Question

If the pH of a 1.00-in. rainfall over 1300 miles2 is 3.30, how many kilograms of sulfuric acid, H2SO4, are present, assuming that it is the only acid contributing to the pH?

For sulfuric acid, *K*a1 is very large and *K*a2
is 0.012.

Answer #1

Volume of rainfall = Area X height

Height = 1 in = 0.254 dm

1mile2 = 2.59 X 10^8 dm^2

so 1300 miles^2 = 3367 X 10^8 dm^2

Volume = 0.254 X 3367 X 10^8 = 855.218 X 10^8 dm^3

Also,

H_{2}SO_{4} ionizes as

H2SO4 --> H+ + HSO4-

Ka1 is very high so it completely dissociates , due to first dissociation [H+] = Concentraion of H2SO4

HSO4- --> H^{+} + SO4^{-2}

We also consider it as high dissciation

so each mole of H2SO4 will give 2 moles of H+ (proton)

pH = 3.30 = -log[H+]

So [H+] = 0.000501 M = 0.000501 moles / L or moles / dm^3

Volume = 855.218 X 10^8 dm^3

so moles of H+ present in this volume = 0.000501 X 855.218 X 10^8 = 4.28 X 10^7 moles

So moles of H2SO4 = 4.28 X 10^7 / 2 = 2.14 X 10^7 moles

Molecular weight of H2SO4 = 98 g / mole

so mass of H2SO4 = Moles X molecular weight = 98 x 2.14 X 10^7
grams = 209.72 X 10^7 grams = **2.09 X 10^6 Kg**

If the pH of a 1.00-in. rainfall over 1500 miles2 is 3.30, how
many kilograms of sulfuric acid, H2SO4, are present, assuming that
it is the only acid contributing to the pH? For sulfuric acid, Ka1
is very large and Ka2 is 0.012.

Part A
If the pH of a 1.00-in. rainfall over 1800 miles2 is 3.30, how
many kilograms of sulfuric acid, H2SO4, are present, assuming that
it is the only acid contributing to the pH?
For sulfuric acid, Ka1 is very large and Ka2
is 0.012.

If the pH of a 1.00-in. rainfall over 1700 miles2 is 3.70, how
many kilograms of sulfuric acid, H2SO4, are present, assuming that
it is the only acid contributing to the pH?
For sulfuric acid, Ka1 is very large and Ka2
is 0.012.

If the pH of a 1.00-in. rainfall over 1400 miles2 is 3.90, how
many kilograms of sulfuric acid, H2SO4, are present, assuming that
it is the only acid contributing to the pH? For sulfuric acid, Ka1
is very large and Ka2 is 0.012.

f the pH of a 1.00-in. rainfall over 1600 miles2 is 3.60, how
many kilograms of sulfuric acid, H2SO4, are present, assuming that
it is the only acid contributing to the pH? For sulfuric acid, Ka1
is very large and Ka2 is 0.012.

Part A
If the pH of a 1.00-in . rainfall over 1700 miles2 is 3.90, how
many kilograms of sulfuric acid, H2SO4 , are present, assuming that
it is the only acid contributing to the pH ?
For sulfuric acid, Ka1 is very large and Ka2
is 0.012.

If the pH of a 1.00-in. rainfall over 1500 miles2 is 3.90, how
many kilograms of sulfuric acid, H2SO4, are present, assuming that
it is the only acid contributing to the pH? For sulfuric acid, Ka1
is very large and Ka2 is 0.012.
I keep following the steps from similar problems with different
values and its still wrong.
Can you please solve step by step.

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

How many of the following responses are true?
1. The % dissociation of H3PO4 is lower
than that of a strong acid because Ka1, Ka2,
and Ka3 are all less than 1
2. Acetic acid is a weak acid and will dissociate completely in
water
3. HCl is a strong acid and will dissociate completely in
water
4. When dissolved in water, only the first two dissociations of
H3PO4 will both produce a significant amount
of the H+ ion
5....

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