−4.

Part F

Calculate the concentration of OH−.

I need help with B-F

Answer #1

Oxalic acid, found in the leaves of rhubarb and other plants, is
a diprotic acid.
H2C2O4 + H2O ↔ H3O+ + HC2O4-
Ka1= ?
HC2O4- + H2O ↔ H3O+ + C2O42-
Ka2 = ?
An aqueous solution that is 1.05 M H2C2O4 has pH = 0.67. The
free oxalate ion concentration in this solution is [C2O42-] = 5.3 x
10-5 M. Determine Ka1 and Ka2 for oxalic acid.

A diprotic acid, H2A, has acid dissociation constants of Ka1 =
3.48× 10–4 and Ka2 = 3.21× 10–12. Calculate the pH and molar
concentrations of H2A, HA–, and A2– at equilibrium for each of the
solutions below.(a) a 0.153 M solution of H2A.(b) a 0.153 M
solution of NaHA.(c) a 0.153 M solution of Na2A

given a diprotic acid, H2A, with two ionization
constants of Ka1 = 1.6×10^-4 and Ka2 = 5.2×10^-11, calculate the ph
for a .206 M solution of NaHA

A sample of a diprotic weak acid (H2A) was titrated with 0.0500M
NaOH (a strong base) The initial acid solution had a concentration
of 0.0250M and had a volume of 50.0mL. For the acid Ka1=1.0*10-3
and Ka2=1.0*10-6.
a) calculate Ve1 and Ve2
b) Calculate the pH after 40.0mL of NaOH was added
c)Calculate the pH after 40.0mL of NaOH was added

Calculate the pH of 0.15 M H2SO4(aq) at 25◦C, given that Ka1 is
very large and Ka2 = 1.2 × 10−2

An 80.9 mL sample of a 0.100 M solution of a diprotic acid, H2A,
is titrated with 0.100 M KOH. For H2A, Ka1 = 8.09 x 10^-5 and Ka2 =
8.09 x 10^-10. A) Calculate the concentration of A2- prior to the
addition of any KOH. B) What is the pH of the initial solution? C)
What is the pH exactly halfway to the first equivalence point? D)
What is the pH exactly halfway between the first and second
equivalence...

To learn how to calculate ion concentrations in an aqueous
solution of a strong diprotic acid.
Sulfuric acid, H2SO4, is a strong acid. Its complete
dissociation in aqueous solution is represented as
H2SO4?H++HSO4?
A HSO4? anion can dissociate further by
HSO4??H++SO42?
but the extent of dissociation is considerably less than 100%.
The equilibrium constant for the second dissociation step is
expressed as
Ka2=[H+][SO42?][HSO4?]=0.012
Part A
Calculate the concentration of H+ ions in a 0.010 M
aqueous solution of sulfuric acid....

For the diprotic weak acid H2A, Ka1 = 2.8 × 10-6 and Ka2 = 6.4 ×
10-9.
What is the pH of a 0.0450 M solution of H2A?
What are the equilibrium concentrations of H2A and A2– in this
solution?
Please show work ? I Have no idea how to do these types of
problems.

Calculate the concentration of H2SO4, HSO4-, SO4-2 and H+ ions in a
0.17 M sulfuric acid solution. Assume H+ and H3O+ to be the same
ions. Ka2 = 1.3 x 10^-2.

22.0 mL of 0.128 M diprotic acid (H2A) was titrated with 0.1017
M KOH. The acid ionization constants for the acid are
Ka1=5.2×10−5and Ka2=3.4×10−10.
Part A
At what added volume of base does the first equivalence point
occur?
Part B
At what added volume of base does the second equivalence point
occur?

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