Question

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.

Answer #1

Since H_{2}SO_{4} is a strong acid.
So, it will dissociate completely as per the following equation

H_{2}SO_{4}
H^{+} + HSO_{4}^{-}

Now, as we have 0.17M H_{2}SO_{4} is
here, [H^{+}] and
[HSO_{4}^{-}] will both be equal to 0.17M.

But HSO_{4}^{-} is a weak acid and it dissociate
as per the following reaction:

HSO_{4}^{-}
H^{+} + SO_{4}^{2-} having K_{a} =
1.3 x 10^{-2}

Final Concentration 0.17-x x x

So, we have K_{a} = x^{2}/
(0.17-x)

1.3 x 10^{-2} = x^{2}/ (0.17-x)

So, x^{2} + 0.013x - 0.00221 = 0

Solving this quadratic equation for x, we get x = 0.0409

So, we have **[SO _{4}^{2-}] =
0.0409M**

**[HSO _{4}^{-}] =** 0.17 - 0.0409

**[H _{2}SO_{4}] = 0**

**[H ^{+}] =** 0.17 + 0.0409

Be sure to answer all
parts.
Calculate the concentrations of H2SO4,
HSO4−, SO42− and
H3O+ ions in a 0.15 M sulfuric acid solution at
25°C (Ka2
for sulfuric acid is
1.3 ×
10−2.)
[H2SO4]
M
[HSO4−]
M
[SO42−]
M
[H3O+]

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....

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....

What are the concentrations of HSO4−, SO42−, and H+ in a 0.25 M
KHSO4 solution? (Hint: H2SO4 is a strong acid; Ka for HSO4− = 1.3 ×
10−2.) [ HSO4− ] = M [ SO42− ] = M [ H+ ] = M

What are the concentrations of HSO4−, SO42−, and H+ in a 0.21 M
KHSO4 solution? (Hint: H2SO4 is a strong acid; Ka for HSO4− = 1.3 ×
10−2.)

1) What is the ph of a 0.005 M , solution of h2so4?
ka2=1.2x10^-2 of HSo4-

The lead storage batteries used in automobiles have a sulfuric
acid (H2SO4) concentration of 3.75 M. The density of the sulfuric
acid solution is 1.230 g/mL and the molar mass of sulfuric acid is
98.08 g/mol.

The lead storage batteries used in automobiles have a sulfuric
acid (H2SO4) concentration of 3.75 M. The density of the sulfuric
acid solution is 1.230 g/mL and the molar mass of sulfuric acid is
98.08 g/mol. What is molality of sulfuric acid?

Calculate the concentrations of
H2C2O4,
HC2O4−,
C2O42−,
and H+ ions in a 0.193
M oxalic acid solution at 25
°C. (Ka1
= 6.5 × 10−2
and Ka2 =
6.1 ×10−5 for oxalic
acid.) (Enter your answer in scientific notation.)

1. Calculate the [H+]-, [HSO4-]- and [SO 42-] - ion
concentrations and the pH of a 0.050 M H2SO4. Ka1 is very large and
Ka2 is 0.012.
2. Write equations to show how you would make:
a) NaHSO4
b) Na2SO4
c) NaHCO3

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